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Potassium chloride
Potassium chloride
Potassium chloride
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Potassium chloride
Names
Other names
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.028.374 Edit this at Wikidata
E number E508 (acidity regulators, ...)
KEGG
RTECS number
  • TS8050000
UNII
  • InChI=1S/ClH.K/h1H;/q;+1/p-1 checkY
    Key: WCUXLLCKKVVCTQ-UHFFFAOYSA-M checkY
  • InChI=1/ClH.K/h1H;/q;+1/p-1
    Key: WCUXLLCKKVVCTQ-REWHXWOFAZ
  • [Cl-].[K+]
Properties
KCl
Molar mass 74.555 g·mol−1
Appearance white crystalline solid
Odor odorless
Density 1.984 g/cm3
Melting point 770 °C (1,420 °F; 1,040 K)
Boiling point 1,420 °C (2,590 °F; 1,690 K)
27.77 g/100mL (0 °C)
33.97 g/100mL (20 °C)
54.02 g/100mL (100 °C)
Solubility Soluble in glycerol, alkalies
Slightly soluble in alcohol Insoluble in ether[1]
Solubility in ethanol 0.288 g/L (25 °C)[2]
Acidity (pKa) ~7
−39.0·10−6 cm3/mol
1.4902 (589 nm)
Structure
face centered cubic
Fm3m, No. 225
a = 629.2 pm[3]
Octahedral (K+)
Octahedral (Cl−)
Thermochemistry
83 J·mol−1·K−1[4]
−436 kJ·mol−1[4]
Pharmacology
A12BA01 (WHO) B05XA01 (WHO)
Oral, IV, IM
Pharmacokinetics:
Kidney: 90%; Fecal: 10%[5]
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
2600 mg/kg (oral, rat)[6]
Safety data sheet (SDS) ICSC 1450
Related compounds
Other anions
 Potassium fluoride
Potassium bromide
Potassium iodide
Other cations
 Lithium chloride
Sodium chloride
Rubidium chloride
Caesium chloride
Ammonium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Potassium chloride (KCl, or potassium salt) is a metal halide salt composed of potassium and chlorine. It is odorless and has a white or colorless vitreous crystal appearance. The solid dissolves readily in water, and its solutions have a salt-like taste. Potassium chloride can be obtained from ancient dried lake deposits.[7] KCl is used as a salt substitute for table salt (NaCl), a fertilizer,[8] as a medication, in scientific applications, in domestic water softeners (as a substitute for sodium chloride salt), as a feedstock, and in food processing, where it may be known as E number additive E508.

It occurs naturally as the mineral sylvite, which is named after salt's historical designations sal degistivum Sylvii and sal febrifugum Sylvii,[9] and in combination with sodium chloride as sylvinite.[10]

Uses

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Fertilizer

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Potassium chloride, compacted, fertilizer grade

The majority of the potassium chloride produced is used for making fertilizer, called potash, since the growth of many plants is limited by potassium availability.[11][12] The term "potash" refers to various mined and manufactured salts that contain potassium in water-soluble form. Potassium chloride sold as fertilizer is known as "muriate of potash"—it is the common name for potassium chloride (KCl) used in agriculture.[13][14][15][16] The vast majority of potash fertilizer worldwide is sold as muriate of potash.[17][18] The dominance of muriate of potash in the fertilizer market is due to its high potassium content (approximately 60% K
2O equivalent) and relative affordability compared to other potassium sources like sulfate of potash (potassium sulfate).[16][19] Potassium is one of the three primary macronutrients essential for plant growth, alongside nitrogen and phosphorus. Potassium plays a vital role in various plant physiological processes, including enzyme activation, photosynthesis, protein synthesis, and water regulation.[20][21] For watering plants, a moderate concentration of potassium chloride (KCl) is used to avoid potential toxicity: 6 mM (millimolar) is generally effective and safe for most plants, which is approximately 0.4 grams (0.014 oz) per liter of water.[22][23]

Medical use

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Main article: Potassium chloride (medical use)

Potassium is vital in the human body, and potassium chloride by mouth is the standard means to treat low blood potassium, although it can also be given intravenously. It is on the World Health Organization's List of Essential Medicines.[24] It is also an ingredient in Oral Rehydration Therapy (ORT)/solution (ORS) to reduce hypokalemia caused by diarrhoea,[25] which is also on the WHO's List of Essential Medicines.[24]

Potassium chloride contains 52% of elemental potassium by mass.[26]

Overdose causes hyperkalemia which can disrupt cell signaling to the extent that the heart will stop, reversibly in the case of some open heart surgeries.[27][28][29]

Culinary use

[edit]

Potassium chloride can be used as a salt substitute for food, but because not everyone likes its flavor, it is often mixed with ordinary table salt (sodium chloride) to improve the taste, to form low sodium salt. The addition of 1 ppm of thaumatin considerably reduces this bitterness.[30] Complaints of bitterness or a chemical or metallic taste are also reported with potassium chloride used in food.[31]

The World Health Organization guideline Use of lower-sodium salt substitutes strongly recommends reducing sodium intake to less than 2 g/day and conditionally recommends replacing regular table salt with lower-sodium salt substitutes that contain potassium. This recommendation is intended for adults (not pregnant women or children) in general populations, excluding individuals with kidney impairments or with other circumstances or conditions that might compromise potassium excretion.[32][33][34]

Execution

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In the United States, potassium chloride is used as the final drug in the three-injection sequence of lethal injection as a form of capital punishment. It induces cardiac arrest, ultimately killing the person.[35]

Industrial

[edit]

As a chemical feedstock, the salt is used for the manufacture of potassium hydroxide and potassium metal. It is also used in medicine, lethal injections, scientific applications, food processing, soaps, and as a sodium-free substitute for table salt for people concerned about the health effects of sodium.[citation needed]

It is used as a supplement in animal feed to boost the potassium level in the feed. As an added benefit, it is known to increase milk production.[citation needed]

It is sometimes used in solution as a completion fluid in petroleum and natural gas operations, as well as being an alternative to sodium chloride in household water softener units.[citation needed]

Glass manufacturers use granular potash as a flux, lowering the temperature at which a mixture melts. Because potash imparts excellent clarity to glass, it is commonly used in eyeglasses, glassware, televisions, and computer monitors.[citation needed]

Because natural potassium contains a tiny amount of the isotope potassium-40, potassium chloride is used as a beta radiation source to calibrate radiation monitoring equipment. It also emits a relatively low level of 511 keV gamma rays from positron annihilation, which can be used to calibrate medical scanners.[citation needed]

Potassium chloride is used in some de-icing products designed to be safer for pets and plants, though these are inferior in melting quality to calcium chloride. It is also used in various brands of bottled water.[citation needed]

Potassium chloride was once used as a fire extinguishing agent, and in portable and wheeled fire extinguishers. Known as Super-K dry chemical, it was more effective than sodium bicarbonate-based dry chemicals and was compatible with protein foam. This agent fell out of favor with the introduction of potassium bicarbonate (Purple-K) dry chemical in the late 1960s, which was much less corrosive, as well as more effective. It is rated for B and C fires.[citation needed]

Along with sodium chloride and lithium chloride, potassium chloride is used as a flux for the gas welding of aluminium.[citation needed]

Potassium chloride is also an optical crystal with a wide transmission range from 210 nm to 20 μm. While cheap, KCl crystals are hygroscopic. This limits its application to protected environments or short-term uses such as prototyping. Exposed to free air, KCl optics will "rot". Whereas KCl components were formerly used for infrared optics, they have been entirely replaced by much tougher crystals such as zinc selenide.[citation needed]

Potassium chloride is used as a scotophor with designation P10 in dark-trace CRTs, e.g. in the Skiatron.[citation needed]

Toxicity

[edit]

The typical amounts of potassium chloride found in the diet appear to be generally safe.[36] In larger quantities, however, potassium chloride is toxic. The LD50 of orally ingested potassium chloride is approximately 2.5 g/kg, or 190 grams (6.7 oz) for a body mass of 75 kilograms (165 lb). In comparison, the LD50 of sodium chloride (table salt) is 3.75 g/kg.

Intravenously, the LD50 of potassium chloride is far smaller, at about 57.2 mg/kg to 66.7 mg/kg; this is found by dividing the lethal concentration of positive potassium ions (about 30 to 35 mg/kg)[37] by the proportion by mass of potassium ions in potassium chloride (about 0.52445 mg K+/mg KCl).[38]

Chemical properties

[edit]

Solubility

[edit]

KCl is soluble in a variety of polar solvents.

Solubility[39]
Solvent Solubility
(g/kg of solvent at 25 °C)
Water 360
Liquid ammonia 0.4
Liquid sulfur dioxide 0.41
Methanol 5.3
Ethanol 0.37
Formic acid 192
Sulfolane 0.04
Acetonitrile 0.024
Acetone 0.00091
Formamide 62
Acetamide 24.5
Dimethylformamide 0.17–0.5

Solutions of KCl are common standards, for example for calibration of the electrical conductivity of (ionic) solutions, since KCl solutions are stable, allowing for reproducible measurements. In aqueous solution, it is essentially fully ionized into solvated K+ and Cl− ions.

Redox and the conversion to potassium metal

[edit]

Although potassium is more electropositive than sodium, KCl can be reduced to the metal by reaction with metallic sodium at 850 °C because the more volatile potassium can be removed by distillation (see Le Chatelier's principle):

KCl(l) + Na(l) ⇌ NaCl(l) + K(g)

This method is the main method for producing metallic potassium. Electrolysis (used for sodium) fails because of the high solubility of potassium in molten KCl.[10]

Other potassium chloride stoichiometries

[edit]

Potassium chlorides with formulas other than KCl have been predicted to become stable under pressures of 20 GPa or more.[40] Among these, two phases of KCl3 were synthesized and characterized. At 20-40 GPa, a trigonal structure containing K+ and Cl3− is obtained; above 40 GPa this gives way to a phase isostructural with the intermetallic compound Cr3Si.[citation needed]

Physical properties

[edit]

Under ambient conditions, the crystal structure of potassium chloride is like that of NaCl. It adopts a face-centered cubic structure known as the B1 phase with a lattice constant of roughly 6.3 Å. Crystals cleave easily in three directions. Other polymorphic and hydrated phases are adopted at high pressures.[41]

Some other properties are

  • Transmission range: 210 nm to 20 μm
  • Transmittivity = 92% at 450 nm and rises linearly to 94% at 16 μm
  • Refractive index = 1.456 at 10 μm
  • Reflection loss = 6.8% at 10 μm (two surfaces)
  • dN/dT (expansion coefficient)= −33.2×10−6/°C
  • dL/dT (refractive index gradient)= 40×10−6/°C
  • Thermal conductivity = 0.036 W/(cm·K)
  • Damage threshold (Newman and Novak): 4 GW/cm2 or 2 J/cm2 (0.5 or 1 ns pulse rate); 4.2 J/cm2 (1.7 ns pulse rate Kovalev and Faizullov)

As with other compounds containing potassium, KCl in powdered form gives a lilac flame.

Production

[edit]
Sylvite
Sylvinite

Potassium chloride is extracted from minerals sylvite, carnallite, and potash. It is also extracted from salt water and can be manufactured by crystallization from solution, flotation or electrostatic separation from suitable minerals. It is a by-product of the production of nitric acid from potassium nitrate and hydrochloric acid.

Most potassium chloride is produced as agricultural and industrial-grade potash in Saskatchewan, Canada, Russia, and Belarus. Saskatchewan alone accounted for over 25% of the world's potash production in 2017.[42]

Laboratory methods

[edit]

Potassium chloride is inexpensively available and is rarely prepared intentionally in the laboratory. It can be generated by treating potassium hydroxide (or other potassium bases) with hydrochloric acid:

KOH + HCl → KCl + H2O

This conversion is an acid-base neutralization reaction. The resulting salt can then be purified by recrystallization. Another method would be to allow potassium to burn in the presence of chlorine gas, also a very exothermic reaction:

2 K + Cl2 → 2 KCl

References

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Further reading

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[edit]
Revisions and contributorsEdit on WikipediaRead on Wikipedia

Potassium chloride

View on Grokipedia
from Grokipedia
is an ionic with the molecular formula KCl, consisting of cations and anions in a 1:1 ratio, manifesting as a or colorless crystalline solid at . This highly water-soluble salt occurs naturally as the mineral , often extracted from underground deposits mixed with . Primarily, it serves as a key ingredient, providing essential for crop nutrition, which enhances plant resistance to stress, improves water use efficiency, and boosts yields, accounting for the majority of its global production. In medicine, is administered to correct , a condition of low blood levels that can arise from diuretics, vomiting, or inadequate intake, thereby preventing cardiac arrhythmias and . Beyond and healthcare, it functions as a in low-sodium diets due to its similar taste profile to , and in industrial contexts for buffer solutions and replenishment.

Properties

Physical properties


Potassium chloride (KCl) appears as a colorless or white crystalline solid at and standard , often forming cubic that cleave easily along three orthogonal planes. It adopts a face-centered cubic (FCC) lattice, characteristic of the rock salt structure, with potassium cations and chloride anions arranged in an alternating octahedral coordination and a lattice parameter of 6.293 Å at ambient conditions. The compound has a of 1.984 g/cm³ at 25 °C. Its is 770 °C, and the is 1420 °C under standard pressure. Potassium chloride is highly soluble in , with a of 34.2 g per 100 mL at 20 °C, and this solubility increases markedly with , reaching approximately 54 g/100 mL at 100 °C.
PropertyValue
Density (25 °C)1.984 g/cm³
770 °C
1420 °C
in (20 °C)34.2 g/100 mL
Thermal conductivity (322 )6.53 W/(m·)
KCl is hygroscopic, readily absorbing atmospheric moisture, though it does not deliquesce under typical ambient relative humidities below 75%. Its is negligible at but increases with heat, following parameters derived from effusion measurements at elevated temperatures above 700 °C.

Chemical properties

Potassium chloride (KCl) is an ionic compound consisting of cations (K⁺) and chloride anions (Cl⁻) in a 1:1 stoichiometric ratio. The results from the substantial difference between (0.82) and (3.16 on the Pauling scale), which exceeds 1.7 and favors complete from K to Cl, forming stable ions rather than covalent sharing./09:Ionic_and_Covalent_Solids-_Energetics/9.12:_Lattice_Energies_and_Solubility) This ionic character leads to a rock-salt with strong electrostatic attractions, manifesting as a of approximately 715 kJ/mol. The of KCl in stems from the hydration energies of K⁺ (-322 kJ/mol) and Cl⁻ (-363 kJ/mol) outweighing the , enabling ion separation and by dipoles. In , KCl fully dissociates into its ions without significant , yielding a neutral pH near 7, as both the parent and are strong electrolytes that do not impart acidity or basicity to the salt. Redox behavior of KCl involves the reduction of to metal (standard potential -2.93 V) and oxidation of Cl⁻ to Cl₂ (+1.36 V), requiring substantial electrical energy input for of molten KCl to decompose it, analogous to the process used for , though practical production of potassium favors thermal reduction due to the metal's high reactivity./Electrochemistry/Redox_Potentials/Standard_Potentials) While exotic high-pressure phases may exhibit non-1:1 stoichiometries, standard KCl remains strictly 1:1 with no stable polyhalide forms under ambient conditions.

Occurrence and production

Natural occurrence

Potassium chloride occurs naturally as the mineral , which precipitates from hypersaline brines in sequences during the of ancient marine or lacustrine waters. typically forms late in the evaporation process, after the precipitation of and other more soluble salts, resulting in its association with bedded deposits of these minerals, including sylvinite, a mixture of and . These deposits originated primarily from Permian and basins where restricted circulation and arid climates promoted extreme levels insufficient for modern oceanic settings due to potassium's high and dilution in . Major deposits are concentrated in sedimentary basins such as the Elk Point Basin underlying , , where vast beds in the Formation span thousands of square kilometers. Significant reserves also exist in the Zechstein Basin of , including the historic Stassfurt deposits, as well as in the Solikamsk Basin of and the Pripyat Basin of . These locations account for the bulk of economically viable resources, with global potash resources estimated at approximately 250 billion tonnes, predominantly as potassium chloride-bearing evaporites.

Industrial production

Potassium chloride is primarily produced industrially from sylvinite ores, which consist of (KCl) intermingled with (NaCl), through either conventional underground followed by physical separation or solution mining techniques. In the flotation method, mined sylvinite ore is crushed, ground, and deslimed before being conditioned with in a flotation cell, where air bubbles selectively adhere to sylvite particles due to hydrophobic collectors like fatty amines, allowing potassium chloride to be concentrated in the froth while halite reports to the ; this process achieves efficient separation for ores with sylvite grades typically above 20%. The resulting concentrate undergoes further purification via washing, dissolution in hot water, and recrystallization to yield muriate of (MOP) with purity exceeding 95%. Solution mining, increasingly adopted for deeper deposits, involves injecting hot water (around 100–110°C) into the formation to selectively dissolve , forming a that is pumped to the surface; the is then processed through solar or mechanical followed by cooling , exploiting the temperature-dependent of KCl to precipitate high-purity crystals while NaCl-rich mother liquor to minimize waste. This method reduces surface disruption compared to conventional but requires energy for heating and , with yields optimized by controlling saturation to achieve over 95% KCl purity in the final product. Global production of potassium chloride reached approximately 48 million metric tons in 2024, predominantly as MOP, with major contributions from (over one-third of output), , and via large-scale operations integrating these methods. Recent advancements in Canadian facilities, such as at Mosaic's Esterhazy complex, include investments in efficiency and to lower by up to 10–15% and reduce discharge volumes, thereby mitigating environmental impacts like salinization. Similarly, Canada's projects emphasize integrated water recycling in , enabling sustained output of 2.86 million tons annually with minimized thermal energy use post-2023 optimizations.

Laboratory synthesis

One standard laboratory method for preparing potassium chloride involves the neutralization reaction between and , which proceeds according to the equation KOH + HCl → KCl + H₂O. The procedure typically begins by dissolving a known quantity of potassium hydroxide pellets in to form an , followed by the slow addition of dilute with stirring until the solution reaches neutrality, as indicated by measurement or phenolphthalein indicator turning colorless. The resulting solution is then gently heated to evaporate excess , yielding potassium chloride crystals upon cooling; this acid-base reaction theoretically provides stoichiometric yields approaching 100% based on the , though practical losses from splashing or incomplete evaporation may reduce recovery to 80-95%. Common impurities, such as unreacted hydroxide or chloride from impure reagents, can be minimized by using analytical-grade starting materials, but sodium chloride contamination may arise if trace sodium is present in the potassium hydroxide source. An alternative approach utilizes or , historically derived from , reacted with : for carbonate, K₂CO₃ + 2HCl → 2KCl + H₂O + ; for bicarbonate, KHCO₃ + HCl → KCl + H₂O + . In practice, solid (2-3 grams) is weighed into an , dissolved in minimal (about 5 mL), and is added dropwise until ceases and neutrality is achieved, followed by to crystallize the product. This method, akin to early 19th-century techniques where was treated with muriatic (an archaic name for HCl), allows for gas evolution that aids in driving the reaction forward and purifying the mixture by removing carbonates. Yields are similarly high under controlled conditions, but carbon dioxide bubbling can introduce minor aeration losses; impurities like residual are avoided by excess . Purity of the synthesized potassium chloride is verified through methods such as to confirm content, flame photometry for potassium ion concentration, or to detect absences of or peaks. determination (around 770°C) or tests in (sparingly soluble, unlike ) further distinguish it from common contaminants. These small-scale syntheses, suitable for educational demonstrations or labs, contrast with industrial processes by prioritizing purity over cost, enabling products with >99% purity when using high-grade inputs.

History

Discovery and early characterization

The element potassium was first isolated on October 6, 1807, by English chemist Humphry Davy through electrolysis of molten caustic potash (potassium hydroxide, KOH), using a powerful voltaic battery composed of hundreds of cells to generate the necessary current and voltage for decomposition. This breakthrough relied on Alessandro Volta's 1800 invention of the voltaic pile, which provided a stable electrical source surpassing earlier frictional machines, enabling Davy to overcome the resistance of alkali compounds previously deemed undecomposable and thus refute lingering phlogiston-era views that such substances were elemental. Davy named the silvery metal "potassium" after "potash," the common source material, distinguishing it from sodium isolated similarly shortly thereafter. Chlorine, the other constituent of potassium chloride, had been identified decades earlier in 1774 by Swedish chemist , who produced the greenish-yellow gas by reacting (then termed muriatic acid) with (pyrolusite). Scheele described its bleaching and corrosive properties but initially viewed it as a compound containing oxygen, a misinterpretation corrected later by in 1810, who established as an element through analogous electrochemical analysis. This elemental identification facilitated the synthesis and characterization of chloride salts, including potassium chloride (KCl), via neutralization of with muriatic acid. Prior to elemental isolation, potassium chloride was recognized in early 19th-century chemistry as "muriate of ," a double decomposition product from and common salt or direct reaction, valued for its and distinct crystalline form despite lacking knowledge of its atomic composition. Post-1807, Davy's work confirmed KCl as a binary ionic compound of the new metal and , with stoichiometric ratios verified through gravimetric analysis and precipitation reactions, such as forming insoluble upon addition of . By the mid-19th century, flame further corroborated 's presence in the salt, as its vivid violet emission lines—distinct from sodium's yellow—emerged when KCl was heated in a , providing of elemental purity without reliance on prior alchemical speculations.

Commercial development

The commercial extraction of potassium chloride commenced in 1861 with the establishment of the world's first dedicated mine in Stassfurt, , where potash salts were recovered from deposits originally targeted for production. This development shifted production from small-scale leaching of —historically used for soaps and —to mechanized underground mining, spurred by Europe's expanding agricultural needs and the scientific validation of as an essential nutrient in the mid-19th century. Output grew swiftly, from 20,000 tons in 1862 to 7 million tons annually by 1909, positioning German deposits as the global cornerstone of supply amid rising demand for crop enhancement. Technological progress in the early facilitated broader industrialization, including the adoption of to separate potassium chloride (as ) from in complex ores, alongside initial of drilling and hoisting in European and emerging North American operations. These innovations lowered costs and enabled exploitation of lower-grade sylvinite deposits, transitioning from labor-intensive manual methods to semi-automated processes that supported export-oriented growth. Canada's province marked a pivotal expansion phase, with commercial initiating in the following discoveries during oil exploration; the Lake mine near became operational around 1953, followed by the Esterhazy facility in 1961, leveraging vast Prairie Evaporite Formation reserves to challenge European dominance. Post-World War II fertilizer requirements escalated production worldwide, as mechanized farming and intensive cropping systems demanded reliable supplies to sustain yields, with demand surges aligning with the Green Revolution's rollout of nutrient-responsive varieties in the 1960s. The 1973-1974 oil crisis, however, imposed sharp cost pressures on energy-dependent , crushing, and refining, driving global prices to nearly triple prior levels and prompting efficiency adaptations amid supply constraints.

Uses

Agricultural applications

Potassium chloride (KCl), commonly known as muriate of , serves as the primary commercial source of fertilizer, providing approximately 60-62% (K₂O) equivalent. This high potassium content makes it economical for replenishing soil potassium depleted by crop removal, particularly in systems. In , potassium from KCl facilitates for water uptake and stomatal control, activates over 60 enzymes involved in and protein synthesis, and enhances disease resistance by strengthening cell walls and reducing pathogen susceptibility. These functions are critical for major cereals like corn and , where potassium deficiency impairs root development and yield potential. Application rates of KCl are determined by soil testing, typically ranging from 100-200 kg K₂O per hectare in potassium-deficient fields to maintain optimal soil levels above 200 kg K/ha in the top 15 cm. Field trials in corn and wheat on deficient soils have demonstrated yield increases of 10-25% with targeted potassium fertilization, with responses more pronounced in corn where up to 25% of sites showed economic benefits. The chloride ion in KCl can contribute to soil salinity buildup, potentially causing osmotic stress and reduced water availability in chloride-sensitive crops such as potatoes, tobacco, and grapes. However, in non-sensitive crops like corn and on well-drained arable soils, these effects are minimal and outweighed by potassium's yield-enhancing benefits, as evidenced by limited yield reductions in Midwest U.S. studies.

Medical and pharmaceutical uses

Potassium chloride serves as the primary therapeutic agent for correcting , a condition characterized by serum levels below 3.5 mmol/L, which can lead to , cardiac s, and impaired neuromuscular function due to disruptions in cellular membrane potentials and action potentials. Oral supplementation is typically initiated for mild to moderate cases, with adult doses ranging from 40 to 100 mEq per day administered in divided doses not exceeding 40 mEq per single dose to minimize gastrointestinal upset, while intravenous administration is reserved for severe (below 2.5-3.0 mmol/L) or when oral intake is not feasible, often at rates of 10-20 mEq per hour diluted in compatible fluids and monitored closely to avoid . Clinical guidelines emphasize replacing deficits based on measured losses, with evidence from observational studies and consensus recommendations showing that prompt correction reduces risk, as prolongs QT intervals and predisposes to ventricular ectopy. In intravenous fluid therapy, potassium chloride is commonly added to isotonic solutions such as 0.9% or dextrose-containing fluids to maintain normokalemia during hospitalization, particularly in patients with ongoing losses from diuretics, , or renal issues; typical maintenance additions are 20-40 mEq per liter infused at rates ensuring serum levels remain within the normal range of 3.5-5.0 mmol/L, which supports optimal skeletal and excitability and acid-base balance. Empirical data from management protocols indicate that such supplementation prevents recurrence in high-risk groups, with randomized trials confirming efficacy in postoperative and critically ill patients when guided by serial serum measurements. Early oral formulations, such as wax-matrix tablets introduced in the mid-20th century, were linked to upper gastrointestinal mucosal injury, including erosions and bleeding, due to prolonged contact with the esophageal or gastric lining, prompting a shift to liquid, effervescent, or microencapsulated extended-release versions by the 1980s that dissolve more rapidly and reduce lesion incidence, as demonstrated in endoscopic studies comparing formulation types. These modern preparations maintain therapeutic efficacy for chronic supplementation in conditions like diuretic-induced hypokalemia while lowering adverse event rates, with clinical practice favoring them for outpatient management. Potassium chloride exhibits approximately 142 known drug interactions, of which 101 are classified as major, primarily involving medications that elevate serum potassium levels, such as ACE inhibitors and ARBs used for blood pressure management, thereby increasing the risk of hyperkalemia when co-administered.

Culinary and nutritional uses

Potassium chloride serves as a low-sodium substitute for in culinary applications, offering approximately 0% sodium content compared to 39% sodium in table salt, thereby enabling reduced sodium intake in processed foods such as cheeses, snacks, and baked goods. The U.S. recognizes potassium chloride as (GRAS) for use in without quantitative limits, provided it complies with good manufacturing practices, and it is commonly incorporated to partially replace in products like baby formulas and . However, its adoption remains limited due to sensory challenges, including a bitter or metallic aftertaste perceived at higher concentrations, which differs from the clean saltiness of and can intensify with overuse, prompting food manufacturers to blend it at levels typically below 30% replacement to mitigate off-flavors. Nutritionally, potassium chloride contributes essential , an intracellular cation vital for maintaining balance, muscle function, and nerve signaling, helping to avert —a deficiency linked to , , and arrhythmias—that affects populations with low fruit and vegetable intake. In dietary contexts, its use as a salt replacer supports potassium enrichment, with meta-analyses of randomized trials indicating that increased potassium intake from such sources modestly lowers systolic by 4-5 mmHg and diastolic by 2-3 mmHg, particularly in individuals with or high baseline sodium consumption, through mechanisms like enhanced and vascular relaxation. These effects, while beneficial, do not fully replicate the sensory satisfaction of , and evidence suggests that blood pressure reductions are more attributable to concurrent sodium restriction than potassium addition alone, with no strong causal link to broader prevention beyond hypertension management in susceptible groups.

Industrial applications

Potassium chloride functions as a regenerant in ion-exchange systems for , where it exchanges with calcium and magnesium ions on beads to prevent scale formation in boilers, cooling towers, and process equipment. Unlike , it introduces potassium ions into the , which may reduce environmental sodium loads in sensitive watersheds, though its higher requires adjustments in regeneration cycles to maintain efficiency. Cost comparisons indicate potassium chloride refills at approximately $25–$50 per 40-pound bag, versus $5–$10 for , making it less economical for large-scale operations unless sodium restrictions apply. In the oil and gas sector, potassium chloride is added to water-based fluids at concentrations of 3–20% by weight to increase for hydrostatic pressure control, stabilize reactive formations, and inhibit clay swelling through cation exchange that dehydrates interlayer water in clays. This application enhances stability, reduces torque and drag on drill strings, and minimizes fluid loss into permeable zones, with typical formulations achieving weights of 8.5–12 pounds per . Potassium chloride serves as a component in fluxes to lower melting points and remove oxides during metal joining processes, particularly in of , where it contributes to formation for arc stabilization. It also acts as an in certain electrochemical cells and systems for metal refining, though commercial scale remains limited compared to chloride-based alternatives. Minor industrial roles include its use in soap manufacturing, where aqueous potassium chloride solutions facilitate the formation of soft, soluble soaps via of fats and oils, preferred for liquid detergents over harder sodium soaps. In explosives production, potassium chloride provides potassium ions in some pyrotechnic and formulations, but its tonnage consumption is negligible relative to primary sectors.

Application in capital punishment

Potassium chloride serves as the final agent in the standard three-drug protocol employed by many U.S. states for , administered intravenously after a sedative-hypnotic such as or and a neuromuscular blocker like . This sequence aims to induce unconsciousness, , and , with potassium chloride specifically triggering through acute . The protocol was first legislated in in 1977, marking the initial adoption of as an execution method in the United States, though the first implementation occurred in in 1982. The physiological mechanism involves rapid intravenous delivery of potassium chloride, typically totaling 240 milliequivalents (mEq) divided across syringes—for instance, two 120 mEq doses in —elevating extracellular potassium ion (K⁺) concentration to levels that irreversibly depolarize cardiac myocytes. This disrupts the resting , halting propagation and inducing or direct within seconds, as confirmed by electrocardiographic monitoring during executions and findings of myocardial . Empirical data from reports indicate that effective delivery results in cessation of cardiac activity shortly after injection, with serum potassium levels postmortem often exceeding 10 mmol/L, far above lethal thresholds observed in clinical cases. Variations include single-drug protocols using high-dose barbiturates for and , but potassium chloride has been incorporated as a standalone agent in some jurisdictions or as a supplement when primary sedatives fail, relying on its cardiotoxic potency at doses of 1–2 mmol/kg intravenously. In veterinary guidelines, however, potassium chloride injection without preceding general is prohibited due to the intense nociceptive response it elicits—described as a severe burning sensation along venous pathways from endothelial irritation and osmotic effects—prompting comparisons to execution outcomes where incomplete could permit similar unexpressed distress, evidenced by indicators like and elevated in cases of protocol malfunctions. Such parallels underscore causal dependencies on adequate for minimizing sensory experiences prior to , as incomplete dosing of initial agents has led to observable signs of respiratory distress and prolonged procedures in documented executions.

Safety, toxicity, and health effects

Physiological effects and toxicity mechanisms

Potassium ions (K⁺) play a fundamental role in cellular physiology, particularly in establishing and maintaining the of excitable cells such as neurons and cardiac myocytes. The high intracellular K⁺ concentration (approximately 140 mmol/L) compared to extracellular levels (3.5–5.0 mmol/L) creates an that, through selective membrane permeability via channels, generates a negative near -70 to -90 mV, as governed by the for K⁺ equilibrium potential (E_K ≈ -90 mV). This potential is essential for propagation, , and impulse transmission; disruptions alter excitability and can lead to impaired cellular function. Excessive potassium chloride intake or absorption elevates serum K⁺ levels, inducing (typically >5.5 mmol/L), which progressively depolarizes the resting toward zero by reducing the K⁺ gradient and inactivating voltage-gated sodium channels. This slows conduction velocity, widens QRS complexes on ECG, and promotes re-entrant arrhythmias, potentially culminating in or at levels exceeding 7.0–8.0 mmol/L; symptoms include , , and peaked T-waves progressing to sine-wave patterns. The acute oral (LD50) in rats is approximately 2600 mg/kg, reflecting dose-dependent absorption overwhelming renal excretion and shift mechanisms like insulin-mediated uptake. Intracellularly, disrupts Na⁺/K⁺-ATPase activity and calcium handling, exacerbating contractility failure in cardiac tissue. Gastrointestinal exposure to potassium chloride causes local primarily through hyperosmotic effects in the gut lumen, drawing fluid via and inducing mucosal , , , , and ; this is dose-related, with high-concentration formulations (>10–20% solutions) amplifying risk via direct chemical . In chronic scenarios, particularly among patients with renal impairment (e.g., stages 3–5), sustained exposure elevates incidence due to diminished glomerular filtration and tubular secretion, associating with heightened mortality from arrhythmias independent of other factors. While acute oral thresholds for potassium chloride (LD50 ≈2600 mg/kg) are comparable to (LD50 ≈3000–4000 mg/kg in ), the former's specificity for membrane confers greater cardiac vulnerability, as sodium overload primarily induces volume expansion and rather than direct conduction blockade.

Risks in medical administration and historical errors

In the 1980s and , concentrated potassium chloride (KCl) vials stocked on nursing units contributed to multiple fatal overdoses in the United States, primarily through inadvertent intravenous administration of undiluted solutions, which induced acute and . For example, York Hospital in reported two patient deaths from KCl mishandling in 1987 and 1989. In June 1990, three infants died at a U.S. after receiving potassium chloride intended for other uses, resulting in rapid drops despite attempts. Between 1996 and 1998, the for Accreditation of Healthcare Organizations identified 10 deaths linked to erroneous KCl dosing, often involving direct IV pushes of concentrate mistaken for compatible fluids. These events highlighted causal factors such as easy access to high-potency forms (e.g., 2 mEq/mL vials) and inadequate dilution protocols, with KCl's narrow therapeutic window—where serum levels exceeding 5.5 mEq/L can trigger arrhythmias—exacerbating outcomes. Post-2000 interventions addressed these vulnerabilities by prioritizing over reliance on individual vigilance. The Joint Commission's 2002 National Patient Safety Goal mandated removing concentrated KCl from patient care areas, prompting nearly all U.S. hospitals to centralize preparation in pharmacies by the , thereby eliminating floor stock as a point. Complementary measures included barcode-assisted administration for dose verification and automated dispensing cabinets to restrict access, reducing opportunities for selection errors. Data from mode analyses confirm these changes lowered administration error rates, with multi-factorial protocols in high-risk units (e.g., ) achieving near-elimination of potential harm through integrated safeguards at prescribing, dispensing, and delivery stages. Residual risks persist from manufacturing and labeling discrepancies, as evidenced by ICU Medical's , 2025, voluntary of one lot each of 20 mEq/100 mL and 10 mEq/50 mL KCl injection bags, where overwrap labels mismatched contents (e.g., 20 mEq bags labeled as 10 mEq), potentially leading to doubled dosing if not verified against inner labels. While such recalls underscore ongoing vulnerabilities, empirical reviews attribute post-intervention declines in KCl errors to systemic redesign rather than overregulation, though some analyses note clinician workarounds in rigidly enforced environments may necessitate balanced policy evolution. In contexts—ironically, the condition induced by KCl overdose—debates center on temporizing agents like insulin (which shifts intracellularly but risks if dosed erroneously at 5-10 units IV) versus potassium binders (e.g., patiromer), with favoring binders for sustained without glucose fluctuations, though insulin remains standard for acute cases due to faster onset (15-30 minutes vs. hours).

Regulatory and handling precautions

Under the U.S. Administration's Hazard Communication Standard (29 CFR 1910.1200), potassium chloride requires safety data sheets detailing handling precautions, including minimizing generation, using such as gloves and , and washing hands after contact to prevent irritation from concentrated forms or . Storage guidelines specify keeping it in tightly closed containers in a dry, cool, well-ventilated area away from due to its hygroscopic and incompatibles like strong acids or oxidizers that could generate hazardous gases. For pharmaceutical applications, the U.S. mandates dilution of potassium chloride injection concentrates before administration, preferably via central venous routes for higher concentrations to ensure thorough blood dilution and avoid localized . Labels emphasize careful verification of dilution and infusion rates, with concentrated forms restricted from patient care units in many facilities following safety alerts. Globally, the Globally Harmonized System (GHS) typically does not classify pure potassium chloride as highly hazardous but notes potential for acute oral toxicity (category 4) and skin/eye irritation in some assessments. Fertilizer-grade potassium chloride, comprising 95-99% purity, adheres to standards like those from the USDA emphasizing safe handling to minimize and contamination, with over 90% of production directed to agricultural use. For execution purposes, protocols often utilize pharmaceutical-grade potassium chloride (>99% purity, USP compliant) but involve heightened security measures and non-clinical preparation to deliver lethal boluses, contrasting with therapeutic dilutions; handling precautions mirror industrial norms but prioritize staff protection from accidental exposure in controlled environments. Implementation of restrictions on unit-dose concentrated potassium chloride in hospitals since the late 1990s, including removal from wards, has empirically reduced fatal medication errors, with reports indicating greater compared to prior decades when such vials were routinely accessible on units.

Economic and market aspects

Global production and trade

Potassium chloride production relies predominantly on underground mining of deposits, primarily sylvinite ore, followed by flotation and crystallization processes to yield fertilizer-grade or industrial-grade KCl. Global output is dominated by , , and , which collectively accounted for over 65% of potash mine production in 2023, with holding about 32% share through operations in . In 2024, produced approximately 15 million metric tons of potash (K₂O equivalent), 9 million metric tons, and 7 million metric tons, reflecting increases from prior years driven by expanded capacity in these nations. Major trade flows involve exports from these producers to import-dependent regions like , , and , with leading shipments of over 22 million metric tons of KCl in 2023, followed by and . Annual global potash trade volumes approximate 40 million metric tons of KCl, underscoring vulnerabilities due to concentration in politically sensitive regions. Geopolitical tensions have periodically strained these dynamics; for instance, Western sanctions in early 2022, including the EU's March import ban on Belarusian and Lithuania's February halt of rail transit through its territory, slashed Belarusian output by 60% to 3 million metric tons that year, necessitating costly rerouting via Russian or alternative Baltic ports and briefly constricting worldwide availability. Potash reserves are unevenly distributed, with possessing the largest at 1.1 billion metric tons (K₂O equivalent), 920 million metric tons, and significant but smaller deposits, ensuring long-term production potential amid current extraction rates of roughly 48 million metric tons annually. Sustainability assessments indicate reserves could support global demand for centuries, though economic factors like energy costs for evaporation and geopolitical stability influence viable recovery rates from these formations.
Country2024 Production (million MT K₂O equiv.)Reserves (billion MT K₂O equiv.)
151.1
90.92
7~0.75
The global potassium chloride market has exhibited steady growth post-2023, projected to reach USD 38.28 billion by 2033, expanding at a compound annual growth rate (CAGR) of 4.9% from 2025 onward, primarily propelled by surging demand for fertilizers amid global population increases and agricultural intensification needs. Fertilizer applications, accounting for over 90% of consumption, continue to dominate, with forecasts indicating potash shipments between 68 and 71 million tons in 2024, reflecting resilient demand despite supply chain fluctuations. This trajectory underscores potassium chloride's cost-effectiveness relative to alternatives like potassium sulfate, prioritizing agricultural productivity enhancements over selective environmental critiques that may undervalue yield imperatives in food security contexts. Pricing dynamics showed recovery following a 2023 dip to approximately USD 383 per metric ton, with prices climbing to around USD 352-378 per by late 2024 and into 2025, buoyed by anticipated stronger demand in early 2025 quarters. Market participants, including major producers like and , reported stabilized revenues despite earlier pressures, with achieving €557.7 million in EBITDA for 2024 amid low prices. Innovations in production have focused on gains, such as AI-driven extraction processes and advanced solution techniques that minimize emissions and operational costs, as adopted by leading firms like for optimized recovery. In January 2025, Qaz Boxs introduced high-purity Potassium Chloride 60% , engineered for superior growth and strength, exemplifying tailored formulations to boost application efficacy. These developments, including innovative structures for enhanced release introduced in by 2023, reinforce potassium chloride's market dominance by addressing both yield optimization and without compromising affordability.

References

  1. https://pubchem.ncbi.nlm.nih.gov/compound/Potassium-Chloride
  2. https://www.epa.gov/system/files/documents/2023-03/Potassium%2520Chloride%2520Supply%2520Chain%2520Profile.pdf
  3. https://www.cropnutrition.com/resource-library/potassium-chloride/
  4. https://www.ncbi.nlm.nih.gov/books/NBK557785/
  5. https://www.americanelements.com/potassium-chloride-7447-40-7
  6. https://next-gen.materialsproject.org/materials/mp-23193
  7. https://www.chemicalbook.com/ChemicalProductProperty_US_CB9137176.aspx
  8. https://hpvchemicals.oecd.org/ui/handler.axd?id=2956d0b6-b409-46f0-8e89-a769869fd00d
  9. https://www.crystran.com/optical-materials/potassium-chloride-kcl/
  10. https://www.sciencedirect.com/science/article/abs/pii/S0921883118302462
  11. https://webbook.nist.gov/cgi/cbook.cgi?ID=C7447407&Mask=4&Type=ANTOINE&Plot=on
  12. https://www.ck12.org/flexi/chemistry/energy-and-covalent-bond-formation/what-is-the-molecule-kcl/
  13. http://ch301.cm.utexas.edu/atomic/#bonding/bonding-all.php
  14. https://www.chemtopper.com/smf/cbse-xi-and-xii-chemistry/lattice-energy-hydration-energy-solution-energy/
  15. https://www.echemi.com/cms/2103069.html
  16. https://www.researchgate.net/figure/Stability-of-new-potassium-chlorides-a-Pressure-composition-phase-diagram-of-the-K-Cl_fig1_303498256
  17. https://www.sciencedirect.com/topics/earth-and-planetary-sciences/sylvite
  18. https://pubs.usgs.gov/sir/2010/5090/s/pdf/sir2010-5090-S.pdf
  19. https://pubs.usgs.gov/periodicals/mcs2022/mcs2022-potash.pdf
  20. https://www.uralkali.com/buyers/production/methods/
  21. http://scientists.uz/uploads/202305/A-21.pdf
  22. https://www.sciencedirect.com/science/article/abs/pii/S0892687518305351
  23. https://www.nouryon.com/globalassets/nouryon/2.-markets/2-market-segment-pages/mining/article-fertilizer-international-mining-sustainable-potash-reagents-en.pdf
  24. https://nora.nerc.ac.uk/id/eprint/534427/1/mpf_potash.pdf
  25. https://www.911metallurgist.com/blog/potash-recovery-solar-evaporation-flotation/
  26. https://ebner-co.de/en/applications/crystallization-of-kcl-mop/
  27. https://pubs.usgs.gov/periodicals/mcs2020/mcs2020-potash.pdf
  28. https://investingnews.com/daily/resource-investing/agriculture-investing/potash-investing/top-potash-countries-by-production/
  29. https://mosaicco.com/fileLibrary/publicFiles/0-2024-Sustainability-Disclosure-and-GRI.pdf
  30. https://www.veolia.com/en/our-customers/achievements/industries/mining/canada-k-s-potash
  31. https://issuu.com/delcomminc/docs/ppe_1_-_2024
  32. https://www.docbrown.info/page03/abs-equations/abs06a-kcl.htm
  33. https://quizlet.com/398442633/quantitative-preparation-of-potassium-chloride-flash-cards/
  34. https://www.atamanchemicals.com/potassium-chloride_u24956/
  35. https://pubs.acs.org/doi/10.1021/acsreagents.4283
  36. https://www.sciencehistory.org/stories/magazine/science-and-celebrity-humphry-davys-rising-star/
  37. https://uwaterloo.ca/chem13-news-magazine/april-2019/feature/humphry-davy-and-voltaic-pile
  38. https://pubsapp.acs.org/cen/80th/print/potassium.html
  39. https://www.britannica.com/biography/Carl-Wilhelm-Scheele
  40. https://winter.group.shef.ac.uk/webelements/chlorine/history.html
  41. https://www.cambridge.org/core/books/cambridge-world-history-of-food/potassium/D85301E14CF1CF99C173B5BA5613A14F
  42. https://www.bhp.com/news/bhp-insights/2017/07/feeding-the-world-the-case-for-potash-2
  43. https://icl-growingsolutions.com/agriculture/knowledge-hub/the-dead-sea-potash-history/
  44. https://www.911metallurgist.com/blog/potash-flotation/
  45. https://www.src.sk.ca/blog/history-srcs-work-saskatchewans-potash-industry
  46. https://republicofmining.com/2014/03/18/saskatchewan-potash-history-by-john-burton-the-encyclopedia-of-saskatchewan-unknown-date/
  47. https://www.bhp.com/news/bhp-insights/2023/05/the-potash-industrys-fourth-wave
  48. https://documents1.worldbank.org/curated/en/252751492709642600/pdf/Fertilizer-issues-in-the-1970s-and-beyond.pdf
  49. https://www.ipipotash.org/udocs/Chap-1_potash_production.pdf
  50. https://nutrien-ekonomics.com/news/potassium-fertilizers-muriate-of-potash-or-sulfate-of-potash/
  51. https://www.cropnutrition.com/resource-library/what-is-potash/
  52. https://pmc.ncbi.nlm.nih.gov/articles/PMC3645691/
  53. https://pmc.ncbi.nlm.nih.gov/articles/PMC7927068/
  54. https://www.sciencedirect.com/science/article/abs/pii/B9780128001325000031
  55. https://www.alberta.ca/potassium-management-in-crops
  56. https://ohioline.osu.edu/factsheet/anr-0147
  57. https://www.protassiumplus.com/chloride-salt-sensitivity-in-potatoes
  58. https://farmdoc.illinois.edu/field-crop-production/soils/potash-fertilizer-is-there-a-problem.html
  59. https://www.tfi.org/wp-content/uploads/2024/01/tfi-chloride.pdf
  60. https://www.ncbi.nlm.nih.gov/books/NBK539791/
  61. https://www.accessdata.fda.gov/drugsatfda_docs/label/2014/206814lbl.pdf
  62. https://www.aafp.org/pubs/afp/issues/2023/0100/potassium-disorders-hypokalemia-hyperkalemia.html
  63. https://reference.medscape.com/drug/kdur-slow-k-potassium-chloride-344450
  64. https://emedicine.medscape.com/article/2054364-overview
  65. https://www.sciencedirect.com/science/article/pii/S0140673682900022
  66. https://jamanetwork.com/journals/jamainternalmedicine/fullarticle/608303
  67. https://www.drugs.com/drug-interactions/potassium-chloride.html
  68. https://pmc.ncbi.nlm.nih.gov/articles/PMC4848703/
  69. https://www.fda.gov/media/125081/download
  70. https://www.sciencedirect.com/science/article/abs/pii/S0308814618301961
  71. https://www.cargill.com/salt-in-perspective/does-potassium-chloride-taste-salty
  72. https://ods.od.nih.gov/factsheets/Potassium-HealthProfessional/
  73. https://pmc.ncbi.nlm.nih.gov/articles/PMC7429027/
  74. https://www.ncbi.nlm.nih.gov/books/NBK67148/
  75. https://www.ahajournals.org/doi/10.1161/HYPERTENSIONAHA.119.13241
  76. https://academic.oup.com/ckj/article/18/7/sfaf173/8177122
  77. https://www.brenntag.com/en-ch/products/potassium-chloride.html
  78. https://www.gunjalindustries.com/potassium-chloride-industrial-grade/
  79. https://www.inchcalculator.com/water-softener-cost-guide/
  80. https://www.lowes.com/n/buying-guide/water-softener-salt-vs-potassium
  81. https://www.tridentenergyintl.com/blogs/post/role-of-potassium-chloride-in-the-oil-gas-industry
  82. https://vinipulchemicals.com/potassium-chloride-industrial-applications
  83. https://neuchem.com/product/potassium-chloride
  84. https://gilsonite-bitumen.com/products/potassium-chloride/
  85. https://bchem.com/product/oil-gas-chemicals/potassium-chloride/
  86. https://www.britannica.com/science/potassium/Principal-compounds-and-reactions-with-other-elements
  87. https://pmc.ncbi.nlm.nih.gov/articles/PMC1876417/
  88. https://www.uspharmacist.com/article/use-of-legally-marketed-drugs-for-lethal-injection
  89. https://deathpenaltyinfo.org/executions/methods-of-execution/description-of-each-method
  90. https://oklahoma.gov/content/dam/ok/en/doc/documents/policy/section-04/040301ad.pdf
  91. https://pubmed.ncbi.nlm.nih.gov/19924677/
  92. https://iacuc.wsu.edu/documents/2019/11/sop-6.pdf/
  93. https://www.hrw.org/report/2006/04/23/so-long-they-die/lethal-injections-united-states
  94. https://avmajournals.avma.org/view/journals/javma/259/2/javma.259.2.197.pdf
  95. https://eji.org/news/lethal-injections-cause-suffocation-and-severe-pain-autopsies-show/
  96. https://www.ncbi.nlm.nih.gov/books/NBK538338/
  97. https://teachmephysiology.com/nervous-system/synapses/resting-membrane-potential/
  98. https://www.merckmanuals.com/professional/endocrine-and-metabolic-disorders/electrolyte-disorders/hyperkalemia
  99. https://www.fishersci.com/store/msds?partNumber=P217500&productDescription=POT%2BCHLORIDE%2BACS%2B500G&vendorId=VN00033897&countryCode=US&language=en
  100. https://pmc.ncbi.nlm.nih.gov/articles/PMC9356601/
  101. https://pubmed.ncbi.nlm.nih.gov/29595886/
  102. https://www.pamedmal.com/hospital-medication-mistakes/
  103. https://www.nytimes.com/1990/06/24/us/three-infants-dead-after-hospital-gives-them-wrong-drugs.html
  104. https://pmc.ncbi.nlm.nih.gov/articles/PMC3327087/
  105. https://pmc.ncbi.nlm.nih.gov/articles/PMC3138362/
  106. https://pmc.ncbi.nlm.nih.gov/articles/PMC1181270/
  107. https://journals.sagepub.com/doi/abs/10.1177/1078155213504443
  108. https://www.fda.gov/safety/recalls-market-withdrawals-safety-alerts/icu-medical-issues-nationwide-recall-potassium-chloride-injection-20-meq-and-potassium-chloride
  109. https://emcrit.org/ibcc/hyperkalemia/
  110. https://pmc.ncbi.nlm.nih.gov/articles/PMC11626971/
  111. https://www.fishersci.ca/content/dam/fishersci/en_US/documents/programs/education/regulatory-documents/sds/chemicals/chemicals-p/S25484A.pdf
  112. https://www.accessdata.fda.gov/drugsatfda_docs/label/2019/019904s020lbl.pdf
  113. https://www.ams.usda.gov/sites/default/files/media/2023TechnicalReport_HandlingPotassiumChloride.pdf
  114. https://basekim.ae/potassium-chloride-kcl-grades/
  115. https://www.nursingcenter.com/journalarticle?Article_ID=4401093&Journal_ID=237151&Issue_ID=4401088
  116. https://natural-resources.canada.ca/minerals-mining/mining-data-statistics-analysis/minerals-metals-facts/potash-facts
  117. https://pubs.usgs.gov/periodicals/mcs2025/mcs2025-potash.pdf
  118. https://wits.worldbank.org/trade/comtrade/en/country/ALL/year/2023/tradeflow/Exports/partner/WLD/product/310420
  119. https://www.osw.waw.pl/en/publikacje/osw-commentary/2024-11-20/tough-business-tough-times-belarusian-exports-potash
  120. https://www.ips-journal.eu/topics/economy-and-ecology/belarus-potash-industry-is-going-through-the-mill-7139/
  121. https://www.astuteanalytica.com/industry-report/potassium-chloride-market
  122. https://finance.yahoo.com/news/potassium-chloride-market-worth-over-163000319.html
  123. https://www.maximizemarketresearch.com/market-report/global-potassium-chloride-market/46536/
  124. https://www.statista.com/statistics/469705/potassium-chloride-price-forecast/?srsltid=AfmBOoqoHhJHlGwkQ46JxnEbRVE0MBag9CIk6pEVAWpRJcGf2na-d7DE
  125. https://ycharts.com/indicators/potassium_chloride_muriate_of_potash_spot_price
  126. https://www.chemanalyst.com/Pricing-data/potassium-chloride-1161
  127. https://www.kpluss.com/en-us/newsroom/press-releases/ks-on-track-despite-low-potash-prices/
  128. https://www.futuremarketinsights.com/reports/potassium-chloride-market
  129. https://www.grandviewresearch.com/industry-analysis/potassium-chloride-market-report
  130. https://www.globalgrowthinsights.com/market-reports/potassium-chloride-market-107652
  131. https://marketmindsadvisory.com/potassium-chloride-market-trends/
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