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Potassium formate
Potassium formate
Potassium formate
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Potassium formate[1]
Names
Preferred IUPAC name
Potassium formate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.008.799 Edit this at Wikidata
UNII
  • InChI=1S/CH2O2.K/c2-1-3;/h1H,(H,2,3);/q;+1/p-1 ☒N
    Key: WFIZEGIEIOHZCP-UHFFFAOYSA-M ☒N
  • InChI=1/CH2O2.K/c2-1-3;/h1H,(H,2,3);/q;+1/p-1
    Key: WFIZEGIEIOHZCP-REWHXWOFAK
  • C(=O)[O-].[K+]
Properties
CHKO2
Molar mass 84.115 g·mol−1
Appearance Colorless deliquescent crystals
Density 1.908 g/cm3
Melting point 167.5 °C (333.5 °F; 440.6 K)
Boiling point Decomposes
32.8 g/100 mL (0 °C)
331 g/100 mL (25°C)
657 g/100 mL (80 °C)
Solubility soluble in alcohol
insoluble in ether
Basicity (pKb) 10.25
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H315, H319, H335
P261, P280, P302+P352, P305+P351+P338
Lethal dose or concentration (LD, LC):
5500 mg/kg (oral, mouse)
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 formate, HCO2K, HCOOK, or KHCO2, is the potassium salt of formic acid. This strongly hygroscopic white solid[2] is an intermediate in the formate potash process for the production of potassium.[3] Potassium formate has also been studied as a potential environmentally friendly deicing salt for use on roads.[4][5] It has also been suggested for use in a less corrosive liquid desiccant.[6] A 52% solution of potassium formate has a freezing point of −60 °C (−76 °F).[7] Potassium formate brines are sometimes used for heat transfer, despite being much more corrosive than many other liquid coolants, especially to zinc and aluminum but even to many steels,[8] though some formulations are compatible with aluminum and steels.[9]

Since 1995, potassium formate has been increasingly used in aqueous drilling fluids to increase density, stabilize the hole, and improve drilling performance.[10][11][12]

References

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Revisions and contributorsEdit on WikipediaRead on Wikipedia

Potassium formate

View on Grokipedia
from Grokipedia
Potassium formate, chemically denoted as KHCO₂ or CHKO₂, is the potassium salt of (HCOOH), appearing as a colorless, hygroscopic crystalline solid with a molecular weight of 84.12 g/mol. It exhibits a of 1.91 g/cm³ and a of 165–168 °C, while being highly soluble in at approximately 337 g/100 mL at 20 °C. This compound serves as a versatile buffering agent in chemical formulations due to its ability to maintain stability in aqueous solutions. In the oil and gas industry, potassium formate is a critical additive in high-density, clear drilling and completion fluids, particularly for high-pressure, high-temperature (HPHT) wells, where it provides superior , , and inhibition of clay swelling without the need for solid weighting agents like barite. These formate brines are fully soluble in , recyclable with 80–90% recovery rates, and demonstrate low environmental , with acute LC50 values ranging from 540 mg/L for to 6900 mg/L for Mysidopsis . Beyond drilling, potassium formate functions as an eco-friendly de-icing agent, especially at for and treatment, effective in temperatures from -20 °F to 15 °F, with minimal to metals and rapid that poses low risk to or oxygen levels in water bodies. It also appears in fluids for low-temperature applications and as a in select industrial processes, underscoring its broad utility in environmentally conscious operations.

Properties

Physical properties

Potassium formate has the HCOOK and a molecular weight of 84.12 g/mol. It appears as a white, hygroscopic crystalline powder and is odorless. The hygroscopic nature causes it to absorb moisture from the air, leading to deliquescence in humid conditions. The of the solid is 1.908 g/cm³ at 20°C. It has a of 167.5°C and decomposes upon further heating without reaching a . Potassium formate exhibits high in , with values increasing markedly with , as shown in the following table:
Temperature (°C)Solubility (g/100 mL water)
032.8
20331
80657
It is soluble in methanol, ethanol, and glycerol but insoluble in acetone and benzene. Aqueous solutions of potassium formate are neutral to slightly alkaline, with a pH around 7-9 for a 10% solution.

Chemical properties

Potassium formate, as the potassium salt of formic acid, dissociates completely in aqueous solution to yield formate ions (HCOO⁻) and potassium cations (K⁺). In terms of acid-base properties, potassium formate solutions are weakly basic due to the of the formate ion, the conjugate base of the weak acid (pKa = 3.75). It functions effectively as a buffering agent when combined with , maintaining stability in the range around 3.75. Potassium formate exhibits high thermal stability up to approximately 200°C, beyond which it undergoes decomposition primarily to potassium oxalate and hydrogen gas via the coupling of formate ions. The compound is generally resistant to oxidation under ambient conditions but can participate in reactions where the formate ion serves as a mild , capable of reducing certain metal ions such as silver(I) to metallic silver in analytical procedures akin to variants of the Tollens' test. Potassium formate demonstrates good compatibility with most metals, exhibiting low corrosivity toward materials and serving as a less aggressive alternative to chloride-based salts in applications requiring material stability. Additionally, it is readily biodegradable under aerobic conditions, with degradation rates exceeding 70% within 28 days in environmental media such as and .

Synthesis

Industrial production

Potassium formate is primarily produced on an industrial scale through the neutralization of with or in . The key reaction is \ceHCOOH+KOH−>HCOOK+H2O\ce{HCOOH + KOH -> HCOOK + H2O}, which is exothermic and yields potassium formate along with as the sole . This method is favored for its simplicity, high efficiency, and ability to produce a product with purity exceeding 98%. The reaction is typically carried out under controlled conditions in stirred reactors, with temperatures maintained between 0 and 100°C to facilitate complete neutralization without or side reactions; excess base is carefully avoided to prevent formation of impurities like potassium . Following the reaction, the is concentrated via multi-effect to remove , after which the product is crystallized, separated by or , and dried to obtain solid potassium formate in flake, , or granular form. This purification sequence ensures minimal waste and high recovery rates, often above 95%, contributing to the process's economic viability and environmental profile. An alternative industrial route, though less commonly employed due to higher energy requirements, involves the reaction of with under elevated (above 690 kPa) and (100–200°C), proceeding as \ceKOH+CO−>HCOOK\ce{KOH + CO -> HCOOK}. This high-pressure method avoids reliance on but demands specialized equipment and catalysts in some variants, limiting its adoption compared to the neutralization process. Global production of potassium formate is concentrated in facilities across and , where major chemical manufacturers like operate dedicated plants with capacities reaching tens of thousands of tons annually; output is closely aligned with demand from the oilfield chemicals sector. The overall process generates low waste, primarily water, positioning it as an eco-friendly option in large-scale chemical .

Laboratory preparation

Potassium formate is commonly prepared in the laboratory through the neutralization of formic acid with potassium hydroxide. High-purity (p.a. grade) 85% formic acid is slowly added to a standardized aqueous solution of potassium hydroxide while stirring, ensuring complete reaction by monitoring the pH to neutrality or slight basicity (pH 7-8). The reaction is typically titrated using phenolphthalein as an indicator, which changes from colorless to pink at the endpoint, allowing precise control for small-scale synthesis. Following neutralization, the solution is evaporated under reduced pressure to concentrate the product, and the resulting solid is purified by recrystallization from a hot ethanol-water mixture to remove impurities and obtain colorless crystals. The purified salt is then washed with cold ethanol and dried over sulfuric acid in a desiccator. This method typically affords yields of 90-95% based on the , with the product's purity confirmed by acid-base against a standard or spectroscopic analysis such as IR or NMR to verify the absence of unreacted acid. The procedure requires the use of a to mitigate exposure to irritating vapors and an for accurate stoichiometric measurements, ensuring safety and reproducibility on a gram scale suitable for or educational purposes. Unlike the less common high-pressure method sometimes used industrially, laboratory synthesis prioritizes simplicity and precision without specialized equipment. An alternative laboratory route involves the direct reaction of with , yielding potassium formate, , and gas via gentle : \ceKHCO3+HCOOH−>HCOOK+H2O+CO2\ce{KHCO3 + HCOOH -> HCOOK + H2O + CO2} This exothermic process is carried out by adding dropwise to a suspension of in at , followed by evaporation and recrystallization as described above, offering a convenient option when is unavailable. Potassium formate was first prepared in laboratories during the using analogous neutralization techniques, aligning with the early development of organic acid salts following the isolation of .

Uses

In petroleum industry

Potassium formate serves as a key component in drilling fluids for the petroleum industry, particularly as a high-density brine used to formulate weighted, solids-free systems in high-pressure/high-temperature (HPHT) wells. Its maximum density of 1.57 g/cm³ at approximately 75-77% concentration enables effective hydrostatic pressure control without the need for solid weighting agents like barite, reducing settling issues and enhancing fluid stability. In water-based muds, potassium formate is typically incorporated at concentrations of 10-50% to achieve desired densities ranging from 8.4 to 13.1 lb/gal, providing low , high , and compatibility with polymers for improved and reduced compared to traditional cesium or zinc-based brines. It stabilizes formations by inhibiting clay hydration and swelling, minimizing instability in water-sensitive reservoirs. These properties make it suitable for non-damaging drill-in and completion fluids, particularly in sensitive and formations. Environmentally, potassium formate offers a biodegradable, non-toxic alternative to chloride-based brines, significantly lowering formation damage, scaling, and overall ecological impact during offshore operations. Its non-corrosive nature further supports compatibility with equipment, contributing to cost savings in fluid management through reduced waste and simpler disposal. Since the 1990s, potassium formate has been widely adopted in and operations for HPHT , with case studies demonstrating improved rates of penetration and production optimization in challenging reservoirs. Recent developments as of 2025 include its integration with , such as hydrothermal carbon nanospheres, to enhance thermal stability and performance in ultra-HPHT conditions exceeding 150°C and 10,000 psi.

Other applications

Potassium formate serves as an effective de-icing agent in airport fluids, typically formulated as 50-75% aqueous solutions that exhibit a low eutectic freezing point around -60°C, enabling efficient ice removal and prevention in harsh winter conditions. Its low corrosivity to materials, combined with compliance to FAA specifications, makes it suitable for applications, while its biodegradability and minimal offer environmental advantages over traditional or glycol-based de-icers by reducing runoff pollution and toxicity to aquatic life. Potassium formate functions as a buffer in various chemical processes, particularly for control in leather tanning where it serves as a neutralizing agent and "camouflage acid" to gradually adjust acidity during chromium tanning, improving penetration and uniformity. In textile , it regulates bath to enhance fixation on fibers and prevent uneven coloration. Additionally, its high ionic conductivity makes it valuable as an in alkaline cells, where formate solutions support efficient in direct formate designs operating up to 80°C. As an component in fluids, potassium formate is employed in solar thermal systems at concentrations of 30-70%, providing non-volatility and thermal stability across a wide range from -60°C to 218°C, which minimizes losses and supports reliable performance in applications. Emerging applications as of 2025 include its role in carbon capture and utilization, where electrochemical reduction of CO₂ produces potassium formate as a intermediate for CO₂ sequestration and conversion into fuels or chemicals via pilot-scale facilities. In pharmaceuticals, it functions as a and intermediate in syntheses, such as the extraction of or preparation of active compounds. While the remains the dominant consumer of potassium formate, non-oilfield applications such as de-icing and account for a portion of total global consumption.

Safety

Toxicity

Potassium formate exhibits low across various exposure routes. The oral LD50 in mice is reported as 5500 mg/kg, exceeding the threshold of 2000 mg/kg for as non-toxic. Dermal LD50 values are greater than 2000 mg/kg in rats, based on analogous testing with similar formate salts. data for dust forms indicate low hazard potential, with no specific LC50 established but general assessments showing no acute classification under GHS criteria. Skin and eye contact with potassium formate results in mild , causing temporary redness and discomfort but no evidence of , , or severe damage in rabbit dermal and ocular tests. Ingestion may lead to gastrointestinal upset, including and , particularly at high doses; excessive intake can elevate serum potassium levels, potentially causing , though such poisoning is rare due to the compound's low inherent . incidents are uncommon. Chronic exposure to potassium formate shows no evidence of carcinogenicity, mutagenicity, germ cell mutagenicity, or , with regulatory assessments confirming its non-hazardous status under GHS guidelines. Long-term studies are limited, but the absence of target organ toxicity supports safe use in occupational settings at typical exposure levels. Regulatory bodies classify potassium formate as non-hazardous. It is not listed under EPA hazardous substances or SARA Title III sections, and REACH evaluations do not assign it hazard classifications for human health endpoints. Individuals with renal impairment require caution, as impaired potassium excretion may exacerbate risks of from exposure.

Handling and storage

Potassium formate should be handled with appropriate (PPE) to minimize exposure risks. For handling the powder form, gloves (with a breakthrough time of at least 480 minutes), safety goggles or glasses with side shields, and a or P1 filter are recommended to prevent contact, eye , and of . Concentrated solutions require similar PPE, with emphasis on avoiding direct contact due to potential mild . Storage of potassium formate requires cool, dry, well-ventilated conditions in tightly sealed containers made of or coated to protect against its hygroscopic nature. It should be kept away from incompatible materials such as strong acids and oxidizing agents to prevent reactions. Under these conditions, the compound maintains stability for extended periods, typically exceeding two years when shielded from . In the event of a spill, ensure adequate ventilation and avoid generating ; for , sweep up carefully and collect into suitable containers, while for liquids, dike the area and absorb with an inert material such as or before disposal. Residues may be neutralized with dilute acid if necessary, but ventilation of the area is essential to disperse any fumes. Potassium formate is non-flammable under normal conditions but may decompose during a fire, releasing , , , and potassium oxides; use fog, dry chemical, or for cooling surrounding containers, and firefighters should wear . For transportation, potassium formate is not classified as a dangerous good and has no , allowing shipment under standard regulations such as ADR, IMDG, and DOT without special precautions. Waste disposal involves diluting small quantities with water and flushing to a sewer if permitted by local regulations, as the compound is biodegradable and non-hazardous; larger amounts should be sent to an approved waste disposal facility in sealed containers.

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