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Disodium phosphate
Disodium phosphate
Disodium phosphate
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Disodium phosphate
Structural formula of disodium phosphate
Ball-and-stick model of the component ions of disodium phosphate
  Sodium, Na
  Phosphorus, P
  Oxygen, O
  Hydrogen, H
Names
IUPAC name
Disodium hydrogen phosphate
Other names
  • Acetest
  • Dibasic sodium phosphate
  • Disodium hydrogen orthophosphate
  • Disodium hydrogen phosphate
  • Disodium phosphate
  • Sodium phosphate dibasic
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.590 Edit this at Wikidata
EC Number
  • 231-448-7
E number E339(ii) (antioxidants, ...)
RTECS number
  • WC4500000
UNII
  • InChI=1S/2Na.H3O4P/c;;1-5(2,3)4/h;;(H3,1,2,3,4)/q2*+1;/p-3 ☒N
    Key: BNIILDVGGAEEIG-UHFFFAOYSA-K ☒N
  • InChI=1/2Na.H3O4P/c;;1-5(2,3)4/h;;(H3,1,2,3,4)/q2*+1;/p-3
    Key: BNIILDVGGAEEIG-DFZHHIFOAK
  • OP(=O)([O-])[O-].[Na+].[Na+]
Properties
Na2HPO4
Molar mass
  • 141.96 g/mol (anhydrous)
  • 177.99 g/mol (dihydrate)
  • 268.07 g/mol (heptahydrate)
Appearance White crystalline solid
Odor Odorless
Density 1.7 g/cm3
Melting point 250 °C (482 °F; 523 K) Decomposes
7.7 g/(100 ml) (20 °C)
11.8 g/(100 ml) (25 °C, heptahydrate)
Solubility Insoluble in ethanol
log P −5.8
Acidity (pKa) 12.35
−56.6·10−6 cm3/mol
1.35644 to 1.35717 at 20°C
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Irritant
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):
17000 mg/kg (rat, oral)
Safety data sheet (SDS) ICSC 1129
Related compounds
Other anions
 sodium phosphite
Other cations
 Dipotassium phosphate
Diammonium phosphate
Related compounds
 Monosodium phosphate
Trisodium phosphate
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 ?)

Disodium phosphate (DSP), or disodium hydrogen phosphate, or sodium phosphate dibasic, is an inorganic compound with the chemical formula Na2HPO4. It is one of several sodium phosphates. The salt is known in anhydrous form as well as hydrates Na2HPO4·nH2O, where n is 2, 7, 8, and 12. All are water-soluble white powders. The anhydrous salt is hygroscopic.[1]

The pH of disodium hydrogen phosphate water solution is between 8.0 and 11.0, meaning it is moderately basic:

HPO2−4 + H2O ⇌ H2PO−4 + OH−

Production and reactions

[edit]

It can be generated by neutralization of phosphoric acid with sodium hydroxide:

H3PO4 + 2 NaOH → Na2HPO4 + 2 H2O

Industrially It is prepared in a two-step process by treating dicalcium phosphate with sodium bisulfate, which precipitates calcium sulfate:[2]

CaHPO4 + NaHSO4 → NaH2PO4 + CaSO4

In the second step, the resulting solution of monosodium phosphate is partially neutralized:

NaH2PO4 + NaOH → Na2HPO4 + H2O

Uses

[edit]

It is used in conjunction with trisodium phosphate in foods and water softening treatment. In foods, it is used to adjust pH. Its presence prevents coagulation in the preparation of condensed milk. Similarly, it is used as an anti-caking additive in powdered products.[3] It is used in desserts and puddings, e.g. Cream of Wheat to quicken cook time, and Jell-O Instant Pudding for thickening. In water treatment, it retards calcium scale formation.[citation needed] It is also found in some detergents and cleaning agents.[2]

Heating solid disodium phosphate gives the useful compound tetrasodium pyrophosphate:[citation needed]

2 Na2HPO4 → Na4P2O7 + H2O

Laxative

[edit]

Monobasic and dibasic sodium phosphate are used as a saline laxative to treat constipation or to clean the bowel before a colonoscopy.[4]

References

[edit]
[edit]
Revisions and contributorsEdit on WikipediaRead on Wikipedia

Disodium phosphate

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from Grokipedia
Disodium phosphate, also known as dibasic or disodium hydrogen phosphate, is an inorganic sodium salt of with the chemical formula Na₂HPO₄. It appears as a colorless to white crystalline solid that is highly soluble in but insoluble in , with a molecular weight of 141.96 g/mol and a range of 8.4–9.6 in a 1% . This compound is produced commercially by neutralizing with or , followed by and if the anhydrous form is required. , domestic production was approximately 0.5 million kilograms in 2019, with combined U.S. consumption of monosodium and disodium phosphates around 19 million kilograms in 2019, largely supplemented by imports primarily from . Disodium phosphate is widely recognized as safe (GRAS) by the U.S. for use as a , serving as an emulsifying agent, buffer, , and sequestrant in products such as processed cheeses, baked goods, cereals, and beverages to improve texture, stability, and . Beyond food applications, it functions as a fertilizer component to supply to , a buffering agent in pharmaceuticals and , and a or scale preventer in systems. In industrial settings, it is employed in detergents, , and formulations due to its and ability to bind metal ions. While generally safe at regulated levels, disodium phosphate can cause to the skin, eyes, and upon direct contact or , and excessive may lead to gastrointestinal distress or, in rare cases, phosphate-related health issues such as nephropathy. Its environmental impact is moderated through controlled use, particularly in to prevent without excessive phosphate discharge.

Chemical properties

Molecular structure

Disodium phosphate, also known as sodium hydrogen phosphate, has the \ceNa2HPO4\ce{Na2HPO4} in its form. It exists as an ionic compound composed of two sodium cations (\ceNa+\ce{Na+}) and one hydrogen phosphate anion (\ceHPO42−\ce{HPO4^2-}). The hydrogen phosphate anion features a central atom bonded to four oxygen atoms in a tetrahedral , with one oxygen atom protonated, forming P-O bonds typical of groups. The compound commonly occurs in hydrated forms, represented by the general formula \ceNa2HPO4⋅nH2O\ce{Na2HPO4 \cdot nH2O}, where n=0,2,7,8,n = 0, 2, 7, 8, or 1212. The anhydrous form (n=0n = 0) appears as a white, hygroscopic crystalline powder that readily absorbs moisture from the air. In contrast, the dihydrate form (n=2n = 2) crystallizes in an orthorhombic system with Pbca. The of the form is 141.96 g/mol, while that of the dihydrate is 177.99 g/mol. These structural features, including the ionic dissociation and tetrahedral arrangement, underpin the compound's and reactivity in aqueous environments.

Physical characteristics

Disodium phosphate appears as a , odorless, hygroscopic powder in its form. This characteristic enables it to readily absorb atmospheric moisture, influencing its handling and storage requirements. The compound exhibits high solubility in water, with the anhydrous form dissolving at approximately 11.8 g per 100 g of at 25°C, while the heptahydrate shows a solubility of 11.8 g per 100 mL at the same temperature. It is slightly soluble or insoluble in alcohol () and insoluble in . These solubility traits stem from its ionic nature, which facilitates dissociation in polar solvents like but not in non-polar ones. The density of anhydrous disodium phosphate is 1.70 g/cm³. It does not have a defined , instead decomposing at around 250°C to form sodium without . Aqueous solutions of disodium phosphate are alkaline, with values ranging from 8.0 to 11.0 depending on concentration; for instance, a 5% solution at 25°C has a of 8.9–9.2. This basicity arises from the of the hydrogen phosphate . Due to its hygroscopic properties, anhydrous disodium phosphate absorbs from the air to form , typically incorporating 2 to 7 moles of depending on ambient and , with common forms including the dihydrate (stable up to about 92.5°C) and dodecahydrate under high conditions. The stability of these hydrate forms varies with relative : the form is stable below 50% RH, while higher favors the heptahydrate or dodecahydrate.

Production

Industrial production

Disodium phosphate is primarily produced on an industrial scale through the neutralization of with or , a that ensures by utilizing readily available and generating the product in high yield. The reaction is controlled to a pH of approximately 8.2–8.5 to selectively form the disodium salt, avoiding over-neutralization to . For the route, the balanced equation is: H3PO4+2NaOH→Na2HPO4+2H2O\mathrm{H_3PO_4 + 2NaOH \rightarrow Na_2HPO_4 + 2H_2O} This method leverages wet-process phosphoric acid derived from the digestion of phosphate rock with sulfuric acid, a key step in the global fertilizer industry that supplies the bulk of industrial phosphoric acid. The scale of disodium phosphate production is thus closely linked to fertilizer manufacturing, with U.S. output reaching about 0.5 million kilograms in 2019 across a few dedicated facilities. An alternative industrial route involves a two-step reaction starting with and : first, CaHPO₄ + NaHSO₄ → NaH₂PO₄ + CaSO₄, producing and precipitating () as a byproduct, followed by partial neutralization of the with or to form disodium phosphate: NaH₂PO₄ + NaOH → Na₂HPO₄ + H₂O. This is followed by to remove the insoluble (), enhancing purity. Gypsum generation in this process aligns with broader phosphate industry practices, where it accumulates as a major waste stream from wet-process acid production, often exceeding 5 tons per ton of . Purification typically occurs via from an of the neutralized product, allowing separation of the disodium phosphate as either the form or common hydrates like the dodecahydrate (Na₂HPO₄·12H₂O). Hydrated crystals can be further processed in a to yield the variant if required for specific applications, optimizing yield and minimizing energy costs in large-scale operations. This step is particularly effective due to the compound's characteristics, ensuring high-purity output from impure wet-process feedstocks.

Laboratory synthesis

Disodium phosphate is commonly prepared in the laboratory through the neutralization of with , targeting a 1:2 molar ratio to form Na₂HPO₄ specifically. The process involves dissolving orthophosphoric acid (H₃PO₄) in and slowly adding a standardized (NaOH) solution under constant stirring and cooling to control the . The pH is closely monitored using a to ensure complete conversion to the disodium salt (near the pKₐ₂ of at 7.2 for the second step) without over-neutralization that would yield (Na₃PO₄). The resulting solution is then filtered to remove any impurities and evaporated at or slightly elevated temperatures (below 100°C) to it, followed by cooling to induce of the dodecahydrate form, Na₂HPO₄·12H₂O, which is the stable under typical lab conditions due to its characteristics. For the anhydrous form, higher temperatures (around 100–110°C) are used during , though this risks . Alternative laboratory routes involve adjusting sodium phosphate mixtures, such as treating (NaH₂PO₄) with additional NaOH to shift the equilibrium toward Na₂HPO₄ via partial deprotonation (NaH₂PO₄ + NaOH → Na₂HPO₄ + H₂O), or using resins loaded with sodium ions to exchange protons from derivatives. Selective can also be employed by exploiting solubility differences; for instance, cooling a supersaturated solution of a mixed sodium phosphate system favors the precipitation of the less soluble dodecahydrate over other forms. Purity and composition of the synthesized disodium phosphate are verified analytically, primarily through acid-base . A sample is dissolved in , excess standardized (HCl) is added to convert it fully to , and the excess acid is back-titrated with NaOH using a or potentiometrically to quantify the content and confirm the Na₂HPO₄ . Spectroscopic methods, such as () , provide structural confirmation by identifying characteristic absorption bands for the phosphate group (e.g., P-O stretches at 900–1100 cm⁻¹) and absence of impurities like unreacted acid.

Chemical reactivity

Reactions with acids and bases

Disodium phosphate (Na₂HPO₄) serves as a key component in the buffer system, functioning as a in the dihydrogen phosphate (H₂PO₄⁻)/hydrogen phosphate (HPO₄²⁻) conjugate pair. This system is effective for maintaining in the range of approximately 6 to 8, centered around the pKₐ₂ value of , which is 7.2 at 25°C. The buffering capacity arises from the equilibrium: \ceH2PO4−⇌HPO42−+H+\ce{H2PO4^- ⇌ HPO4^2- + H^+} with a pKₐ of 7.2, allowing Na₂HPO₄ to resist pH changes by accepting protons to form H₂PO₄⁻ or donating them to form HPO₄²⁻. In reactions with acids, disodium phosphate undergoes protonation to yield monosodium phosphate. For example, treatment with hydrochloric acid proceeds as: \ceNa2HPO4+HCl−>NaH2PO4+NaCl\ce{Na2HPO4 + HCl -> NaH2PO4 + NaCl} This acid-base neutralization shifts the phosphate speciation toward the more acidic form, H₂PO₄⁻, and is commonly used to adjust buffer compositions or prepare specific phosphate salts. Conversely, reactions with bases involve to form . Addition of results in: \ceNa2HPO4+NaOH−>Na3PO4+H2O\ce{Na2HPO4 + NaOH -> Na3PO4 + H2O} This process converts HPO₄²⁻ to PO₄³⁻, increasing the solution's basicity and altering the ionic composition for applications requiring higher environments. The of disodium phosphate in aqueous solutions is influenced by pH-dependent of ions, as shifts in state change the prevailing ionic forms (H₂PO₄⁻, HPO₄²⁻, or PO₄³⁻) and their interactions with sodium counterions. At lower pH, to H₂PO₄⁻ enhances due to reduced charge repulsion, while higher pH favors PO₄³⁻ formation, potentially decreasing through increased effects.

Thermal decomposition

Disodium phosphate, typically encountered as a hydrate such as the dodecahydrate (Na₂HPO₄·12H₂O) or heptahydrate, undergoes initial through , where it loses molecules to form the Na₂HPO₄. This process begins around 100 °C and proceeds stepwise, with significant mass loss observed up to approximately 120 °C in dry conditions, corresponding to the release of up to 12 molecules per in the fully hydrated form. Upon further heating in the range of 250–350 °C, disodium phosphate undergoes via intermolecular condensation, primarily yielding and . The key reaction is represented as: 2Na2HPO4→Na4P2O7+H2O2 \mathrm{Na_2HPO_4} \rightarrow \mathrm{Na_4P_2O_7} + \mathrm{H_2O} This transformation involves a mass loss of about 2.5% due to elimination and is detectable starting around 232 °C, becoming rapid near 321 °C under inert or dry atmospheres. At higher temperatures around 300–600 °C, the products can further condense to form sodium polyphosphates or sodium metaphosphate (NaPO₃), with conversions observed up to 593 depending on heating duration, peak temperature, and conditions. The kinetics of these steps are influenced by environmental conditions, particularly the atmosphere. In dry or inert atmospheres, and condensation proceed more readily at lower onset temperatures compared to humid conditions, where represses initiation by elevating the required dissociation pressure, thus delaying the reaction and potentially altering product distribution toward metaphosphates. Oxidative atmospheres show minimal deviation from inert ones for these inorganic processes, as no combustible volatiles are produced, though humidity remains the dominant factor affecting rates.

Applications

Food and beverage industry

Disodium phosphate serves as a multifunctional in the food and beverage industry, primarily functioning as a regulator, emulsifier, and stabilizer to enhance product quality and shelf life. It is recognized as (GRAS) by the U.S. (FDA) for use in accordance with good manufacturing practices, allowing its incorporation in various processed foods without specific numerical limits in many categories. In the , it is approved as E339(ii) under Regulation (EC) No 1333/2008, with maximum permitted levels expressed as (P₂O₅) equivalents, typically ranging from (as needed) to 5,000 mg/kg in select categories. As a pH regulator and emulsifier, disodium phosphate is commonly added to dairy products such as evaporated and condensed milk to prevent protein coagulation and gelation during processing and storage, maintaining smooth texture and stability. In evaporated milk, it acts as a buffer to inhibit unwanted thickening by sequestering calcium ions and adjusting pH, typically at levels up to 1,000 mg/kg. Similarly, in processed cheeses and cream-based products, it stabilizes emulsions by promoting even fat distribution and preventing separation, with usage often limited to 0.5–1% by weight in dairy formulations to achieve optimal meltability and consistency. In processed meats like sausages and cured products, it functions as an emulsifier to bind water and fats, improving tenderness and yield while controlling pH to inhibit microbial growth, authorized at up to 5,000 mg/kg in the EU. Disodium phosphate also acts as an anti-caking agent in powdered foods, absorbing to ensure free-flowing properties and prevent clumping. It is incorporated into powders and dry mixes, such as or seasoning blends, at low concentrations to maintain pourability during handling and storage. Nutritionally, disodium phosphate contributes , an essential mineral for health and , serving as a fortificant in some formulations while complying with regulatory intake guidelines. Its GRAS status underscores its safety for these applications when used within approved parameters.

Pharmaceutical and medical uses

Disodium phosphate, typically in combination with , serves as an osmotic in oral solutions for bowel evacuation prior to procedures such as . It functions by drawing water into the intestines osmotically, which softens stool and stimulates bowel movements to cleanse the colon effectively. The typical dosage for adults is 20–30 grams of sodium phosphates dissolved in water, administered in divided doses the day before the procedure, accompanied by substantial clear fluid intake to prevent . Rectal enemas containing disodium phosphate are also used for similar purposes, providing rapid relief from or preparation for diagnostic exams. Following a voluntary recall of the over-the-counter Fleet Phospho-Soda brand due to risks of , the U.S. added black box warnings in 2009 for oral products, contraindicating their use in patients over 55 years old, with , , or , and requiring careful medical supervision. Generic oral solutions remain available over-the-counter with these warnings, while prescription tablet forms like OsmoPrep are used. Disodium phosphate-based laxatives have been employed in medical practice since the late , with products like Fleet Phospho-Soda introduced around 1869. These formulations demonstrate high efficacy for short-term bowel preparation, achieving adequate cleansing in over 90% of cases when used as directed. However, misuse or overuse can lead to imbalances, including and , particularly in vulnerable patients such as the elderly or those with renal impairment. In medical settings, disodium phosphate is incorporated into intravenous phosphate replacement therapies to treat or prevent , a condition characterized by low serum levels that can arise from , renal disorders, or critical illness. Administered as part of balanced solutions, it helps replenish stores while monitoring for or sodium overload, with dosing guided by serum levels—often 0.08–0.16 mmol/kg over several hours. Oral supplements containing disodium phosphate may be prescribed for milder cases, though potassium-based alternatives are sometimes preferred to avoid excess sodium intake.

Industrial applications

Disodium phosphate serves as a key agent in , particularly for softening and preventing scale formation in boilers and cooling systems. It functions by precipitating calcium and magnesium ions as insoluble phosphates, such as (Ca5(PO4)3OH), which forms a softer, more dispersible deposit than traditional scales, thereby reducing buildup on surfaces. This precipitation mechanism, often part of coordinated programs, maintains pH between 8.3 and 10.5, inhibits , and enhances overall system efficiency in applications like power generation and . Additionally, disodium phosphate acts as a buffer and sequestering agent to control ions at low concentrations (typically 2–10 ppm), preventing their redeposition in cooling towers. In the production of detergents and cleaners, disodium phosphate acts as a builder that enhances the effectiveness of by softening water through of calcium and magnesium ions, suspending soil particles, and preventing dirt redeposition on surfaces during cleaning. This role improves overall cleaning performance in industrial formulations, such as and products, where it contributes to better grease and . However, its use has declined significantly since the due to environmental concerns over phosphate contributions to , with voluntary industry reductions in detergent content beginning around 1970 and leading to widespread bans or restrictions by the . At its peak in the mid-20th century, phosphates like disodium phosphate comprised a major portion of builder formulations, accounting for up to 20% of inputs to surface waters from detergents, which fueled algal blooms and oxygen depletion in lakes and rivers. Beyond and cleaning, disodium phosphate finds application as a in textiles, where it promotes char formation and inhibits by releasing and forming protective layers upon heating. It is incorporated into fireproofing compounds for fabrics, wood, and paper, often in combination with other phosphates or borates to enhance durability and reduce flammability in industrial settings like and protective . In processes, disodium phosphate serves as a buffering agent to stabilize in baths, ensuring uniform metal deposition; for instance, it is mixed with diammonium hydrogen phosphate in solutions to maintain optimal acidity and prevent precipitation of metal complexes. This buffering action supports consistent coating quality in applications such as and automotive .

Safety and environmental impact

Toxicity and health effects

Disodium phosphate exhibits low acute mammalian toxicity, with an oral LD50 of 17,000 mg/kg in rats, indicating it is not highly poisonous when ingested in moderate amounts. However, it acts as an irritant upon direct contact, causing eye irritation, mild redness, and discomfort if as dust or fumes. Inhalation exposure in industrial settings can lead to coughing or due to its alkaline nature, though no specific inhalation LC50 data is available for mammals. Chronic exposure to disodium phosphate, primarily through oral as a , is generally safe at low levels but poses risks for individuals with renal impairment, where it can contribute to by elevating serum phosphate levels and disrupting calcium-phosphate balance. High oral doses, such as those used historically as a , may induce osmotic by drawing water into the intestines, leading to gastrointestinal upset including and . In patients with , even dietary phosphate from additives like disodium phosphate has been linked to worsened outcomes, including vascular , though this effect is more pronounced in those with impaired phosphate excretion. Animal studies demonstrate no evidence of carcinogenicity from disodium phosphate or related inorganic phosphates, with no tumors observed in long-term bioassays. Subchronic trials in rats and rabbits at high doses (e.g., ≥580 mg /kg-day) revealed mild renal effects like and increased weight, alongside gastrointestinal irritation, but no severe systemic at levels relevant to dietary exposure. These findings underscore its low overall hazard profile when handled appropriately, though vulnerable populations require monitoring for accumulation.

Regulatory status

Disodium phosphate is recognized as (GRAS) by the U.S. (FDA) for use as a direct when employed in accordance with good manufacturing practices, as specified in 21 CFR 182.6290. In the , it is authorized as the E339(ii) under Regulation (EC) No 1333/2008, with maximum permitted levels outlined in Annex II; for instance, up to 5 g/kg (expressed as P₂O₅) is allowed in certain preparations to function as an acidity regulator, stabilizer, or sequestrant. The Commission's General Standard for Food Additives (CODEX STAN 192-1995) similarly approves disodium phosphate under INS 339(ii) for use in food categories such as products at levels up to 5 g/kg (as P₂O₅) or under good manufacturing practices where no specific limit applies. For pharmaceutical applications, dibasic sodium phosphate is subject to the (USP) monograph, which defines purity standards (not less than 98.0% and not more than 100.5% of Na₂HPO₄ on a dried basis) and specifications for its use in injectable solutions, buffering agents, and other medicinal formulations. However, when formulated as a (often in combination with monobasic sodium phosphate), the FDA issues warnings against its over-the-counter use in children under 18 years and in elderly adults over 65 years without physician oversight, due to elevated risks of , imbalances, and . Environmentally, the European Union's Detergents Directive, evolving from post-1980s measures like Directive 73/404/EEC and strengthened by Regulation (EU) No 259/2012, restricts phosphates—including —in household detergents to combat in water bodies, limiting total to 0.5 g per wash load for laundry detergents and 0.3 g for automatic dishwashers. In the United States, the Environmental Protection Agency (EPA) lacks a federal effluent standard for but endorses site-specific National Pollutant Discharge Elimination System (NPDES) permits that commonly enforce total limits of 1 mg/L or lower in discharges to sensitive waters, promoting advanced treatment technologies to curb . As of 2025, regulatory frameworks for disodium phosphate remain stable without significant alterations, though international initiatives under the Environment Programme's Global Partnership on intensify focus on sustainable phosphate use, urging reduced nutrient runoff to support (life below water) through better and efficiency practices.

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  52. https://chemical-sales.com/articles/Electroplating-Nickel-Plating-Gold-Plating-Chrome-Plating-Plating-Process-Coating-Thickness-Corrosion-Resistance-Plating-Adhesion-Electrolyte-Current-Density
  53. https://www.innophos.com/-/media/innophos-com/customer-center-files/phosphates/public/unique/001/dspa-sds.pdf
  54. https://pmc.ncbi.nlm.nih.gov/articles/PMC3278747/
  55. https://hhpprtv.ornl.gov/issue_papers/Sodiumsaltsofinorganicphosphates.pdf
  56. https://eur-lex.europa.eu/legal-content/EN/TXT/HTML/?uri=CELEX:02008R1333-20240602
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