Pyrophosphate, Sodium pyrophosphate, Tetrasodium pyrophosphate (anhydrous), TSPP
3D model (JSmol)
|E number||E450(iii) (thickeners, ...)|
|Molar mass||265.90 g·mol−1|
|Appearance||Colorless or white crystals|
|Melting point|| 988 °C (1,810 °F; 1,261 K) (anhydrous) |
79.5 °C (decahydrate)
|2.61 g/100 mL (0 °C) |
6.7 g/100 mL (25 °C)
42.2 g/100 mL (100 °C)
|Solubility||insoluble in ammonia, alcohol|
Refractive index (nD)
Heat capacity (C)
|241 J/mol K|
|270 J/mol K|
Std enthalpy of
Gibbs free energy (ΔfG˚)
|US health exposure limits (NIOSH):|
|TWA 5 mg/m3|
IDLH (Immediate danger)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Tetrasodium pyrophosphate, also called sodium pyrophosphate, tetrasodium phosphate or TSPP, is a colorless transparent crystalline chemical compound with the formula Na4P2O7. It is a salt composed of pyrophosphate and sodium ions. Toxicity is approximately twice that of table salt when ingested orally. There is also a hydrated form, Na4P2O7 · 10(H2O).
Tetrasodium pyrophosphate is used as a buffering agent, an emulsifier, a dispersing agent, and a thickening agent, and is often used as a food additive. Common foods containing tetrasodium pyrophosphate include chicken nuggets, marshmallows, pudding, crab meat, imitation crab, canned tuna, and soy-based meat alternatives and cat foods and cat treats where it is used as a palatability enhancer.
In toothpaste and dental floss, tetrasodium pyrophosphate acts as a tartar control agent, serving to remove calcium and magnesium from saliva and thus preventing them from being deposited on teeth. Tetrasodium pyrophosphate is used in commercial dental rinses before brushing to aid in plaque reduction.
Tetrasodium pyrophosphate is sometimes used in household detergents to prevent similar deposition on clothing, but due to its phosphate content it causes eutrophication of water, promoting algae growth.
Tetrasodium pyrophosphate is produced by the reaction of furnace-grade phosphoric acid with sodium carbonate to form disodium phosphate, which is then heated to 450 °C to form tetrasodium pyrophosphate.
Alternatively, it can be created by the molecular dehydration of dibasic sodium phosphate at 500 °C (932 °F).
- CDC - NIOSH Pocket Guide to Chemical Hazards
- "NIOSH Pocket Guide to Chemical Hazards #0606". National Institute for Occupational Safety and Health (NIOSH).
- Handbook of food toxicology, S. S. Deshpande, page 260
- D.L. Perry S.L. Phillips (1995) Handbook of inorganic compounds CRC Press ISBN 0-8493-8671-3