Sodium bisulfate

Sodium bisulfate

Names
IUPAC name Sodium hydrogen sulfate
Other names Sodium acid sulfate Bisulfate of soda
Identifiers
CAS Number	7681-38-1 Y 10034-88-5 (monohydrate) Y
3D model (JSmol)	Interactive image
ChemSpider	56397 Y
ECHA InfoCard	100.028.787
EC Number	231-665-7
E number	E514 (acidity regulators, ...)
PubChem CID	516919
RTECS number	VZ1860000
InChI InChI=1S/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 Y Key: WBHQBSYUUJJSRZ-UHFFFAOYSA-M Y InChI=1/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 Key: WBHQBSYUUJJSRZ-REWHXWOFAO
SMILES [Na+].[O-]S(=O)(=O)O
Properties
Chemical formula	NaHSO4
Molar mass	120.06 g/mol (anhydrous) 138.07 g/mol (monohydrate)
Appearance	white solid
Density	2.742 g/cm3 (anhydrous) 1.8 g/cm3 (monohydrate)
Melting point	58.5 °C (137.3 °F; 331.6 K) (monohydrate) 315 °C (anhydrous)
Boiling point	decomposes to Na2S2O7 (+ H2O) at 315 °C (599 °F; 588 K)
Solubility in water	28.5 g/100 mL (25 °C) 100 g/100 mL (100 °C)
Solubility	Insoluble in ammonia
Acidity (pKa)	1.99
Structure
Crystal structure	triclinic (anhydrous) monoclinic (monohydrate)
Hazards
Safety data sheet	External MSDS
R-phrases (outdated)	R34 R37 R41
S-phrases (outdated)	S26 S36 S37 S39 S45
NFPA 704	0 2 1
Flash point	Non-flammable
Related compounds
Other anions	Sodium sulfate
Other cations	Potassium bisulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is YN ?)
Infobox references

Sodium bisulfate, also known as sodium hydrogen sulfate,^[1] is the sodium salt of the bisulfate anion, with the molecular formula NaHSO₄. Sodium bisulfate is an acid salt formed by partial neutralization of sulfuric acid by an equivalent of sodium base, typically either in the form of sodium hydroxide or sodium chloride. It is a dry granular product that can be safely shipped and stored. The anhydrous form is hygroscopic. Solutions of sodium bisulfate are acidic, with a 1M solution having a pH of around 1.

Production

One production method involves mixing stoichiometric quantities of sodium hydroxide and sulfuric acid which react to form sodium bisulfate and water.

NaOH + H₂SO₄ → NaHSO₄ + H₂O

A second production method involves reacting sodium chloride (salt) and sulfuric acid at elevated temperatures to produce sodium bisulfate and hydrogen chloride gas.

NaCl + H₂SO₄ → NaHSO₄ + HCl

The liquid sodium bisulfate is sprayed and cooled so that it forms a solid bead. The hydrogen chloride gas is dissolved in water to produce hydrochloric acid as a useful coproduct of the reaction. Sodium bisulfate is also produced as a byproduct of the production of many other mineral acids via the reaction of their sodium salts with an excess of sulfuric acid:

• NaCN + H₂SO₄ → NaHSO₄ + HCN
• NaNO₃ + H₂SO₄ → NaHSO₄ + HNO₃
• NaClO₄ + H₂SO₄ → NaHSO₄ + HClO₄

In most cases, the acids produced have a lower boiling point than the reactants and are separated from the reaction mixture by distillation.

There are only two producers in the USA, one being Jones-Hamilton Co., who uses the sulfuric acid/sodium chloride process, which produces the anhydrous form. The other supplier, Jost Chemical, uses the sodium hydroxide/sulfuric acid method, which produces the monohydrate.

Uses

Sodium bisulfate is used primarily to lower pH. For technical-grade applications, it is used in metal finishing, cleaning products,^[2] and to lower the pH of water for effective chlorination in swimming pools and hot tubs. Sodium bisulfate is also AAFCO approved as a general-use feed additive, including companion animal food. It is used as a urine acidifier to reduce urinary stones in cats.

It is highly toxic to at least some echinoderms, but fairly harmless to most other life forms; sodium bisulfate is used in controlling outbreaks of crown-of-thorns starfish.

In jewelry making, sodium bisulfate is the primary ingredient used in many pickling solutions to remove the oxidation layer from surfaces, which occurs after heating.^[3] Sodium bisulfate was the primary active ingredient in crystal toilet bowl cleaners Vanish and Sani-Flush, both now discontinued.^[4]

In the textiles industry, it is sometimes applied to velvet cloth made with a silk backing and a pile of cellulose-based fiber (rayon, cotton, hemp, etc.) to create "burnout velvet": the sodium bisulfate, when applied to such a fabric and heated, causes the cellulose-based fibers to become brittle and flake away, leaving burned-out areas in the finished material, usually in attractive patterns.^[5]

Sodium bisulfate is the active ingredient in some granular poultry litter treatments used to control ammonia.^[6] Sodium bisulfate has also been shown to significantly reduce the concentration of Campylobacter and Salmonella in chicken houses.^[7]

In food

Sodium bisulfate is used as a food additive to leaven cake mixes (make them rise)^[8] as well as being used in meat and poultry processing and most recently in browning prevention of fresh-cut produce.^[9] Sodium bisulfate is considered generally recognized as safe (GRAS) by the FDA. The food-grade product also meets the requirements set out in the Food Chemicals Codex. It is denoted by E number E514ii in the EU and is also approved for use in Australia, New Zealand, Canada, and Mexico.^[10] where it is listed as additive 514. Food grade sodium bisulfate is used in a variety of food products, including beverages, dressings, sauces, and fillings. It has many synonyms including^[11] bisulfate of soda, sodium acid sulfate, mono sodium hydrogen sulfate, sodium hydrogen sulfate, sodium hydrosulfate, and sulfuric acid sodium salt (1:1).

Sodium bisulfate is considered natural by the Grocery Manufacturers Association (GMA) since it is made from minerals. No artificial or synthetic ingredients are used in the manufacturing. No covalent bonds are broken or formed in the manufacturing process, therefore it is not synthetic.^[12]

Sodium bisulfate lowers the pH without a sour taste and has been used in the place of citric, malic or phosphoric acids^[13] and can also be used as an anti-browning agent.^[14]

References

External links

• Food Chemicals Codex