Potassium bisulfate

Potassium bisulfate
Names
	IUPAC name Potassium hydrogen sulfate
	Other names Potassium acid sulfate
Identifiers
CAS Number	7646-93-7 ;
3D model (JSmol)	Interactive image;
ChemSpider	56396 ;
ECHA InfoCard	100.028.722
EC Number	231-594-1;
E number	E515(ii) (acidity regulators, ...)
PubChem CID	516920;
RTECS number	TS7200000;
UNII	1J1K03241F ;
UN number	2509
CompTox Dashboard (EPA)	DTXSID8047715 ;
	InChI InChI=1S/K.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 Key: CHKVPAROMQMJNQ-UHFFFAOYSA-M ; InChI=1/K.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 Key: CHKVPAROMQMJNQ-REWHXWOFAH;
	SMILES OS(=O)(=O)[O-].[K+];
Properties
Chemical formula	KHSO4
Molar mass	136.169 g/mol
Appearance	colorless solid
Odor	odorless
Density	2.245 g/cm3
Melting point	197 °C (387 °F; 470 K)
Boiling point	300 °C (572 °F; 573 K) (decomposes)
Solubility in water	36.6 g/100 mL (0 °C) ; 49 g/100 mL (20 °C) ; 121.6 g/100 mL (100 °C)
Solubility	soluble in acetone, ethanol.
Magnetic susceptibility (χ)	−49.8·10−6 cm3/mol
Thermochemistry
Std enthalpy of; formation (ΔfH⦵298)	-1163.3 kJ/mol
Hazards
Safety data sheet	External MSDS
EU classification (DSD) (outdated)	Corrosive (C)
R-phrases (outdated)	R34, R36, R37, R38
S-phrases (outdated)	(S1/2), S26, S36/37/39, S45
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	2340 mg*kg−1
Related compounds
Related compounds	Potassium sulfate; Sodium bisulfate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Potassium bisulfate is an inorganic compound with the chemical formula KHSO₄ and is the potassium acid salt of sulfuric acid. It is a white, water-soluble solid.

Preparation

More than 1 million tons were produced in 1985 as the initial stage in the Mannheim process for producing potassium sulfate. The relevant conversion is the exothermic reaction of potassium chloride and sulfuric acid:[1][2]

KCl + H₂SO₄ → HCl + KHSO₄

Potassium bisulfate is a by-product in the production of nitric acid from potassium nitrate and sulfuric acid:[3]

KNO₃ + H₂SO₄ → KHSO₄ + HNO₃

Chemical Properties

Thermal decomposition of potassium bisulfate forms potassium pyrosulfate:[1]

2 KHSO₄ → K₂S₂O₇ + H₂O

Above 600 °C potassium pyrosulfate converts to potassium sulfate and sulfur trioxide:[4]

K₂S₂O₇ → K₂SO₄ + SO₃

Uses

Potassium bisulfate is commonly used to prepare potassium bitartrate for winemaking.[5] Potassium bisulfate is also used as a disintegrating agent in analytical chemistry or as a precursor to prepare potassium persulfate, a powerful oxidizing agent.[6]

Occurrence

Mercallite, the mineralogical form of potassium bisulfate, occurs very rarely.[7] Misenite is another more complex form of potassium bisulfate with the formula K₈H₆(SO₄)₇.

References

Washington Wiley, Harvey (1895). Principles and Practice of Agricultural Analysis: Fertilizers. Easton, PA.: Chemical Publishing Co. p. 218. Retrieved 31 December 2015. Potassium disulfate.
H. Schultz, G. Bauer, E. Schachl, F. Hagedorn, P. Schmittinger (2005). "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_039. ISBN 978-3527306732.CS1 maint: uses authors parameter (link)
Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. New York: McGraw-Hill. p. 636. ISBN 978-0070494398.
Iredelle Dillard Hinds, John (1908). Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry. New York: John Wiley & Sons. p. 547. Retrieved 31 December 2015. Potassium disulfate.
Weisblatt, Jayne; Montney, Charles B. (2006). Chemical Compounds. ISBN 978-1-4144-0453-0.
Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. New York: Academic Press. p. 392. ISBN 978-0121266011.
"Mercallite: Mineral information, data and localities". mindat.org. Retrieved 2019-05-08.

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[Washington-1] Washington Wiley, Harvey (1895). Principles and Practice of Agricultural Analysis: Fertilizers. Easton, PA.: Chemical Publishing Co. p. 218. Retrieved 31 December 2015. Potassium disulfate.

[UllmannK-2] H. Schultz, G. Bauer, E. Schachl, F. Hagedorn, P. Schmittinger (2005). "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_039. ISBN 978-3527306732.CS1 maint: uses authors parameter (link)

[HB2003-3] Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. New York: McGraw-Hill. p. 636. ISBN 978-0070494398.

[4] Iredelle Dillard Hinds, John (1908). Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry. New York: John Wiley & Sons. p. 547. Retrieved 31 December 2015. Potassium disulfate.

[5] Weisblatt, Jayne; Montney, Charles B. (2006). Chemical Compounds. ISBN 978-1-4144-0453-0.

[Georg-6] Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. New York: Academic Press. p. 392. ISBN 978-0121266011.

[7] "Mercallite: Mineral information, data and localities". mindat.org. Retrieved 2019-05-08.