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Acid salt is a class of salts that produces an acidic solution after being dissolved in a solvent. Its formation as a substance has a greater electrical conductivity than that of the pure solvent.^[1] An acidic solution formed by acid salt is made during partial neutralization of diprotic or polyprotic acids. A half-neutralization occurs due to the remaining of replaceable hydrogen atoms from the partial dissociation of weak acids that have not been reacted with hydroxide ions (OH^-) to create water molecules. Acid salt is an ionic compound consisted of an anion, contributed from a weak parent acid, and a cation, contributed from a strong parent base.

Acidic solution and examples of acid salts

Acid-base property of the resulting solution from a neutralization reaction depends on the remaining salt products. A salt containing reactive cations undergo hydrolysis by which they react with water molecules, causing deprotonation of the conjugate acids.
For example, the acid salt ammonium chloride is the main species formed upon the half neutralization of ammonia in hydrochloric acid solution^[2]:

NH₃ _(aq) + HCl _(aq) → NH₄Cl _(aq)

**Examples of acid salts:**
Names:	Structural formula:	Names:	Structural formula:
Sodium bicarbonate (NaHCO₃)		Sodium bisulfate (NaHSO₄)
Monosodium phosphate (NaH₂PO₄)		Disodium phosphate (Na₂HPO₄)

Example of acid salts^[3]
Identity:	Sodium bicarbonate	Sodium bisulfate	Monosodium phosphate	Disodium phosphate
Structural formula
Chemical formula	NaHCO ₃	NaHSO ₄	NaH ₂PO ₄	Na ₂HPO ₄
IUPAC Name	Sodium hydrogen carbonate	Sodium hydrogen sulfate	Sodium dihydrogen phosphate	Disodium hydrogen phosphate
Other name	Baking Soda Carbonic Acid Monosodium Salt	Sodium acid sulfate Bisulfate of soda	Monobasic sodium phosphate Sodium acid phosphate Sodium biphosphate	Disodium hydrogen orthophosphate Sodium phosphate dibasic disodium phosphate
Molecular Weight	84.006 g/mol	120.054 g/mol	119.976 g/mol	141.957 g/mol
Formal Charge	zero	zero	Zero	Zero
Odour	Odourless^[4]	Odourless	Odourless	Odourless^[5]
Appearance	White crystalline powder or lumps^[6]	White crystals or granules	White crystalline powder^[7]	White, hygroscopic powder^[8]
Structure	Monoclinic^[9]	triclinic (anhydrous) monoclinic (monohydrate)	Monoclinic crystals^[10]	Monoclinic crystals (anhydrous)^[11]
Solubility	Soluble in water Insoluble in ethanol^[9]	Soluble in water Insoluble in ammonia	Soluble in water Insoluble in ethanol or ether	Soluble in water Insoluble in ethanol
Density	2.1 g/cm³	2.742 g/cm³ (anhydrous) 1.8 g/cm³ (monohydrate)	0.5-1.2 g/cm³	1.7 g/cm³
Decomposition (through heating)	Emits acrid smoke, fumes, and carbon dioxide^[12]	Forms sodium carbonate, water, and carbon dioxide	Emits toxic fumes of phosphoxides and sodium oxide^[13]	Emits toxic fumes of phosphorus- and sodium oxides^[13]
Uses	Drug indication; treatment of metabolic acidosis Automotive Care Products Food additives	Bleaching agents Plating agents and surface treating agents Cleaning and Furnishing Care Products	Treat constipation Clean the bowel before a colonoscopy Bleaching agents	A source of phosphorus Visicol tablets are indicated for cleansing of the colon Corrosion inhibitors and anti-scaling agents

Use in food

Some acid salts such as sodium bicarbonate, NaHCO₃ are used in baking. They are found in baking soda, bread soda or cooking soda and are typically divided into low-temperature (or single-acting) and high-temperature (or double-acting) acid salts. Common low-temperature acid salts react at room temperature to produce a leavening effect. They include cream of tartar, calcium phosphate, and citrates. High-temperature acid salts produce a leavening effect during baking and are usually aluminium salts such as calcium aluminium phosphate. Some acid salts may also be found in non-dairy coffee creamers. And also disodium phosphate, Na₂HPO₄ is used in foods and monosodium phosphate, NaH₂PO₄ is used in animal feed, toothpaste and evaporated milk.

Intensity of acid

An acid with higher K_a value dominates the chemical reaction. It serves as a better contributor of proton (H⁺). A comparison between the K_a and K_b indicates the acid-base property of the resulting solution by which:

The solution is acidic if K_a > K_b. It contains a greater concentration of H⁺ ions than concentration of OH^- ions due more extensive of cation hydrolysis compared to that of anion hydrolysis.
The solution is alkali if K_a < K_b. Anions hydrolyze more than cations, causing an exceeding concentration of OH^- ions.
The solution is expected to be neutral only if K_a and K_b are identical.^[14]

Other pissible factors that could vary pH level of a solution are the relevant equilibrium constants and the additional amounts of any base or acid.

For example, in ammonium chloride solution, NH₄⁺ is the main influence for acidic solution. It has greater K_a value compared to that of water molecules; K_a of NH₄⁺ is 5.6 x 10^-10 and K_w of H₂O is 1.0 x 10^-14. This ensures its deprotonation when reacting with water, and is responsible for the ph below 7 at room temperature. Cl^- will have no affinity for H⁺ nor tendency to hydrolyze, as its K_b value is very low (K_b of Cl^- is 7.7 x 10^-21).^[15]

Hydrolysis of ammonium at room temperature produces:

NH₄⁺ _(aq) + H₂O _(aq) ⇌ NH₃ _(aq) + H₃O⁺ _(aq)

K_{\mathrm {a} }={\frac {\mathrm {[NH_{3}][H_{3}O^{+}]} }{\mathrm {[NH_{4}^{+}]} }}={\frac {K_{\mathrm {w} }}{K_{\mathrm {b} }}}

K_{\mathrm {a} }={\frac {[\mathrm {1.0x10^{-14}} ]}{\mathrm {[1.8x10^{-5}]} }}

= 5.6 x 10^-10

References

^ Cady, H. P.; Elsey, H. M. (1928). "A general definition of acids, bases, and salts". Journal of Chemical Education. 5 (11): 1425. doi:10.1021/ed005p1425. Retrieved 27 February 2018.
^ Dekock, Roger L.; Gray, Harry B. (1989). Chemical bonding and structure (Second ed.). Sausalito, California: University Science Book. pp. 97–98. ISBN 0-935702-61-X. Retrieved 8 February 2018.
^ "Sodium Bicarbonate". PubChem Compound Database. National Center for Biotechnology Information. Retrieved 2 March 2018.
^ Osol, A. and J.E. Hoover, et al. (eds.). Remington's Pharmaceutical Sciences. 15th ed. Easton, Pennsylvania: Mack Publishing Co., 1975., p. 736
^ U.S. Coast Guard, Department of Transportation. CHRIS - Hazardous Chemical Data. Volume II. Washington, D.C.: U.S. Government Printing Office, 1984-5.
^ O'Neil, M.J. (ed.). The Merck Index - An Encyclopedia of Chemicals, Drugs, and Biologicals. 13th Edition, Whitehouse Station, NJ: Merck and Co., Inc., 2001., p. 1536
^ Lewis, R.J. Sr.; Hawley's Condensed Chemical Dictionary 15th Edition. John Wiley & Sons, Inc. New York, NY 2007., p. 1153
^ Lide, D.R. CRC Handbook of Chemistry and Physics 88TH Edition 2007-2008. CRC Press, Taylor & Francis, Boca Raton, FL 2007, p. 4-90
^ ^a ^b Raton, Boca (2005). CRC Handbook of Chemistry and Physics (86th Edition Edited by David R. Lide ed.). CRC Press. p. 4-87. ISBN 0-8493-0486-5. {{cite book}}: |access-date= requires |url= (help)
^ Haynes, W.M. (ed.). CRC Handbook of Chemistry and Physics. 95th Edition. CRC Press LLC, Boca Raton: FL 2014-2015, p. 4-89
^ Somov, N.V.; Chausov, F.F.; Russ, J. (2017). "High-symmetry polymorph of anhydrous disodium hydrogen phosphate". Russian Journal of Inorganic Chemistry. 62 (2): 172–174. doi:10.1134/S0036023617020176. Retrieved 2 March 2018.
^ Sax, N.I. Dangerous Properties of Industrial Materials. 6th ed. New York, NY: Van Nostrand Reinhold, 1984., p. 2413
^ ^a ^b Wiley, John; Hoboken, NJ (2004). Sax's Dangerous Properties of Industrial Materials (11th Edition By Richard J. Lewis ed.). Wiley-Interscience. p. 3274. ISBN 0-471-47662-5. Retrieved 4 March 2018.
^ Raymond, Chang (2010). Chemistry (PDF) (tenth ed.). Americas, New York: McGraw-Hill. pp. 725–727. ISBN 0077274318. Retrieved 9 February 2018.
^ Lower, S.K., (1999). Introduction to acid-base chemistry. Chem1 Genneral Chemistry Text. Retrieved from http://www.chem1.com/acad/pdf/c1xacid1.pdf

Category:Salts Category:Acids

[1] Cady, H. P.; Elsey, H. M. (1928). "A general definition of acids, bases, and salts". Journal of Chemical Education. 5 (11): 1425. doi:10.1021/ed005p1425. Retrieved 27 February 2018.

[2] Dekock, Roger L.; Gray, Harry B. (1989). Chemical bonding and structure (Second ed.). Sausalito, California: University Science Book. pp. 97–98. ISBN 0-935702-61-X. Retrieved 8 February 2018.

[3] "Sodium Bicarbonate". PubChem Compound Database. National Center for Biotechnology Information. Retrieved 2 March 2018.

[4] Osol, A. and J.E. Hoover, et al. (eds.). Remington's Pharmaceutical Sciences. 15th ed. Easton, Pennsylvania: Mack Publishing Co., 1975., p. 736

[5] U.S. Coast Guard, Department of Transportation. CHRIS - Hazardous Chemical Data. Volume II. Washington, D.C.: U.S. Government Printing Office, 1984-5.

[6] O'Neil, M.J. (ed.). The Merck Index - An Encyclopedia of Chemicals, Drugs, and Biologicals. 13th Edition, Whitehouse Station, NJ: Merck and Co., Inc., 2001., p. 1536

[7] Lewis, R.J. Sr.; Hawley's Condensed Chemical Dictionary 15th Edition. John Wiley & Sons, Inc. New York, NY 2007., p. 1153

[8] Lide, D.R. CRC Handbook of Chemistry and Physics 88TH Edition 2007-2008. CRC Press, Taylor & Francis, Boca Raton, FL 2007, p. 4-90

[:9-9] Raton, Boca (2005). CRC Handbook of Chemistry and Physics (86th Edition Edited by David R. Lide ed.). CRC Press. p. 4-87. ISBN 0-8493-0486-5. {{cite book}}: |access-date= requires |url= (help)

[10] Haynes, W.M. (ed.). CRC Handbook of Chemistry and Physics. 95th Edition. CRC Press LLC, Boca Raton: FL 2014-2015, p. 4-89

[11] Somov, N.V.; Chausov, F.F.; Russ, J. (2017). "High-symmetry polymorph of anhydrous disodium hydrogen phosphate". Russian Journal of Inorganic Chemistry. 62 (2): 172–174. doi:10.1134/S0036023617020176. Retrieved 2 March 2018.

[12] Sax, N.I. Dangerous Properties of Industrial Materials. 6th ed. New York, NY: Van Nostrand Reinhold, 1984., p. 2413

[:13-13] Wiley, John; Hoboken, NJ (2004). Sax's Dangerous Properties of Industrial Materials (11th Edition By Richard J. Lewis ed.). Wiley-Interscience. p. 3274. ISBN 0-471-47662-5. Retrieved 4 March 2018.

[14] Raymond, Chang (2010). Chemistry (PDF) (tenth ed.). Americas, New York: McGraw-Hill. pp. 725–727. ISBN 0077274318. Retrieved 9 February 2018.

[15] Lower, S.K., (1999). Introduction to acid-base chemistry. Chem1 Genneral Chemistry Text. Retrieved from http://www.chem1.com/acad/pdf/c1xacid1.pdf

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Acidic solution and examples of acid salts

Use in food

Intensity of acid

See also

References