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Chapter 15: Problem 73

Define salt hydrolysis. Categorize salts according to how they affect the \(\mathrm{pH}\) of a solution.

Short Answer

Expert verified
Salt hydrolysis is the reaction where salts interact with water to form acidic or basic solutions. The effects of salts on the pH of a solution are categorized as follows: Salts from strong acids and strong bases do not affect pH; salts from strong acids and weak bases make the solution acidic (pH<7); salts from weak acids and strong bases make the solution basic (pH>7).

Step by step solution

01

Definition of Salt Hydrolysis

Salt hydrolysis is a reaction in which salts react with water to form acidic or basic solutions. This happens when a salt's positive ion (cations) or negative ion (anions), having the ability to react with water, shows acidic or basic characteristics.
02

Categorisation of Salts

There are three categories of salts based on their effect on the pH of a solution: 1) Salts from strong acids and strong bases: These salts do not hydrolyze and thus do not affect the pH of the solution. The solution remains neutral with pH=7. 2) Salts from strong acids and weak bases: These salts tend to make the solution acidic as they will be hydrolyzed to a higher degree and pH will be less than 7. 3) Salts from weak acids and strong bases: These salts make the solution basic, as their hydrolysis shifts the equilibrium to produce more hydroxide ions, making the pH greater than 7.
03

Examples

1) Salt from Strong Acid and Strong Base (Neutral): Sodium chloride (NaCl) - Results from the neutralization of hydrochloric acid (HCl) and sodium hydroxide (NaOH). There is no shift in pH. 2) Salt from Strong Acid and Weak Base (Acidic): Ammonium chloride (NH4Cl) - Results from the reaction of ammonium hydroxide (NH4OH) and hydrochloric acid (HCl). The pH will be less than 7. 3) Salt from Weak Acid and Strong Base (Basic): Sodium acetate (CH3COONa) - Aerosolized from acetic acid (CH3COOH) and sodium hydroxide (NaOH). The pH will be greater than 7.

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Most popular questions from this chapter

Specify which of the following salts will undergo hydrolysis: \(\mathrm{KF}, \mathrm{NaNO}_{3}, \mathrm{NH}_{4} \mathrm{NO}_{2}, \mathrm{MgSO}_{4}, \mathrm{KCN}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}, \mathrm{RbI}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{CaCl}_{2}, \mathrm{HCOOK}\).

What are the Lewis definitions of an acid and a base? In what way are they more general than the Brønsted definitions?

True or false? If false, explain why each statement is wrong. (a) All Lewis acids are Brønsted acids. (b) The conjugate base of an acid always carries a negative charge. (c) The percent ionization of a base increases with its concentration in solution. (d) A solution of barium fluoride is acidic.

Malonic acid \(\left[\mathrm{CH}_{2}(\mathrm{COOH})_{2}\right]\) is a diprotic acid. Compare its two \(K_{\mathrm{a}}\) values with that of acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\left(K_{\mathrm{a}}\right),\) and account for the differences in the three \(K_{\mathrm{a}}\) values.

From the relationship \(K_{\mathrm{a}} K_{\mathrm{b}}=K_{\mathrm{w}},\) what can you deduce about the relative strengths of a weak acid and its conjugate base?
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