Consider the dissociation of strong versus weak acids: HCl (aq) + H2O (l) →H3O + (aq) + Cl - (aq) HF (aq) + H2O (l) ⇌H3O + (aq) + F - (aq) The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, F-, can react with H3O+. Now consider the solubility of insoluble salts: AgCl (s) ⇌Ag + (aq) + Cl - (aq) AgF (s) ⇌Ag + (aq) + F - (aq) The addition of acid has no effect on silver chloride. But for the second reaction, H3O + will react with F-, decreasing its concentration and driving the equilibrium to the right. Thus, salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases.

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Young

Chemistry

16 September, 10:16

Consider the dissociation of strong versus weak acids: HCl (aq) + H2O (l) →H3O + (aq) + Cl - (aq) HF (aq) + H2O (l) ⇌H3O + (aq) + F - (aq) The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, F-, can react with H3O+. Now consider the solubility of insoluble salts: AgCl (s) ⇌Ag + (aq) + Cl - (aq) AgF (s) ⇌Ag + (aq) + F - (aq) The addition of acid has no effect on silver chloride. But for the second reaction, H3O + will react with F-, decreasing its concentration and driving the equilibrium to the right. Thus, salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases.

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Grey · Answer 1

The solubility of those salts increases which contains conjugate of weak acid. Conjugate of weak acid refers to strong base such as sodium hydroxide and potassium hydroxide etc.

Explanation:

The solubility of salts in strong acidic solution increases due to the presence of conjugate of weak acid which is actually a strong base. So if the salts contain strong base, it readily react with strong acid that is present in the solution.