Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) AgBr

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Identify the solubility of AgBr in water and how it might change in an acidic solution. AgBr is a slightly soluble salt in water, but its solubility can increase in acidic solutions due to the reaction of its anion with the hydrogen ions (H+) present in the acid.

Write the dissolution reaction of AgBr in water: AgBr(s) ⇌ Ag+(aq) + Br-(aq).

Consider the common ions in an acidic solution, mainly H+. The bromide ion (Br-) can react with H+ to form hydrogen bromide (HBr), which is a soluble gas.

Write the reaction of Br- with H+ in an acidic solution: Br-(aq) + H+(aq) → HBr(g).

Combine the dissolution reaction and the reaction with H+ to write the net ionic equation for the dissolution of AgBr in an acidic solution: AgBr(s) + H+(aq) → Ag+(aq) + HBr(g).

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주요 개념

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Solubility and pH

The solubility of certain compounds can be affected by the pH of the solution. In acidic solutions, the concentration of hydrogen ions (H+) increases, which can shift equilibria and enhance the solubility of some salts, particularly those containing basic anions that can react with H+.

Common Ion Effect

The common ion effect describes how the solubility of a salt decreases in a solution that already contains one of its constituent ions. In acidic solutions, the presence of H+ can influence the solubility of salts like AgBr by shifting the dissolution equilibrium, potentially increasing solubility if the anion reacts with H+.

Net Ionic Equations

A net ionic equation represents the actual chemical species that are involved in a reaction, excluding spectator ions. For dissolution reactions, it shows the ions produced when a compound dissolves in solution, allowing for a clearer understanding of the chemical processes occurring, especially in the context of solubility changes.