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

Verified step by step guidance

1. 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.
2. Write the dissolution reaction of AgBr in water: AgBr(s) ⇌ Ag+(aq) + Br-(aq).
3. 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.
4. Write the reaction of Br- with H+ in an acidic solution: Br-(aq) + H+(aq) → HBr(g).
5. 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).

Key Concepts

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.