Which of the following compounds are more soluble in acidic...

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 b) ${CaCO}_{3}$ c) ${Ni}({OH})_{2}$ d) ${Ca}_{3}({PO}_{4})_{2}$

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 b) ${CaCO}_{3}$
c) ${Ni}({OH})_{2}$ d) ${Ca}_{3}({PO}_{4})_{2}$

Key Concepts

Le Chatelier’s Principle

Le Chatelier’s Principle explains how a system at equilibrium responds to disturbances. In the context of solubility, when an acid is added and reacts with a basic ion, the equilibrium shifts to produce more ions from the solid phase, thus increasing its solubility. This principle helps in understanding why sparingly soluble compounds become more soluble under acidic conditions.

Net Ionic Equations

Net ionic equations condense chemical reactions to include only the ions and molecules directly involved in the reaction, omitting spectator ions. These equations are essential for clearly representing the actual chemical change, especially in reactions where acid dissolves a sparingly soluble salt by protonating one of its components.

Acid-Base Reactions and Protonation

In acidic solutions, added H? ions can react with basic anions (such as carbonate, hydroxide, or phosphate) that are present in sparingly soluble salts. This protonation reduces the effective concentration of the anions, thereby shifting the dissolution equilibrium to favor further dissolution of the solid compound.

Solubility Equilibria

Solubility equilibria involve the balance between the solid phase of a compound and its ions dissolved in solution. This concept is crucial when discussing sparingly soluble compounds, as it explains how changes in the concentration of ions, pH, or other conditions can shift the equilibrium and affect the compound's solubility.

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