For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS (b) PbF₂ (c) AuCl₃ (e) CuBr (d) Hg₂C₂O₄.

Verified step by step guidance

1. Identify the slightly soluble salt: Hg2C2O4 is mercury(I) oxalate.
2. Recognize that a strong acid will react with the anion of the salt. In this case, the oxalate ion (C2O4^2-) will react with the strong acid.
3. Write the dissociation equation for the slightly soluble salt: Hg2C2O4(s) ⇌ Hg2^2+(aq) + C2O4^2-(aq).
4. Consider the reaction of the oxalate ion with the strong acid (e.g., HCl): C2O4^2-(aq) + 2H+(aq) → H2C2O4(aq).
5. Combine the dissociation and the reaction with the strong acid to write the net ionic equation: Hg2C2O4(s) + 2H+(aq) → Hg2^2+(aq) + H2C2O4(aq).

Key Concepts

Solubility and Slightly Soluble Salts

Solubility refers to the ability of a substance to dissolve in a solvent, typically water. Slightly soluble salts, like Hg2C2O4, do not dissolve significantly in water, leading to limited ionization. Understanding solubility is crucial for predicting how these salts will behave in reactions, particularly with acids.

Net Ionic Equations

A net ionic equation represents the actual chemical species that are involved in a reaction, excluding spectator ions that do not participate. This simplification helps to focus on the essential changes occurring during the reaction, particularly in acid-base reactions where ions exchange or react to form new products.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) from an acid to a base. In the case of slightly soluble salts reacting with strong acids, the acid can often protonate the anions of the salt, leading to the formation of soluble products. Understanding this interaction is key to writing accurate net ionic equations for such reactions.