Question

Acetic acid is added to a solution of lithium cyanide. Write the net equation for a possible reaction and predict whether products or reactants are favored at equilibrium.

A) CH3COOH + LiCN → LiCH3COO + HCN; Products favored
B) CH3COOH + LiCN → LiCH3COO + HCN; Reactants favored
C) CH3COOH + LiCN → LiCNCH3COOH; Products favored
D) CH3COOH + LiCN → LiCNCH3COOH; Reactants favored

Answer 1

The reaction between acetic acid and lithium cyanide produces lithium acetate and hydrogen cyanide. Since both products are weak acids and acetic acid is weaker than hydrogen cyanide, the equilibrium favors the reactants. Thus, the correct answer is B) CH3COOH + LiCN → LiCH3COO + HCN; Reactants favored.

Step-by-step explanation:

When acetic acid (CH3COOH) is added to lithium cyanide (LiCN), a reaction can occur in which the acetic acid donates a proton (H+) to the cyanide ion, resulting in the formation of lithium acetate (LiCH3COO) and hydrogen cyanide (HCN). The correct net equation for this reaction is:

CH3COOH + LiCN → LiCH3COO + HCN

Acetic acid is a weak acid, and hydrogen cyanide is also a weak acid; however, HCN is slightly stronger than acetic acid. Based on this information, the equilibrium will favor the formation of reactants, because the weak acid (acetic acid) tends to retain its protons better than it donates them to form the slightly stronger acid (hydrogen cyanide). Therefore, the correct answer is:

B) CH3COOH + LiCN → LiCH3COO + HCN; Reactants favored