Question

Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42- , Kf = 2.9×1015 . Use the pull-down boxes to specify states such as (aq) or (s).

Answer 1

The solubility of ZnCO3 (s) increases in the presence of hydroxide ions due to the formation of a complex ion. The net ionic equation for this reaction is Zn²+ (aq) + 2OH¯(aq) → Zn(OH)₂ (s), and the equilibrium constant is 2.9×10¹⁵.

Step-by-step explanation:

The solubility of ZnCO3 (s), zinc carbonate, increases in the presence of hydroxide ions due to the formation of a complex ion. The net ionic equation for this reaction is:

Zn²+ (aq) + 2OH¯(aq) → Zn(OH)₂ (s)

The equilibrium constant for this reaction is given by Kf = [Zn(OH)₄²⁻] / ([Zn²+] * [OH¯]²), which is equal to 2.9×10¹⁵.