Question

Write a balanced net ionic equation to show why the solubility of Zn(CN)₂(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.

I really need help with both because I am on my last attempt and cannot seem to understand exactly how to solve for K. Thank you for your help! I will be sure to rate your answer if it is correct.

Write a balanced net ionic equation to show why the solubility of Zn(CN)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pl-down boxes to pecify states such as (ag) or(o) Write a balanced net ionic equation to show why the solubility of Ca(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s)

Answer 1

Q1. The balanced net ionic equation is :

Zn(CN)₂ (s) + 2 H₃O⁺ (aq) $\rightarrow$ Zn²⁺ (aq) + 2 HCN (aq) + 2 H₂O (l)

K = 8.0 x 10¹⁶

Q2. The balanced net ionic equation is :

Ca(OH)₂ (s) + 2 H₃O⁺ (aq) $\rightarrow$ Ca²⁺ (aq) + 2 H₂O (l)

K = 7.9 x 10²²

Explanation

Q1. K = (K_sp Zn(CN)₂) / (K_w)²

K = (8.0 x 10^-12) / (1.0 x 10^-14)²

K = (8.0 x 10^-12) / (1.0 x 10^-28)

K = 8.0 x 10¹⁶

Q2. K = (K_sp Ca(OH)₂) / (K_w)²

K = (7.9 x 10^-6) / (1.0 x 10^-14)²

K = (7.9 x 10^-6) / (1.0 x 10^-28)

K = 7.9 x 10²²