Chapter 18, Problem 80IAE

Interpretation Introduction

Interpretation:

The $K_{sp}$ value of $\text{AgCN}$ should be calculated, where the solubility of $\text{AgCN}\left(s\right)$ in 0.200 M ${\text{NH}}_{\text{3}}\left(aq\right)$ is 8 $8.8\times {10}^{-6}{\text{mol L}}^{-1}$.

Concept introduction:

The formation constant, K_f, of a complex ion is the equilibrium constant that defines the formation of a complex ion. Solubility product constant is defined as an equilibrium constant for salts which are slightly soluble in an aqueous solution.

It is the amount up to which a solute can dissolve in solution. Equilibrium constant, K, for a net ionic equation can calculated with use of solubility of each equilibrium or with use of other equilibrium constants.