Chapter 17, Problem 17.111SP

Interpretation Introduction

(a)

Interpretation:

The molar solubility of ${\text{PbCrO}}_{\text{4}}$ in pure water is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ to be an ionic compound. Its dissociation occurs as follows:

${\text{A}}_x{\text{B}}_y\rightleftharpoons x{\text{A}}^{y+}+y{\text{A}}^{x-}$

The expression for its $K_{\text{sp}}$ is as follows:

$K_{\text{sp}}={\left[{\text{A}}^{y+}\right]}^x{\left[{\text{B}}^{x-}\right]}^y$

Interpretation Introduction

(b)

Interpretation:

The molar solubility of ${\text{PbCrO}}_{\text{4}}$ in $1.0\times {10}^{-3}M$ of ${\text{K}}_2{\text{CrO}}_4$ solution is to be calculated.

Concept introduction:

Solubility product is equilibrium constant for reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by $K_{\text{sp}}$. Consider ${\text{A}}_x{\text{B}}_y$ to be an ionic compound. Its dissociation occurs as follows:

${\text{A}}_x{\text{B}}_y\rightleftharpoons x{\text{A}}^{y+}+y{\text{A}}^{x-}$

The expression for its $K_{\text{sp}}$ is as follows:

$K_{\text{sp}}={\left[{\text{A}}^{y+}\right]}^x{\left[{\text{B}}^{x-}\right]}^y$