Chapter 17.6, Problem 1PE

(a)

Interpretation Introduction

Interpretation:

From the given data, the molar solubility of $\text{AgBr}$ dissolved in pure water has to be calculated.

Concept introduction:

• Molar solubility is defined as amount of solute that can be dissolved in one litre of solution before it attains saturation.
• Solubility of a compound is expressed as concentration of its ions in saturated solution.
• The solubility product constant (${\text{K}}_{\text{sp}}$) is defined as the equilibrium between compound and its ions in an aqueous solution.
• Solubility product is the multiplication of concentration of dissolved ion, raised to the power of coefficients.

  For ionic compound ${\text{A}}_{\text{3}}\text{B}$, ${\text{K}}_{\text{sp}}\text{=}{\left[\text{A}\right]}^{\text{3}}\left[\text{B}\right]$.

(b)

Interpretation Introduction

Interpretation:

From the given data, the molar solubility of $\text{AgBr}$ dissolved in $\text{0}\text{.0010 M NaBr}$ has to be calculated.

Concept introduction:

• Molar solubility is defined as amount of solute that can be dissolved in one litre of solution before it attains saturation.
• Solubility of a compound is expressed as concentration of its ions in saturated solution.
• The solubility product constant (${\text{K}}_{\text{sp}}$) is defined as the equilibrium between compound and its ions in an aqueous solution.
• Solubility product is the multiplication of concentration of dissolved ion, raised to the power of coefficients.

  For ionic compound ${\text{A}}_{\text{3}}\text{B}$, ${\text{K}}_{\text{sp}}\text{=}{\left[\text{A}\right]}^{\text{3}}\left[\text{B}\right]$.