Chapter 6, Problem 6.21P

(a)

Interpretation Introduction

Interpretation:

The concentration of ${\text{Hg}}_{\text{2}}^{\text{2+}}\text{and}{\text{IO}}_{\text{3}}^{\text{-}}$ in a saturated solution of $H{g}_2{\left(I{O}_3\right)}_2$ has to be found.

Concept-Introduction:

Acid–base titration: It consists of a neutralization reaction where a measured volume of a known concentrated an acid or a base is used for determining the concentration of an unknown solution of base or acid with known volume.  The known concentrated solution is called the titrant, while the unknown concentrated solution is called the analyte.

Molarity: The concentration for solutions is expressed in terms of molarity as follows,

  $\text{M = }\frac{n}{\text{V}}$

  Where, M is molarity; n is moles of solute; and V is volume in L.

(b)

Interpretation Introduction

Interpretation:

The concentration of ${\text{Hg}}_{\text{2}}^{\text{2+}}$ in $0.010M$ a solution of $KI{O}_3$ saturated with $H{g}_2{\left(I{O}_3\right)}_2$ has to be found.

Concept-Introduction:

Acid–base titration: It consists of a neutralization reaction where a measured volume of a known concentrated an acid or a base is used for determining the concentration of an unknown solution of base or acid with known volume.  The known concentrated solution is called the titrant, while the unknown concentrated solution is called the analyte.

Molarity: The concentration for solutions is expressed in terms of molarity as follows,

  $\text{M = }\frac{n}{\text{V}}$

  Where, M is molarity; n is moles of solute; and V is volume in L.