Chapter 6, Problem 6J.4E

(a)

Interpretation Introduction

Interpretation:

Whether a precipitate will form when 5.0 mL of 0.10 M ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}$ and 1.00 L of 0.010 M${\text{AgNO}}_{\text{3}}{}_{\text{(aq)}}$ are mixed has to be determined. (b) 3.3 mL of 1.0 M${\text{HCl}}_{\text{(aq)}}$, 4.9 mL of 0.0030 M${\text{AgNO}}_{\text{3}}{}_{\text{(aq)}}$, and enough water to dilute the solution to 50.0 mL.

Concept Introduction:

Solubility Product:

The equilibrium constant for a chemical reaction in which a solid ionic compound dissolves to yields its ions in solution is known as “solubility product”. It is denoted by ‘${\text{K}}_{\text{sp}}$’. Solubility product is also known as “ion product”.

Common ion Effect:

The decrease in solubility of an ionic compound by the addition to the solution of soluble compound contains common ion. That common ion lesser the solubility of the compound.

(a)

Interpretation Introduction

Interpretation:

Whether a precipitate will form when 3.3 mL of 1.0 M${\text{HCl}}_{\text{(aq)}}$ and 4.9 mL of 0.0030 M${\text{AgNO}}_{\text{3}}{}_{\text{(aq)}}$ are mixed has to be determined.

Concept Introduction:

Refer part (a).