   # Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid–base properties. a. Ag 3 PO 4 , K sp = 1.8 × 10 −18 b. CaCO 3 , K sp = 8.7 × 10 −9 c. Hg 2 Cl 2 , K sp = 1.1 × 10 −18 (Hg 2 2+ is the cation in solution.) ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 15, Problem 27E
Textbook Problem
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## Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid–base properties.a. Ag3PO4, Ksp = 1.8 × 10−18b. CaCO3, Ksp = 8.7 × 10−9c. Hg2Cl2, Ksp = 1.1 × 10−18 (Hg22+ is the cation in solution.)

(a)

Interpretation Introduction

Interpretation: The solubility product of Ag3PO4,CaCO3, and Hg2Cl2 is given. By using these values, the solubility (in mol/L ) of Ag3PO4,CaCO3, and Hg2Cl2 is to be calculated.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated as,

Ksp=[A]x[B]y

Where,

• x is coefficient of concentration of A .
• y is coefficient of concentration of B .

### Explanation of Solution

Explanation

To determine: The solubility of Ag3PO4 (in mol/L ) from the given Ksp value.

The solubility of Ag3PO4 is 1.6×105mol/L_ .

Given

Solubility product of Ag3PO4 is 1.8×1018 .

Since, solid Ag3PO4 is placed in contact with water. Therefore, compound present before the reaction is Ag3PO4 and H2O . The dissociation reaction of Ag3PO4 is,

Ag3PO4(s)3Ag+(aq)+PO43(aq)

Since, Ag3PO4 does not dissolved initially, hence,

[Ag+]initial=[PO43]initial=0

The solubility of Ag3PO4 can be calculated from the concentration of ions at equilibrium.

It is assumed that smol/L of solid is dissolved to reach the equilibrium. The meaning of 3:1 stoichiometry of salt is,

smol/LAg3PO43smol/LAg++smol/LPO43

Make the ICE table for the dissociation reaction of Ag3PO4

(b)

Interpretation Introduction

Interpretation: The solubility product of Ag3PO4,CaCO3, and Hg2Cl2 is given. By using these values, the solubility (in mol/L ) of Ag3PO4,CaCO3, and Hg2Cl2 is to be calculated.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated as,

Ksp=[A]x[B]y

Where,

• x is coefficient of concentration of A .
• y is coefficient of concentration of B .

(c)

Interpretation Introduction

Interpretation: The solubility product of Ag3PO4,CaCO3, and Hg2Cl2 is given. By using these values, the solubility (in mol/L ) of Ag3PO4,CaCO3, and Hg2Cl2 is to be calculated.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated as,

Ksp=[A]x[B]y

Where,

• x is coefficient of concentration of A .
• y is coefficient of concentration of B .

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