   # The K sp for silver sulfate (Ag 2 SO 4 ) is 1.2 × 10 −5 . Calculate the solubility of silver sulfate in each of the following. a. water b. 0.10 M AgNO 3 c. 0.20 M K 2 SO 4 . ### 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 39E
Textbook Problem
16 views

## The Ksp for silver sulfate (Ag2SO4) is 1.2 × 10−5. Calculate the solubility of silver sulfate in each of the following.a. waterb. 0.10 M AgNO3c. 0.20 M K2SO4.

(a)

Interpretation Introduction

Interpretation: The solubility product of Ag2SO4 is given. By using this value, the solubility of Ag2SO4 is to be calculated for each given conditions.

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 Ag2SO4 in water.

The solubility of Ag2SO4 in water is 0.0144mol/L_ .

Given

Solubility product of Ag2SO4 is 1.2×105 .

Since, solid Ag2SO4 is placed in contact with water. Therefore, compound present before the reaction is Ag2SO4 and H2O . The dissociation reaction of Ag2SO4 is,

Ag2SO4(s)2Ag+(aq)+SO42(aq)

Since, Ag+ does not dissolved initially, hence,

[Ag+]initial=[SO42]initial=0

The solubility of Ag2SO4 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 2:1 stoichiometry of salt is,

smol/LAg2SO42smol/LAg++smol/LSO42

Make the ICE table for the dissociation reaction of Ag2SO4

(b)

Interpretation Introduction

Interpretation: The solubility product of Ag2SO4 is given. By using this value, the solubility of Ag2SO4 is to be calculated for each given conditions.

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 Ag2SO4 is given. By using this value, the solubility of Ag2SO4 is to be calculated for each given conditions.

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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