   Chapter 16, Problem 28E

Chapter
Section
Textbook Problem

# Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid–base properties.a. PbI2, Ksp = 1.4 × 10−8b. CdCO3, Ksp = 5.2 × 10−12c. Sr3(PO4)2, Ksp = 1 × 10−31

(a)

Interpretation Introduction

Interpretation: The solubility product of PbI2,CdCO3, and Sr3(PO4)2 is given. By using these values, the solubility (in mol/L ) of PbI2,CdCO3, and Sr3(PO4)2 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

Explanation

To determine: The solubility of PbI2 (in mol/L ) from the given Ksp value.

The solubility of PbI2 is 1.5×103mol/L_ .

Given

Solubility product of PbI2 is 1.4×108 .

Since, solid PbI2 is placed in contact with water. Therefore, compound present before the reaction is PbI2 and H2O . The dissociation reaction of PbI2 is,

PbI2(s)Pb2+(aq)+2I(aq)

Since, PbI2 does not dissolved initially, hence,

[Pb2+]initial=[I]initial=0

The solubility of PbI2 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 1:2 stoichiometry of salt is,

smol/LPbI2smol/LPb2++2smol/LI

Make the ICE table for the dissociation reaction of PbI2

(b)

Interpretation Introduction

Interpretation: The solubility product of PbI2,CdCO3, and Sr3(PO4)2 is given. By using these values, the solubility (in mol/L ) of PbI2,CdCO3, and Sr3(PO4)2 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 PbI2,CdCO3, and Sr3(PO4)2 is given. By using these values, the solubility (in mol/L ) of PbI2,CdCO3, and Sr3(PO4)2 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 .

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 