   # Assuming that the solubility of Ca 3 (PO 4 ) 2 ( s ) is 1.6 × 10 −7 mol/L at 25°c, calculate the K sp for this salt. Ignore any potential reactions of the ions with water. ### 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 93CWP
Textbook Problem
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## Assuming that the solubility of Ca3(PO4)2(s) is 1.6 × 10−7 mol/L at 25°c, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.

Interpretation Introduction

Interpretation: The Ksp value of Ca3(PO4)2 is to be calculated.

Concept introduction: Solubility product is defined as the mathematical product of the dissolved ion concentration of a substance raised to the power of its stoichiometric coefficients. When sparingly soluble ionic compound releases ions in the solution, it gives relevant solubility product. The solvent is generally water. Precipitate formation takes place in solution if ionic product is greater than the solubility product.

### Explanation of Solution

Explanation

To determine: The Ksp value of Ca3(PO4)2 .

Given:

The solubility of Ca3(PO4)2 is 1.6×107 mol/L .

The salt Ca3(PO4)2 dissolves according to the equilibrium given below.

Ca3(PO4)2(s)3Ca2+(aq)+2PO43(aq)

The solubility product expression of Ca3(PO4)2 is,

Ksp=[3Ca2+]3[2PO43-]2

Where,

• Ksp is the solubility product of Ca3(PO4)2

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