   Chapter 16, Problem 94CWP

Chapter
Section
Textbook Problem

# Order the following solids (a–d) from least soluble to most soluble. Ignore any potential reactions of the ions with water.a. AgCl Ksp = 1.6 × 10−10b. Ag2S Ksp = 1.6 × 10−49c. CaF2 Ksp = 4.0 × 10−11d. CuS Ksp = 8.5 × 10−45

Interpretation Introduction

Interpretation: The given solids are to be arranged in the order of least soluble to most soluble.

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

Explanation

To determine: The order of least soluble to most soluble solid.

The equilibrium established between a solid and its corresponding ions in a solution is represented by solubility product constant (Ksp) . The solids that have high Ksp values are more soluble in aqueous solution as compared to the one having low Ksp values.

The given solids and their Ksp values are:

AgClKsp=1.6×1010Ag2SKsp=1.6×1049CaF2Ksp=4

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