   Chapter 16, Problem 43E

Chapter
Section
Textbook Problem

# The solubility of Ce(IO3)3 in a 0.20-M KIO3 solution is 4.4 × 10−8 mol/L. Calculate Ksp for Ce(IO3)3.

Interpretation Introduction

Interpretation: The solubility of Ce(IO3)3 and the concentration of KIO3 solution is given. The solubility product of Ce(IO3)3 is to be calculated in the given concentration of KIO3 solution.

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 product of Ce(IO3)3 in 0.20M KIO3 .

The solubility product of Ce(IO3)3 in 0.20M KIO3 is 3.5×1010_ .

Given

Solubility of Ce(IO3)3 is 4.4×108mol/L .

Concentration of KIO3 is 0.20M .

The major species in the solution before dissociation of Ce(IO3)3 are K+,IO3 and H2O . The dissociation reaction of Ce(IO3)3 is,

Ce(IO3)3(s)Ce3+(aq)+3IO3(aq)

The ratio of moles between ions is 1:3 .

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

smol/LCe(IO3)31smol/LCe3++3smol/LIO3

The concentrations are as follows,

Initialconcentration(mol/L)Equilibriumconcentration(mol/L)[Ce3+]=0[Ce3+]=s[IO3]=0

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