   # A solution contains 2.0 × 10 −3 M Ce 3+ and 1.0 × 10 −2 M IO 3 3− . Will Ce(IO 3 ) 3 ( s ) precipitate? [ K sp for Ce(IO 3 ) 3 is 3.2 × 10 −10 .] ### 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 52E
Textbook Problem
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## A solution contains 2.0 × 10−3 M Ce3+ and 1.0 × 10−2 M IO33−. Will Ce(IO3)3(s) precipitate? [Ksp for Ce(IO3)3 is 3.2 × 10−10.]

Interpretation Introduction

Interpretation: The solubility product of Ce(IO3)3 and concentration of each ion Ce3+ and IO33 is given. It is to be checked that Ce(IO3)3 will precipitate out or not when two solutions are mixed.

Concept introduction: The formation of solid in a solution is known as precipitation.

Solubility product, Ksp is defined as the concentration of ions in a saturated solution where each ion is raised to the power of their coefficients. Ion product, Q is defined as the initial concentration of ions in any solution where each ion is raised to the power of their coefficients.

The relation between ion product, Q and solubility product, Ksp is as follows.

• If Ksp>Q , then no precipitate will form.
• If Ksp<Q , then precipitate will form.
• If Ksp=Q , then the solution will be in just saturation.

### Explanation of Solution

Explanation

To determine: If Ce(IO3)3 will precipitate out or not when two solutions are mixed.

The ion product of Ce(IO3)3 is 2×109_ .

Given

Initial concentration of Ce3+ is 2.0×103M .

Initial concentration of IO33 is 1.0×103M .

Solubility product of Ce(IO3)3 is 3.2×1010 .

The Ce(IO3)3 will only precipitate out if,

Ksp<Q

The reaction of Ce3+ and IO33 is,

Ce3++3IO33Ce(IO3)3

Formula

The ion product of Ce(IO3)3 is calculated as,

Q=[Ce3+]0[IO33]03

Where,

• Q is ion product

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