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In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg 2+ ] 0 = 3.75 × 10 −3 [F − ] 0 = 6.25 × 10 −2 → reacts to form MgF 2 y mol/Mg 2+ [Mg 2+ ] = 3.75 × 10 −3 − y [F − ] = 6.25 × 10 −2 – 2 y

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 15, Problem 92AE
Textbook Problem
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In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where

Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L

[Mg2+]0 = 3.75 × 10−3

[F]0 = 6.25 × 10−2

reacts to form MgF 2 y mol/Mg 2+

[Mg2+] = 3.75 × 10−3y

[F] = 6.25 × 10−2 – 2y

Interpretation Introduction

Interpretation: The equilibrium concentration of [Mg2+] and [F] 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 by the formula,

Ksp=[A]x[B]y

Explanation of Solution

Explanation

To determine: The equilibrium concentration of [Mg2+] and [F] .

Refer Example 156 .

The equilibrium concentration of [Mg2+] is [3.75×103y] .

The equilibrium concentration of [F] is [6.25×1022y] .

Formula

The solubility product of MgF2 is calculated as,

Ksp=[Mg2+][F]2

Where,

  • Ksp is solubility product.
  • [Mg2+] is equilibrium concentration of Mg2+ .
  • [F] is equilibrium concentration of F .

Substitute the value of the equilibrium concentration of [F] and [Mg2+] in the above expression.

Ksp=[3.75×103y][6.25×1022y]26.4×109=[3.75×103y][(6.25×102)24(6

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Chapter 15 Solutions

Chemistry: An Atoms First Approach
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