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Slaked lime, Ca(OH) 2 is used to soften hard water by removing calcium ions from hard water through the reaction Ca ( OH ) 2 ( a q ) + Ca 2+ ( a q ) +2HCO 3 − ( a q ) → 2CaCO 3 ( s ) +2H 2 O ( l ) Although CaCO 3 ( s ) is considered insoluble, some of it does dissolve in aqueous solutions. Calculate the molar solubility of CaCO 3 in water ( K sp = 8.7 × 10 −9 ).

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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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Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 19, Problem 77AE
Textbook Problem
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Slaked lime, Ca(OH)2 is used to soften hard water by removing calcium ions from hard water through the reaction

Ca ( OH ) 2 ( a q ) + Ca 2+ ( a q ) +2HCO 3 ( a q ) 2CaCO 3 ( s ) +2H 2 O ( l )

Although CaCO3(s) is considered insoluble, some of it does dissolve in aqueous solutions. Calculate the molar solubility of CaCO3 in water (Ksp = 8.7 × 10−9).

Interpretation Introduction

Interpretation: Reaction of slaked lime with calcium ion and its solubility product is given. The molar solubility of CaCO3 is to be calculated.

Concept introduction: 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.

To determine: The molar solubility of CaCO3 in water.

Explanation of Solution

Explanation

Given

The solubility product is 8.7×109 .

The given reaction is,

Ca(OH)2(aq)+Ca2+(aq)+2HCO3(aq)2CaCO3(s)+2H2O(l)

The decomposition reaction of CaCO3 in water is,

CaCO3(s)Ca2+(aq)+CO32(aq)

It is assumed that molar solubility of CaCO3 is S .

The solid components do not affect the value of the equilibrium constant.

The ICE table is formed for the decomposition reaction of CaCO3 .

CaCO3(s)Ca2+(aq)+CO32(aq)Initial(M):00Change(M):

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Chemistry: An Atoms First Approach
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