   Chapter 17, Problem 83GQ

Chapter
Section
Textbook Problem

Rank the following compounds in order of increasing solubility in water Na2CO3, BaCO3, Ag2CO3.

Interpretation Introduction

Interpretation:

Using Ksp values, the given salts in order of increasing solubility in water has to be arranged.

Concept introduction:

The solubility of a salt is defined as the maximum amount of salt that can be dissolved in definite amount of solvent. It is expressed in moles per liter or grams per liter. Solubility in terms of moles per liter is called molar solubility and is defined as the number of moles of solute (salt) dissolved in per liter of solution.

Solubility product constant Ksp is an equilibrium constant and is defined as the product of the equilibrium concentration of the ions of the salt raised to the power of their coefficients in the balanced chemical equation.

The expression for Ksp of a salt is given as,

AxBy(s)xAy+(aq)+yBx(aq)Ksp=[Ay+]x[Bx]y

Explanation

Refer to the Appendix J in the textbook for the value of Ksp.

Solubility product constant Ksp for Na2CO3 is 4.89×102 .

ICE table (1) for Na2CO3 is as follows.

EquationNa2CO3(s)2Na+(aq)+CO32(aq)Initial (M)00Change (M)+2s+sEquilibrium (M) 2ss

Ksp=[Na+]2[CO32]=(2s2)(s)=4s3

Solubility of Na2CO3 is,

s=Ksp43=(4.89×102)43=0.23 molL1

Solubility product constant Ksp for BaCO3 is 2.6×109 .

ICE table (2) for BaCO3 is as follows.

EquationBaCO3(s)Ba2+(aq)+CO32(aq)Initial (M)00Change (M)+s+sEquilibrium (M) ss

Ksp=[Ba2+][CO32]=(s)(s)=s2

Solubility of BaCO3 is,

s=Ksp=2

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