   Chapter 17, Problem 86GQ

Chapter
Section
Textbook Problem

If you place 5.0 mg of SrSO4 in 1.0 L of pure water, will all of the salt dissolve before equilibrium is established, or will some salt remain undissolved?

Interpretation Introduction

Interpretation:

From Ksp value SrSO4, whether all 5 mg Strontium sulphate placed in 1 L of water will dissolve or not has to be predicted.

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

Solubility product constant Ksp for SrSO4 is 3.4×107.

Amount of strontium sulphate dissolved in 1 L of water is 5 mg.

SrSO4 Dissociates as follows in water,

SrSO4(s)Sr2+(aq)+SO42(aq)

The expression for Ksp,

Ksp=[Sr2+][SO42] (1)

The ICE table (1) is as follows,

EquationSrSO4(s)Sr2+(aq)+SO42(aq)Initial (M)00Change (M)+s+sEquilibrium (M) ss

Here, s is the molar solubility of strontium sulphate.

Substitute value of the concentration of lead and sulphate ions in equation (1) from the table

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