   # What is the solubility of PbSO 4 in water at 25°C if the solution already contains 0.25 M Na 2 SO 4 ( K sp for PbSO 4 ≡ 2.5 ×10 −8 ) (a) 1.0 × 10 −7 M (b) 1.6 × 10 −4 M (c) 6.3 × 10 −9 M ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17.4, Problem 4RC
Textbook Problem
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## What is the solubility of PbSO4 in water at 25°C if the solution already contains 0.25 M Na2SO4(Ksp for PbSO4 ≡ 2.5 ×10−8) (a) 1.0 × 10−7 M (b) 1.6 × 10−4 M (c) 6.3 × 10−9 M

Interpretation Introduction

Interpretation:

Solubility of salt PbSO4 is to be calculated in pure water at 25°C and this solution already contains (0.25M)ofNa2SO4 hence correct solubility should be identified.

Concept introduction:

The solubility of a salt is defined as the maximium 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.

Expression for Ksp of a salt is given as,

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

Relation between Ksp and s is derived as follows,

EquationAxByxAy++yBxInitial(M)00Change(M)+xs+ysEquilibrium(M)xsys

Ksp=[Ay+]x[Bx]yKsp=(xs)x(ys)y=xxyy(s)x+y

Rearrange the expression for s .

(s)x+y=Kspxxyy=(Kspxxyy)1/(x+y)

Here,

• x is the coefficient of cation A+y
• y is the coefficient of anion Bx
• s is the molar solubility

Ksp is calculated by using molar solubility of the salt.

### Explanation of Solution

Solubility of salt PbSO4 in pure water is to be calculated as follows,

Given:

The value of solubility product Ksp of PbSO4 is 2.5×108 at 25°C

PbSO4 when dissolved in water dissociates as ,

PbSO4(s) Pb2+(aq)+ SO42(aq)

The ICE table is as follows,

EquationPbSO4Pb2++SO42Initial (M)00Change (M)+s+sEquilibrium (M) ss

Ksp=[

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