   Chapter 17, Problem 53PS

Chapter
Section
Textbook Problem

The Ksp value for radium sulfate, RaSO4, is 4.2 × 10−11. If 25 mg of radium sulfate is placed in 1.00 × 102 mL of water, does all of it dissolve? If not, how much dissolves?

Interpretation Introduction

Interpretation:

From Ksp value for RaSO4, all 25 mg radium sulphate placed in 1.0×102ml of water will dissolve or not has to be predicted. Also the amount of RaSO4 dissolved has to be calculated.

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 RaSO4 is 4.2×1011.

Amount of radium sulphate dissolved in 1.0×102ml is 25 mg.

RaSO4 dissociates as follows in water,

RaSO4(s)Ra2+(aq)+SO42(aq)

The expression for Ksp,

Ksp=[Ra2+][SO42] (1)

The ICE table (1) is as follows,

EquationRaSO4(s)Ra2+(aq)+SO42(aq)Initial (M)00Change (M)+s+sEquilibrium (M) ss

Here, s is the molar solubility of RaSO4

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