   Chapter 16, Problem 110IP

Chapter
Section
Textbook Problem

# A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 × 10−2 atm at 25°C. Calculate the Ksp value for the salt, assuming ideal behavior.

Interpretation Introduction

Interpretation: The osmotic pressure of a saturated solution with a salt of type M3X2 is given. The solubility product of the salt is to be calculated.

Concept introduction: The solubility product is the mathematical product of a substance’s dissolved ion concentration raised to its power of its stoichiometric coefficients. When sparingly soluble ionic compound releases ions in the solution, it gives relevant solubility product. The solvent is generally water.

Explanation

Explanation

To determine: The solubility product of the salt of type M3X2 .

The solubility product of the salt of type M3X2 is 5.08×10-17M5_ .

Given

The osmotic pressure of the solution is 2.64×102atm .

Temperature is 25°C or 298K .

The equilibrium equation for the dissociation of M3X2 is as follows:

M3X2(s)3M2+(aq)+2X3(aq) .

The number of moles of M3X2 to be dissolved to reach equilibrium are considered to be x .

Initialconcentration(mol/L)[M2+]=0[X3]=0toreachequilibriumxmoles/LdissolvesEquilibriumconcentration(mol/L)[M2+]=3x[X3]=2x

The solubility product of M3X2 is calculated by the formula,

Ksp=[M2+]3[X3]2

Where,

• Ksp is the solubility product of M3X2

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