   # Using the following data, calculate the value of K sp for Ba(NO 3 ) 2 , one of the least soluble of the common nitrate salts. Species Δ G f o Ba 2+ ( aq ) −561 KJ/mol NO 3 − ( aq ) −109 KJ/mol Ba(NO 3 ) 2 ( s ) −797KJ/mol ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 16, Problem 87AE
Textbook Problem
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## Using the following data, calculate the value of Ksp for Ba(NO3)2, one of the least soluble of the common nitrate salts. Species Δ G f o Ba2+(aq) −561 KJ/mol NO3−(aq) −109 KJ/mol Ba(NO3)2(s) −797KJ/mol

Interpretation Introduction

Interpretation: The value of Ksp for Ba(NO3)2(s) is to be calculated from the given data.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at a certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated by the formula,

Ksp=[A]x[B]y

ΔG°=RTln(Ksp)

### Explanation of Solution

The dissociation reaction of Ba(NO3)2(s) is,

Ba(NO3)2(s)Ba2+(aq)+2NO3(aq)

Data from given table,

The value of ΔG°(kJ/mol) at 298K is,

 Molecules ΔG°(kJ/mol) Ba2+(aq) −561 NO3−(aq) −109 Ba(NO3)2(s) −797

The formula of ΔG° is,

ΔG°=npΔG°(product)nfΔG°(reactant)

Where,

• np is the number of moles of each product.
• nr is the number of moles each reactant.
• ΔG°(product) is the free energy of product at a pressure of 1atm .
• ΔG°(reactant) is the free energy of reactant at a pressure of 1atm .

Substitute all values from the table in the above equation

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