   Chapter 16, Problem 89AE

Chapter
Section
Textbook Problem

# a. Using the Ksp value for Cu(OH)2 (1.6 × 10−19) and the overall formation constant for Cu(NH3)42+ (1.0 × 1013), calculate the value for the equilibrium constant for the following reaction: Cu(OH) 2 ( s )   +   4NH 3 ( a q )   ⇌   C u ( N H 3 ) 4 2 + ( a q )   +   2 O H − ( a q ) b. Use the value of the equilibrium constant you calculated in part a to calculate the solubility (in mol/L) of Cu(OH)2 in 5.0 M NH3. In 5.0 M NH3 the concentration of OH− is 0.0095 M.

(a)

Interpretation Introduction

Interpretation: The Ksp value for Cu(OH)2 and the overall formation constant for Cu(NH3)42+ is given. The questions based on the stated data are to be answered.

Concept introduction: The equilibrium constant for a given reaction is calculated by the formula, Equilibriumconstant=KspKf

At equilibrium, the equilibrium constant expression is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Explanation

To determine: The value for the equilibrium constant for the given reaction.

The value for the equilibrium constant for the given reaction is 1.6×10-6_ .

Given

The value of Kf is 1.0×1013 .

The value of Ksp is 1.6×1019 .

The given reaction is,

Cu(OH)2(s)+4NH3(aq)Cu(NH3)42+(aq)+2O

(b)

Interpretation Introduction

Interpretation: The Ksp value for Cu(OH)2 and the overall formation constant for Cu(NH3)42+ is given. The questions based on the stated data are to be answered.

Concept introduction: The equilibrium constant for a given reaction is calculated by the formula, Equilibriumconstant=KspKf

At equilibrium, the equilibrium constant expression is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

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