   Chapter 16, Problem 53PS

Chapter
Section
Textbook Problem

What are the equilibrium concentration of H 3 O + , CN‒ and HCN in a 0.025 M solution of HCN? What is the pH of the solution?

Interpretation Introduction

Interpretation:

The equilibrium concentration of H3O+,CN- and HCN in a 0.025 M solution of HCN and also pH of the solution has to be calculated.

Concept introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Explanation

The equation for the reaction of a HCN with water and its equilibrium constant expression are

HCN(aq) + H2O(l) CN-(aq) + H3O+(aq)Ka(HCN)= [CN-][H3O+][HCN]

Enter the ICE table the concentrations before equilibrium is established, the change that occurs as the reaction proceeds to equilibrium and the concentrations when equilibrium has been achieved.

HCN(aq)     +  H2O(l) CN- + H3O+I       0.025                --                --          --C          -x                  --              + x       + xE    (0.025 - x)           --                x           x

The Ka of the Hydrogen cyanide is 4.0×10-10

Ka(HCN) = [CN-][H3O+][HCN] = 4.0×10-10

4

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