Chapter 16, Problem 93GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# m-Nitrophenol, a weak acid, can be used as a pH indicator because it is yellow at pH above 8.6 and colorless at pH below 6.8. If the pH of a 0.010M solution of the compound is 3.44, calculates its pKa.

Interpretation Introduction

Interpretation:

The pKa value 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 an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Explanation

pKa of m-Nitrophenol solution is 4.87.

Letâ€™s calculate the hydronium ion concentration.

pHÂ =Â -logÂ [H3O+]theÂ givenÂ pHÂ =Â 3.44[H3O+]Â Â =Â 10-3.44[H3O+]Â Â =Â Â 3.6Ã—10-4M

The equilibrium chemical reaction is as follows.

C6H4NO2OHÂ (aq)Â +Â H2O(l)Â â‡ŒC6H4NO2O-Â (aq)Â +Â H3O+(aq)

The equilibrium expression:

Ka=Â [C6H4NO2O-][H3O+][C6H4NO2OH]

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.

The given concentration =0.010 M

Â Â Â Â Â Â Â Â Â Â C6H4NO2OHÂ (aq)Â +Â H2O(l)Â â‡ŒC6H4NO2O-Â (aq)Â +Â H3O+(aq)IÂ Â Â Â Â Â Â Â Â 0

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