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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

You travel to a distant, cold planet where the ammonia flows like water. In fact, the inhabitants of this planet use ammonia (an abundant liquid on their planet) much as earthlings use water. Ammonia is also similar to water in that it is amphoteric and undergoes autoionization. The K value for the autoionization of ammonia is 1.8 × 10−12 at the standard temperature of the planet. What is the pH of ammonia at this temperature?

Interpretation Introduction

Interpretation: The equilibrium constant for the ionization of ammonia is given. The pH value for this reaction is to be calculated.

Concept introduction: The expression of equilibrium constant K is,

K=ConcentrationofproductConcentrationofreactant

To determine: The pH value for the ionization of ammonia.

Explanation

The concentration of H+ is 1.342×106M_ .

Given

The equilibrium constant is 1.8×1012 .

The reaction of ionization of ammonia (NH3) is,

NH3NH2+H+

It is clear from the above equation that, the concentration of NH2 is equal to the concentration of H+ .

Formula

The expression of equilibrium constant for the given reaction is,

K=ConcentrationofproductConcentrationofreactant=[NH2][H+]

Where,

  • K is the equilibrium constant.

Since, the concentration of NH2 is equal to the concentration of H+ . Therefore, the above equation becomes,

K=[NH2][H+]=[H+]2

Substitute the value of K in the above expression

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