   Chapter 16.1, Problem 16.3E General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

What is the pH of an aqueous solution that is 0.0030 M pyruvic acid, HC3H3O3? (Pyruvic acid forms during the breakdown of glucose in a cell.)

Interpretation Introduction

Interpretation:

The pH of an aqueous solution of pyruvic acid has to be calculated

Concept Information:

Acid ionization constant Ka :

The ionization of a weak acid HA can be given as follows,

HA(aq)H+(aq)+A-(aq)

The equilibrium expression for the above reaction is given below.

Ka=[H+][A-][HA]

Where,

Ka is acid ionization constant,

[H+]   is concentration of hydrogen ion

[A-]   is concentration of acid anion

[HA] is concentration of the acid

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H+]

On rearranging, we get

[H+]= 10-pH

To Calculate: The pH of an aqueous solution of pyruvic acid

Explanation

Given data:

The concentration of pyruvic acid solution = 0.0030 M

The Ka value of pyruvic acid is 1.4×10-4

Concentration of hydrogen ion:

Set up the equilibrium table for the hydrolysis of acetic acid reaction.

Let x be the unknown concentration

 HC3H3O3(aq)+H2O(l)     ⇄        C3H3O3-(aq)   +     H3O+(aq) Initial (M) 0.0030 -x 0.0030-x 0.00 0.00 Change (M) +x +x Equilibrium (M) x x

The Ka value of pyruvic acid is 1

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