 # What is the pH of a solution that is 0.600 M HCHO 2 (formic acid) and 0.400 M NaCHO 2 ? ### General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343 ### General Chemistry - Standalone boo...

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

#### Solutions

Chapter
Section
Chapter 16, Problem 16.71QP
Textbook Problem

## What is the pH of a solution that is 0.600 M HCHO2 (formic acid) and 0.400 M NaCHO2?

Expert Solution
Interpretation Introduction

Interpretation:

The pH of a solution that is 0.600 M HCHO2 (formic acid) and 0.400 M NaCHO2 has to be calculated.

Concept Introduction:

The equilibrium expression for the weak acid 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 hydronium ion [H+] concentration.

pH=-log[H+]

To calculate: The pH of a solution that is 0.600 M HCHO2 (formic acid) and 0.400 M NaCHO2

### Explanation of Solution

Given data:

The concentration of HCHO2 is 0.600 M

The concentration of NaCHO2 is 0.400 M

Calculation of concentration:

Construct an equilibrium table, using a initial [HCHO2] as 0.600 M from HCHO2 and a initial concentration of [CHO2-] as 0.400 M from NaCHO2

Let x be the unknown concentration.

 HCHO2(aq)+H2O(l)     ⇌        H3O+(aq)  +   CHO2−(aq) Initial (M) 0.600 -x 0.600-x 0.00 0.400 Change (M) +x +x Equilibrium (M) x 0.400+x

The Ka of HCHO2 is 1.7×104

Substitute the equilibrium concentrations into equilibrium-constant expression

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