   Chapter 16.5, Problem 16.10E 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 concentration of formate ion, CHO2−, in a solution at 25°C that is 0.10 M HCHO2 and 0.20 M HCl? What is the degree of ionization of formic acid, HCHO2?

Interpretation Introduction

Interpretation:

The concentration of formate ion and degree of ionization of formic acid in a solution of 0.10 M HCHO2 and 0.20 M HCl has to be calculated

Concept Information:

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

Degree of ionization (α)  is the amount of reactant that undergone ionization in the reaction.

To Calculate: The concentration of formate ion and the degree of ionization of formic acid for the reaction of 0.1 M HCHO2 and 0.20 M HCl

Explanation

Given data:

The concentration of formic acid (HCOOH) = 0.10 M

The concentration of hydrochloric acid (HCl)  = 0.20 M

Explanation:

Identify the reaction for acid and find out whether any ions in solution from added acid (Hydrochloric acid) that will disturb the chemical reaction

HCOOH + H2O HCOO- + H+

Hydrogen chloride gives H+ and Cl- ions

Assemble the usual table using a starting hydrogen ion of 0.20 M from HCl

Construct the equilibrium table, by considering the concentration of hydrogen ion from HCl

 HCOOH   +   H2O  ⇌   HCOO-   +   H+ Initial (M) 0.10 −x 0.10-x 0.00 0.20 Change (M) +x +x Equilibrium (M) x 0.20+x

The Ka for formic acid is 1.7×104

Substitute into the equilibrium-constant equation

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