   # What are the pH and ion concentrations in a solution of 0.10 M sodium formate, NaCHO 2 ? K b for the formate ion, HCO 2 − is 5.6 × 10 −11 . pH [Na + ] [CHO 2 − ] [OH − ] (a) 5.63 0.10 0.10 2.4 × 10 -6 (b) 837 0.10 0.10 2.4 × 10 6 (c) 822 0.050 0.050 17 × 10-‘ (d) 5.63 0.10 0.10 42 × 10 * ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 16.7, Problem 3RC
Textbook Problem
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## What are the pH and ion concentrations in a solution of 0.10 M sodium formate, NaCHO2? Kb for the formate ion, HCO2− is 5.6 × 10−11. pH [Na+] [CHO2−] [OH−] (a) 5.63 0.10 0.10 2.4 × 10-6 (b) 837 0.10 0.10 2.4 × 10 6 (c) 822 0.050 0.050 17 × 10-‘ (d) 5.63 0.10 0.10 42 × 10 *

Interpretation Introduction

Interpretation:

The sodium formate ( Kb ) value has given in the statement, and correct molar concentration (pH) ranges should be calculate and identified.

Concept introduction:

pH concept of hydronium ions: A strong acid completely dissociates into its constituent ions in aqueous solution, as a result, the concentration of its ion is same as the initial concentration of that strong acid.

For example, strong acid dissociates as follows in water,

HA(aq)+H2O(l)H3O+(aq)+A(aq)

[H3O+]=[A]=[HA]

The pH of a solution is basically the measure of the molar concentration of the H+ or H3O+ ion in the solution. More the concentration of H+ or H3O+ ion in the solution, lesser will be the pH value and more acidic will be the solution.

The expression for pH is given as,

pH=log[H3O+]

The concentration of OH ions is calculated by using the ionic product of water.

Kw=[H3O+][OH]

The value of Kw is 1.0×1014 .

If pH<7 then, the solution is acidic in nature.

If pH<7 then, the solution is basic in nature.

If pH<7 then, the solution is neutral in nature.

### Explanation of Solution

The value of pH for formate ion (NaCHO2) solution and the concentration of the solution is calculated below.

Given

The initial concentration of CHO2- solution is 0.10 M .

CHO2- is a week base and it dissociates as follows in water,

CHO2-(aq)+H2O(l)HCHO2(aq)+OH-(aq)

The ICE table is as follows,

CHO2-(aq)+H2O(aq)HCHO2(aq)+OH-(aq)Initial(M)0.100Change(M)-x+x+xEquilibrium(M)(0.1-x)xx

Theequilibriumexpressionshownbelow:Kb=[HCHO2][OH-][CHO2-]GivenKbvalueofCHO2-=5.6×1011Thisvaluehassubstitutedaboveequation5

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