   # Equal amounts (moles) of acetic acid(aq) and sodium sulfite, Na 2 SO 3 (aq), are mixed. The resulting solution is (a) acidic (b) basic (c) neutral ### 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 16.6, Problem 2RC
Textbook Problem
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## Equal amounts (moles) of acetic acid(aq) and sodium sulfite, Na2SO3(aq), are mixed. The resulting solution is (a) acidic (b) basic (c) neutral

Interpretation Introduction

Interpretation:

The acid, basic and neutral nature should be determined given the statement of resulting solution.

Concept introduction:

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

Given the statement equal amount (moles) of acetic acid and sodium sulfide are produced to sodium acetate, water and sulfur dioxide gas, the corresponding reaction given below.

Na2SO3(aq)+2CH3COOH(aq)2CH3COONa+(aq)+H2O(aq)+SO2(g)BaseAcidConjugatebaseConjugateacid

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