   # Equal amounts (moles) of HCl(aq) and NaCN(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 1RC
Textbook Problem
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## Equal amounts (moles) of HCl(aq) and NaCN(aq) are mixed. The resulting solution is (a) acidic (b) basic (c) neutral

Interpretation Introduction

Interpretation:

The buffer nature (acidic or basic) should be identified 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 of HCl(aq) and NaCN(aq) are produced to NaCl and HCN , so this reaction has more acidic hence resulting solution behaved for acidic nature.

The weakest acid have the strongest conjugate basic nature, since (HCN) is the week acid, so it has the strongest conjugate base.

Let us consider the fallowing reaction

NaCN(aq)+HCl(aq)NaCl(aq)+HCN(aq)BaseAcidConjugateacidConjugatebase

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