   # A 25-mL sample of 0.40 M HCI is added to 32 mL of 030 M NaOH. Is the resulting solution acidic basic, or neutral? (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 4.7, Problem 1RC
Textbook Problem
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## A 25-mL sample of 0.40 M HCI is added to 32 mL of 030 M NaOH. Is the resulting solution acidic basic, or neutral? (a) acidic (b) basic (c) neutral

Interpretation Introduction

Interpretation:

It should be determine that the final solution prepared after mixing a 25mL of 0.40MHCl and 32mL of 0.30MNaOH is acidic, basic or neutral

Concept introduction:

• pH of a solution is the negative of the base -10 logarithm of the hydronium ion concentration.

pH=-log[H3O+]

• For an acidic solution pH<7 and for a basic solution pH>7
• Concentration=AmountofthesubstanceVolume
• Amountofthesubstance=Concentration×Volume

### Explanation of Solution

Given,

25mL of 0.40MHCl and 32mL of 0.30MNaOH , the amount of these  substances can be calculated as follows,

AmountofHCl=0.40molL×0.025L=0.01molAmountofNaOH=0.30molL×0.032L=0.0096mol

To neutralize the reaction equal amount of reactant is required. But here 0.0004mol of HCl is excess after mixing 25mL of 0.40MHCl and 32mL of 0.30MNaOH

Then the concentration of the solution can be determined as follows,

Concentration=0

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