   Chapter 16, Problem 16.85QP 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 pH of a solution in which 15 mL of 0.10 M NaOH is added to 25 mL of 0.10 M HCl?

Interpretation Introduction

Interpretation:

The pH of the solution prepared by addition of 15 mL of 0.10 M NaOH with 25 mL of 0.10 M HCl has to be calculated

Concept Introduction:

pH definition:

The pH of a solution is defined as the negative base-10 logarithm of the hydronium ion [H3O+] concentration.

pH=-log[H3O+]

To Calculate: The pH of the solution prepared by addition of 15 mL of 0.10 M NaOH with 25 mL of 0.10 M HCl

Explanation

Given data:

The concentration of NaOH = 0.10 M

The concentration of HCl = 0.10 M

The volume of NaOH = 15 mL

The volume of HCl = 25 mL

pH calculation:

All of the hydroxide ion OH reacts with the hydronium ion H3O+ from HCl .

The moles are calculated as follows,

mol H3O+ =(0.10 mol HCl/L) × 0.025 L HCl =0.0025 mol H3O+mol OH =(0.10 mol NaOH/L) × 0.015 L NaOH =0.0015 mol OH

The moles of hydronium ion remaining can be obtained by subtracting the initial moles of hydronium ion by the moles of hydroxide ion reacted.

mol H3O+ left = intial mol of H3O+ mol of OH- =0

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