   Chapter 16.7, Problem 16.14E 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 has been 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 and 25 mL of 0.10 M HCl has to be calculated.

Concept Information:

pH definition:

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

pH=-log[H+]

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

Explanation

Given data:

The amount of sodium hydroxide = 15 mL

The amount of hydrogen chloride = 25 mL

The concentration of sodium hydroxide = 0.10 M

The concentration of hydrogen chloride = 0.10 M

All the hydroxide ions reacts with the hydronium ion from HCl

Let us first do the stoichiometric calculation:

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

The total volume of the solution is calculated as,

Total volume = 0.025 L + 0.015 L =0

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