   # Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH) 2 solution. What is the concentration of the excess H + or OH − ions left in this solution? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 73E
Textbook Problem
739 views

## Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of the excess H+ or OH− ions left in this solution?

Interpretation Introduction

Interpretation:

To find concentration of the excess H+ or OH- ions left in the hydrochloric acid 75.0ml  of 0.250M  is added to 225ml of 0.0550M Ba(OH)2 solution.

Concept introduction:

It's a clear neutralization reaction. Since the volume and the molarity is specified we can easily calculate the excess quantity of ions left, we can calculate the moles in solution type the formula is,

moles =molarity of the solution×volume of the solution

### Explanation of Solution

To find: The moles of HCl solution

Given,

75mlof 0.250MHClsolution

HCl Produces H+

moles =molarity of the solution×volume of the solution

0.25×75=18.75moles

Concentration of the solution is multiple with volume of solution to give a mole of H+ ion produced by acid.

To find: The moles of Ba(OH)2 solution

Given,

225mlof 0.0550MBa(OH)2solution

Ba(OH)2 Produces 2OH-

moles =molarity of the solution×volume of the solution

225×0.0550×2=24.75moles .

Concentration of the solution is multiple with volume of solution to give a mole of OH- ion produced by Ba(OH)2 .

To find: The new excess concentration of OH- ions

Find out difference of the H+ ions and OH-

=24

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