   # A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H + I and the pH of this solution. HBr and HI are both considered strong acids. ### 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 13, Problem 56E
Textbook Problem
191 views

## A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H+I and the pH of this solution. HBr and HI are both considered strong acids.

Interpretation Introduction

Interpretation: A solution prepared by mixing the given amount of HBr and HI is given. The [H+] and the pH of this solution is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The number of moles of a solute is calculated by the formula,

Molesofsolute=Volume(L)×Molarity

### Explanation of Solution

Explanation

To determine: The [H+] and the pH of the given solution.

The moles of HBr are 0.0025mol_ and that of HI are 0.015mol_ .

Given

Volume of HBr is 50.0mL(0.050L) .

Concentration of HBr is 0.050M .

Volume of HI is 150.0mL(0.150L) .

Concentration of HI is 0.10M .

The number of moles of a solute is calculated by the formula,

Molesofsolute=Volume(L)×Molarity

Substitute the value of volume and molarity of HBr and HI in the above expression.

For HBr ,

MolesofHBr=0.050L×0.050M=0.0025mol_

For HI ,

MolesofHI=0.150L×0.10M=0.015mol_

The [H+] is 0.0875M_ .

The total volume of the solution is calculated by the formula,

Totalvolume=VolumeofHBr+VolumeofHI

Substitute the value of the volume of HBr and the volume of HI in the above expression

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