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ChemistryChemistry: An Atoms First Approach2nd Edition
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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.

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Chemistry: An Atoms First Approach

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

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 56E
Textbook Problem
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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,

Moles of solute=Volume(L)×Molarity

Explanation of Solution

Explanation

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

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

Given

Volume of HBr is 50.0 mL (0.050 L) .

Concentration of HBr is 0.050 M .

Volume of HI is 150.0 mL (0.150 L) .

Concentration of HI is 0.10 M .

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

Moles of solute=Volume(L)×Molarity

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

For HBr ,

Moles of HBr=0.050 L×0.050 M=0.0025 mol_

For HI ,

Moles of HI=0.150 L×0.10 M=0.015 mol_

The [H+] is 0.0875 M_ .

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

Total volume=Volume of HBr+Volume of HI

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

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