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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

Calculate the concentration of an aqueous HBr solution that has pH = 4.25. HBr is a strong acid.

Interpretation Introduction

Interpretation: The concentration of the given aqueous solution of HBr that has a pH value of 4.25 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. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

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

Explanation

Explanation

To determine: The concentration of the given aqueous solution of HBr that has a pH value of 4.25 .

The [H+] is calculated by the formula, [H+]=10pH

The pH of a solution is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH (1)

The concentration of the given aqueous solution of HBr is 5.6×10-5M_

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