What mass of KOH is necessary to prepare 800.0 mL of a solution having a pH = 11.56?

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Interpretation Introduction Interpretation: The mass of KOH that is necessary to prepare 800.0 mL of a solution that has a pH value of 11.56 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 pOH of a solution is calculated by the formula, pOH = − log [ OH − ] The sum, pH + pOH = 14 Explanation Explanation To determine: The mass of KOH that is necessary to prepare 800.0 mL of a solution that has a pH value of 11.56 . The pOH value is 2 . 4 4 _ . Given pH = 11.56 The sum, pH + pOH = 14 Substitute the given value of pH in the above expression. 11 .56 + pOH = 14 pOH = 2 . 4 4 _ The [ OH − ] is 0 . 0 0 3 6 M _ . The pOH of a solution is calculated by the formula, pOH = − log [ OH − ] Rearrange the above expression to calculate the value of [ OH − ] . [ OH − ] = 10 − pOH Substitute the given value of pOH in the above expression. [ OH − ] = 10 − 2.44 = 0 . 0 0 3 6 M _ The concentration of KOH is 0 . 0 0 3 6 M _ . KOH is a strong base. It dissociates completely into its ions. It is a monoacidic base. Therefore, the concentration of KOH is equal to the [ OH − ] , that is 0 . 0 0 3 6 M _ . The number of moles of KOH required is 2 . 9 2 8 × 1 0 - 3 m o l _

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The mass of KOH that is necessary to prepare 800.0 mL of a solution that has a pH value of 11.56 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 pOH of a solution is calculated by the formula, pOH=−log[OH−]

The sum, pH+pOH=14

Explanation of Solution

Explanation

To determine: The mass of KOH that is necessary to prepare 800.0 mL of a solution that has a pH value of 11.56 .

The pOH value is 2.44_ .

Given

pH=11.56

The sum, pH+pOH=14

Substitute the given value of pH in the above expression.

11.56+pOH=14pOH=2.44_

The [OH−] is 0.0036 M_ .

The pOH of a solution is calculated by the formula,

pOH=−log[OH−]

Rearrange the above expression to calculate the value of [OH−] .

[OH−]=10−pOH

Substitute the given value of pOH in the above expression.

[OH−]=10−2.44=0.0036 M_

The concentration of KOH is 0.0036 M_ .

KOH is a strong base. It dissociates completely into its ions. It is a monoacidic base.

Therefore, the concentration of KOH is equal to the [OH−] , that is 0.0036 M_ .

The number of moles of KOH required is 2.928×10-3 mol_

What mass of KOH is necessary to prepare 800.0 mL of a solution having a pH = 11.56?

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach