Calculate the concentration of all species present and the pH of a 0.020 -M HF solution.

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Interpretation Introduction Interpretation: The concentration of all the species present in a 0.020 M HF solution and its pH 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 all the species present in a 0.020 M HF solution and its pH . The dissociation of HF is, HF ( a q ) ⇌ H + ( a q ) + F − ( a q ) The stated reaction is, HF ( a q ) ⇌ H + ( a q ) + F − ( a q ) The major species that are present are H + and F − . The [ H + ] and [ F − ] is 3 . 6 × 1 0 - 3 M _ . The change in concentration of HF is assumed to be x . The ICE table for the stated reaction is, HF ( a q ) ⇌ H + ( a q ) + F − ( a q ) Inititial concentration 0.020 0 0 Change − x + x + x Equilibrium concentration 0.020 − x x x The equilibrium concentration of [ HF ] is ( 0.020 − x ) M . The equilibrium concentration of [ H + ] is x M . The equilibrium concentration of [ F − ] is x M . The K a for HF is 6.6 × 10 − 4 . At equilibrium, the equilibrium constant expression is expressed by the formula, K a = Concentration of products Concentration of reactants Where, K a is the acid dissociation constant. The equilibrium constant expression for the given reaction is, K a = [ H + ] [ F − ] [ HF ] Substitute the value of K a , [ HF ] , [ H + ] and [ F − ] in equation (1)

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Chemistry: An Atoms First Approach

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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 concentration of all the species present in a 0.020 M HF solution and its pH 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 of Solution

Explanation

To determine: The concentration of all the species present in a 0.020 M HF solution and its pH .

The dissociation of HF is, HF(aq) ⇌ H+(aq) + F−(aq)

The stated reaction is,

HF(aq) ⇌ H+(aq) + F−(aq)

The major species that are present are H+ and F− .

The [H+] and [F−] is 3.6×10-3 M_ .

The change in concentration of HF is assumed to be x .

The ICE table for the stated reaction is,

HF(aq)⇌H+(aq)+F−(aq)Inititial concentration0.02000Change−x+x+xEquilibrium concentration0.020−xxx

The equilibrium concentration of [HF] is (0.020−x) M .

The equilibrium concentration of [H+] is x M .

The equilibrium concentration of [F−] is x M .

The Ka for HF is 6.6×10−4 .

At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=Concentration of productsConcentration of reactants

Where,

Ka is the acid dissociation constant.

The equilibrium constant expression for the given reaction is,

Ka=[H+][F−][HF]

Substitute the value of Ka , [HF] , [H+] and [F−] in equation (1)

Calculate the concentration of all species present and the pH of a 0.020 -M HF solution.

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

Calculate the concentration of all species present and the pH of a 0.020-M HF solution.

Explanation of Solution

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