Explanation Given The acid-dissociation constant ( K a ) for chlorous acid is 1.1 × 10 − 2 . The initial concentration of chlorous acid ( HClO 2 ) is 0.0125 M . The ionization reaction of chlorous acid in aqueous solution is, HClO 2 ( a q ) + H 2 O ( l ) → ClO 2 − ( a q ) + H 3 O + ( a q ) The initial concentration of chlorous acid is 0.0125 M and the change in concentration is taken as x M . The ICE table for the dissociation reaction of chlorous acid is, HClO 2 ( a q ) ⇌ H 3 O + ( a q ) + ClO 2 − ( a q ) Initial concentration (M): 0.0125 0 0 Change in concentration (M): − x + x + x Equilibrium concentration (M): ( 0.0125 − x ) x x Table 1 The change in concentration ( x ) is calculated by the formula, K a = [ H 3 O + ] [ ClO 2 − ] [ HClO 2 ] H 2 O is acting as a solvent in this reaction, so it is omitted from the expression of acid-dissociation constant of chlorous acid. Where, [ H 3 O + ] is the equilibrium concentration of H 3 O + ions. [ ClO 2 − ] is the equilibrium concentration of ClO 2 − ions. [ HClO 2 ] is the equilibrium concentration of chlorous acid. K a is ionization constant of chlorous acid. Substitute the values of [ H 3 O + ] , [ ClO 2 − ] , [ HClO 2 ] and K a in the above formula

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Chapter 2, Problem 48E

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To determine: The equilibrium concentration of H3O+ , ClO2− and HClO2 if the initial concentration of HClO2 is 0.0125 M .

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Chapter 2, Problem 47E

Chapter 2, Problem 49E

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Chemistry: The Central Science, Books a la Carte Edition & Solutions to Red Exercises for Chemistry & Mastering Chemistry with Pearson eText -- Access Card Package

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The equilibrium concentration of H 3 O + , ClO 2 − and HClO 2 if the initial concentration of HClO 2 is 0.0125 M .

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To determine: The equilibrium concentration of H3O+ , ClO2− and HClO2 if the initial concentration of HClO2 is 0.0125 M .

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