Explanation Given: Dissociation constant of weak acids ( K a ) is equal to 1.0 × 10 − 8 and rate constant ( K ) is 4 . Explanation: The reaction of weak acid is as follows: HA ( a q ) +A − ( a q ) → HA 2 − ( a q ) The rate constant ( K ) for this reaction can be expressed as follows: K = [ HA 2 − ] [ HA ] [ A − 1 ] The ionization reaction of HA is as follows: HA ( a q ) +H 2 O ( l ) → A − ( a q ) + H 3 O + ( a q ) The acid dissociation constant ( K a ) for this reaction is as follows: K a = [ A − 1 ] [ H + ] [ HA ] The dissociated moles can be calculated as follows: The initial concentration of HA is 1 .0 M HA ( a q ) +H 2 O ( l ) → A − ( a q ) + H 3 O + ( a q ) Initial 1 0 0 Equilibrium 1 - x + x + x [ HA ] + [ A − ] + [ HA 2 − ] = 1 …… (1) The hydrogen ion concentration can be written as follows: [ H + ] = [ A − ] + [ HA 2 − ] [ HA 2 − ] = [ H + ] − [ A − ] …… (2) Substitute [ HA 2 − ] from equation (2) in rate constant expression as follows: K = [ H + ] − [ A − ] [ HA ] [ A − 1 ] = [ H + ] [ HA ] [ A − 1 ] − 1 [ HA ] or K = [ H + ] [ HA ] [ A − 1 ] − 1 [ HA ] …… (3) The expression for acid dissociation constant can be expressed as follows: K a [ A − 1 ] = [ H + ] [ HA ] Substitute [ H + ] [ HA ] as K a [ A − 1 ] in equation (3) as follows: K = K a [ A − 1 ] 1 [ A − 1 ] − 1 [ HA ] = K a [ A − 1 ] 2 − 1 [ HA ] or 1 [ HA ] = K a [ A − 1 ] 2 − K or [ HA ] = 1 K a [ A − 1 ] 2 − K …… (4) The concentration of HA 2 − can be written as follows: [ HA 2 − ] = K [ HA ] [ A − 1 ] Substitute [ HA ] from equation (4) in above expression as follows: [ HA 2 − ] = K ( 1 K a [ A − 1 ] 2 − K ) [ A − 1 ] …… (5) Substitute the value of [

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Chapter 16, Problem 151E

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To determine: [H+], [ A− ], and [HA2−] in 1.0 M solution of HA.

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Chapter 16, Problem 150E

Chapter 16, Problem 152E

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Ch. 16 - Prob. 1SAQ Ch. 16 - Q2. Which pair is a Brønsted–Lowry conjugate...Ch. 16 - Prob. 3SAQ Ch. 16 - Prob. 4SAQ Ch. 16 - Q5. An HNO3(aq) solution has a pH of 1.75. What is...Ch. 16 - Q6. Find the pH of a 0.350 M aqueous benzoic acid...Ch. 16 - Q7. Find the pH of a 0.155 M HClO2(aq) solution....Ch. 16 - Prob. 8SAQ Ch. 16 - Prob. 9SAQ Ch. 16 - Prob. 10SAQ

Ch. 16 - Prob. 11SAQ Ch. 16 - Prob. 12SAQ Ch. 16 - Prob. 13SAQ Ch. 16 - Prob. 14SAQ Ch. 16 - Q15. Which acid has the largest Ka: HClO2(aq),...Ch. 16 - 1. What causes heartburn? What are some possible...Ch. 16 - 2. What are the general physical and chemical...Ch. 16 - Prob. 3E Ch. 16 - Prob. 4E Ch. 16 - Prob. 5E Ch. 16 - Prob. 6E Ch. 16 - Prob. 7E Ch. 16 - Prob. 8E Ch. 16 - Prob. 9E Ch. 16 - Prob. 10E Ch. 16 - 11. What are diprotic and triprotic acids? List an...Ch. 16 - 12. Define the acid ionization constant and...Ch. 16 - 13. Write an equation for the autoionization of...Ch. 16 - 14. What happens to the [OH–] of a solution when...Ch. 16 - Prob. 15E Ch. 16 - Prob. 16E Ch. 16 - Prob. 17E Ch. 16 - Prob. 18E Ch. 16 - Prob. 19E Ch. 16 - Prob. 20E Ch. 16 - Prob. 21E Ch. 16 - 22. How can you determine if an anion will act as...Ch. 16 - 23. What is the relationship between the acid...Ch. 16 - 24. What kinds of cations act as weak acids? List...Ch. 16 - 25. 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[ H + ] , [ A − ] , and [ HA 2 − ] in 1 .0 M solution of HA .

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To determine: [H+], [ A− ], and [HA2−] in 1.0 M solution of HA.

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Chapter 16 Solutions