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Chapter 14: Problem 105

Write out the stepwise \(K_{\mathrm{a}}\) reactions for the diprotic acid \(\mathrm{H}_{2} \mathrm{SO}_{3}\)

Short Answer

Expert verified
The stepwise Ka reactions for the diprotic acid H2SO3 are: 1. First ionization reaction: \( H_{2}SO_{3} (aq) \rightleftharpoons H^+ (aq) + HSO_3^- (aq) \) with the Ka1 expression: \( K_{a1} = \frac{[H^+][HSO_3^-]}{[H_{2}SO_{3}]} \) 2. Second ionization reaction: \( HSO_3^- (aq) \rightleftharpoons H^+ (aq) + SO_3^{2-} (aq) \) with the Ka2 expression: \( K_{a2} = \frac{[H^+][SO_3^{2-}]}{[HSO_3^-]} \)

Step by step solution

01

Identify the diprotic acid and its ionization stages

H2SO3 is the given diprotic acid, meaning it can lose two protons (H+). There will be two ionization stages: 1. The first ionization stage will be when H2SO3 loses one proton and becomes HSO3- (the first conjugate base). 2. The second ionization stage will be when HSO3- loses another proton and becomes SO3^2- (the second conjugate base).
02

Write the first ionization reaction and Ka1 expression

The first ionization reaction is given by: \( H_{2}SO_{3} (aq) \rightleftharpoons H^+ (aq) + HSO_3^- (aq) \) The expression for the acid dissociation constant (Ka1) for the first ionization reaction is given by: \( K_{a1} = \frac{[H^+][HSO_3^-]}{[H_{2}SO_{3}]} \)
03

Write the second ionization reaction and Ka2 expression

The second ionization reaction is given by: \( HSO_3^- (aq) \rightleftharpoons H^+ (aq) + SO_3^{2-} (aq) \) The expression for the acid dissociation constant (Ka2) for the second ionization reaction is given by: \( K_{a2} = \frac{[H^+][SO_3^{2-}]}{[HSO_3^-]} \) In summary, the stepwise Ka reactions for the diprotic acid H2SO3 are: 1. First ionization reaction: \( H_{2}SO_{3} (aq) \rightleftharpoons H^+ (aq) + HSO_3^- (aq) \) with the Ka1 expression: \( K_{a1} = \frac{[H^+][HSO_3^-]}{[H_{2}SO_{3}]} \) 2. Second ionization reaction: \( HSO_3^- (aq) \rightleftharpoons H^+ (aq) + SO_3^{2-} (aq) \) with the Ka2 expression: \( K_{a2} = \frac{[H^+][SO_3^{2-}]}{[HSO_3^-]} \)

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Most popular questions from this chapter

A typical aspirin tablet contains 325 mg acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right) .\) Calculate the \(\mathrm{pH}\) of a solution that is prepared by dissolving two aspirin tablets in enough water to make one \(\operatorname{cup}(237 \mathrm{mL})\) of solution. Assume the aspirin tablets are pure acetylsalicylic acid, \(K_{\mathrm{a}}=3.3 \times 10^{-4}\) .

The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: $$ \mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) $$ Acids formed during normal cellular respiration react with the \(\mathrm{HCO}_{3}^{-}\) to form carbonic acid, which is in equilibrium with \(\mathrm{CO}_{2}(a q)\) and \(\mathrm{H}_{2} \mathrm{O}(l) .\) During vigorous exercise, a person's \(\mathrm{H}_{2} \mathrm{CO}_{3}\) blood levels were $26.3 \mathrm{mM},\( whereas his \)\mathrm{CO}_{2}\( levels were 1.63 \)\mathrm{mM}$ . On resting, the \(\mathrm{H}_{2} \mathrm{CO}_{3}\) levels declined to 24.9 \(\mathrm{m} M\) . What was the \(\mathrm{CO}_{2}\) blood level at rest?

A 0.25 -g sample of lime (CaO) is dissolved in enough water to make 1500 \(\mathrm{mL}\) of solution. Calculate the pH of the solution.

A \(1.0 \times 10^{-2}-M\) solution of cyanic acid (HOCN) is 17\(\%\) dissociated. Calculate \(K_{\mathrm{a}}\) for cyanic acid.

Consider 1000 . mL of a \(1.00 \times 10^{-4}-M\) solution of a certain acid HA that has a $K_{\text { a value equal to } 1.00 \times 10^{-4} . \text { How much }}$ water was added or removed (by evaporation) so that a solution remains in which 25.0\(\%\) of \(\mathrm{HA}\) is dissociated at equilibrium? Assume that HA is nonvolatile.
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