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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 solution of formic acid (HCOOH, \(K_{\mathrm{a}}=1.8 \times 10^{-4} )\) has a \(\mathrm{pH}\) of 2.70 . Calculate the initial concentration of formic acid in this solution.

Arrange the following 0.10\(M\) solutions in order from most acidic to most basic. See Appendix 5 for \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values. $$ \mathrm{CaBr}_{2}, \mathrm{KNO}_{2}, \mathrm{HClO}_{4}, \quad \mathrm{HNO}_{2}, \quad \mathrm{HONH}_{3} \mathrm{ClO}_{4} $$

a. The principal equilibrium in a solution of \(\mathrm{NaHCO}_{3}\) is $$ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between \(\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right]\) and \(\left[\mathrm{CO}_{3}^{2-}\right] ?\) c. Using the equilibrium $$ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons 2 \mathrm{H}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ derive an expression for the pH of the solution in terms of \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) using the result from part b. d. What is the pH of a solution of \(\mathrm{NaHCO}_{3} ?\)

When determining the pH of a weak acid solution, sometimes the 5\(\%\) rule can be applied to simplify the math. At what \(K_{\mathrm{a}}\) values will a \(1.0-M\) solution of a weak acid follow the 5\(\%\) rule?

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. \(\mathrm{Li}_{2} \mathrm{O}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{SrO}\)
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