What is the pH of a 0.10 M succinic acid, H₂Sc, solution if we assume that H₂Sc is a weak acid that undergoes stepwise dissociation?
H₂Sc(aq) + H₂O(l) H₃O⁺(aq) + HSc^-(aq) K_a1 = 6.9 x 10^-5
HSc^-(aq) + H₂O(l) H₃O⁺(aq) + Sc^2-(aq) K_a2 = 2.5 x 10^-6

Question

What is the pH of a 0.10 M succinic acid, H₂Sc, solution if we assume that H₂Sc is a weak acid that undergoes stepwise dissociation?
H₂Sc(aq) + H₂O(l)

What is the pH of a 0.10 M succinic acid, H<sub>2</sub>Sc, solution if we assume that H<sub>2</sub>Sc is a weak acid that undergoes stepwise dissociation? H<sub>2</sub>Sc(aq) + H<sub>2</sub>O(l) H<sub>3</sub>O<sup>+</sup>(aq) + HSc<sup>-</sup>(aq) K<sub>a1</sub> = 6.9 x 10<sup>-5</sup> HSc<sup>-</sup>(aq) + H<sub>2</sub>O(l) H<sub>3</sub>O<sup>+</sup>(aq) + Sc<sup>2-</sup>(aq) K<sub>a2</sub> = 2.5 x 10<sup>-6</sup> A) 2.1 B) 2.6 C) 3.3 D) 4.2 E) 5.6

H₃O⁺(aq) + HSc^-(aq) K_a1 = 6.9 x 10^-5
HSc^-(aq) + H₂O(l)

H₃O⁺(aq) + Sc^2-(aq) K_a2 = 2.5 x 10^-6

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The Answer of What is the pH of a 0.10 M succinic acid, H₂Sc, solution if we assume that H₂Sc is a weak acid that undergoes stepwise dissociation? H₂Sc(aq) + H₂O(l) H₃O⁺(aq) + HSc^-(aq) K_a1 = 6.9 x 10^-5 HSc^-(aq) + H₂O(l) H₃O⁺(aq) + Sc^2-(aq) K_a2 = 2.5 x 10^-6

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