Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l) H₃O⁺(aq) + HS^-(aq) K₁ = 1.0 × 10^-7
HS^-(aq) + H₂O(l) H₃O⁺(aq) + S^2-(aq) K₂ = ?
H₂S(g) + 2H₂O(l) 2H₃O⁺(aq) + S^2-(aq) K₃ = 1.3 × 10^-20
What is the value of K₂?

Question

Hydrogen sulfide will react with water as shown in the following reactions. H₂S(g) + H₂O(l)

Hydrogen sulfide will react with water as shown in the following reactions. H<sub>2</sub>S(g) + H<sub>2</sub>O(l) H<sub>3</sub>O<sup>+</sup>(aq) + HS<sup>-</sup>(aq) K<sub>1</sub> = 1.0 × 10<sup>-7</sup> HS<sup>-</sup>(aq) + H<sub>2</sub>O(l) H<sub>3</sub>O<sup>+</sup>(aq) + S<sup>2-</sup>(aq) K<sub>2</sub> = ? H<sub>2</sub>S(g) + 2H<sub>2</sub>O(l) 2H<sub>3</sub>O<sup>+</sup>(aq) + S<sup>2-</sup>(aq) K<sub>3</sub> = 1.3 × 10<sup>-20</sup> What is the value of K<sub>2</sub>? A) 1.3 × 10<sup>-27</sup> B) 2.3 × 10<sup>-7</sup> C) 1.3 × 10<sup>-13</sup> D) 7.7 × 10<sup>12</sup> E) 7.7 × 10<sup>26</sup>

H₃O⁺(aq) + HS^-(aq) K₁ = 1.0 × 10^-7
HS^-(aq) + H₂O(l)

H₃O⁺(aq) + S^2-(aq) K₂ = ?
H₂S(g) + 2H₂O(l)

2H₃O⁺(aq) + S^2-(aq) K₃ = 1.3 × 10^-20
What is the value of K₂?

Quizplus · Accepted Answer

For the first reaction: H₂S(g) + H₂O(l) 11eac68a_1c5c_9f1c_a448_7fa70eb3f124_TB7800_11 H₃O⁺(aq) + HS^-(aq) The equilibrium constant is given as K₁ = 1.0 × 10^-7 For the second reaction: HS^-(aq) + H₂O(l) 11eac68a_1c5c_c62d_a448_734cf559f267_TB7800_11 H₃O⁺(aq) + S^2-(aq) The equilibrium constant is not given but we can calculate it using the equation: K₃ = ((K₁)*(K₂))/((H₂O(l))^2) Substituting the given values, we get: K₃ = ((1.0 × 10^-7)*(2H₃O⁺(aq) + S^2-(aq)))/((H₂O(l))^2) Simplifying we get: K₃ = 1.3 × 10^-20 Therefore, the answer is option C: 1.3 × 10^-13

Hydrogen Sulfide Will React with Water as Shown in the Following