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Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq),  H2S(aq)⇌HS−(aq)+H+(aq),   K1K1K_1 = 9.78×10−8, and HS−(aq)⇌S2−(aq)+H+(aq),  HS−(aq)⇌S2−(aq)+H+(aq),   K2K2K_2 = 1.43×10−19, what is the equilibrium constant KfinalKfinalK_final for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.

Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq),  H2S(aq)⇌HS−(aq)+H+(aq),   K1K1K_1 = 9.78×10−8, and HS−(aq)⇌S2−(aq)+H+(aq),  HS−(aq)⇌S2−(aq)+H+(aq),   K2K2K_2 = 1.43×10−19, what is the equilibrium constant KfinalKfinalK_final for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Given the two reactions
  1. H2S(aq)⇌HS−(aq)+H+(aq),  H2S(aq)⇌HS−(aq)+H+(aq),   K1K1K_1 = 9.78×10−8, and
  2. HS−(aq)⇌S2−(aq)+H+(aq),  HS−(aq)⇌S2−(aq)+H+(aq),   K2K2K_2 = 1.43×10−19,
what is the equilibrium constant KfinalKfinalK_final for the following reaction?

S2−(aq)+2H+(aq)⇌H2S(aq)S2−(aq)+2H+(aq)⇌H2S(aq)

Enter your answer numerically.
Expert Solution
Step 1

The two given reactions are - 

  1. H2S(aq)  ⇌  HS-(aq)  +  H+(aq)                                        K1 = 9.78×10−8
  2. HS-(aq)   ⇌  S2-(aq) +H+(aq)                                            K2 = 1.43×10−19

The  equilibrium constant expression for the given reactions are -

K1 = [HS-][H+][H2S]9.78 × 10-8 = [HS-][H+][H2S]

K2 = [S2-][H+][HS-]1.43 × 10-19 =  [S2-][H+][HS-]

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