H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8 What is the equilibrium constant for the following reaction? HSO3(aq) + OH (aq) → SO3² (aq) + H₂O(l) A. 2.5 × 10² B. 6.4 x 106 C. 3.6 × 10³ D. 6.9 x 107 E. 5.5 × 108

H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8 What is the equilibrium constant for the following reaction? HSO3(aq) + OH (aq) → SO3² (aq) + H₂O(l) A. 2.5 × 10² B. 6.4 x 106 C. 3.6 × 10³ D. 6.9 x 107 E. 5.5 × 108

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 82AP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

The answer is B. Please explain. Thanks.

H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8
What is the equilibrium constant for the following reaction?
HSO3 (aq) + OH (aq) → SO3² (aq) + H₂O(0)
A. 2.5 × 10²
B. 6.4 x 106
C. 3.6 × 10³
D. 6.9 × 107
E. 5.5 ×
108

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