For a 0.315 M solution of H₂C6H606, calculate both the pH and the C6H₂06²- ion concentration.=7.9x10-5H₂C6H6O6 + H₂O — H3O+ + HC₂H0¯ Ka¹HCH6O6 + H2O=H3O+ + CoH6O2- Ka2 = 1.6×10-12pH=[C6H606²-] =M

Given,Molarity of HC6H6O6 = 0.315 M

For a 0.315 M solution of H₂CH², calculate both the pH and the C6H606²- ion concentration. = 7.9x10-5 1.6x10-12 H₂C6H₂O6 + H₂O ⇒ H3O+ + HCH₂0₁¯ ₂¹ HC₂H₂O6 + H₂O — H³O+ + C6H606²- ₂² = pH = [C6H606²-] = = M

For a 0.315 M solution of H₂CH², calculate both the pH and the C6H606²- ion concentration. = 7.9x10-5 1.6x10-12 H₂C6H₂O6 + H₂O ⇒ H3O+ + HCH₂0₁¯ ₂¹ HC₂H₂O6 + H₂O — H³O+ + C6H606²- ₂² = pH = [C6H606²-] = = M

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 10QAP: Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the...

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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

For a 0.315 M solution of H₂C6H606, calculate both the pH and the C6H₂06²- ion concentration.
=
7.9x10-5
H₂C6H6O6 + H₂O — H3O+ + HC₂H0¯ Ka¹
HCH6O6 + H2O=H3O+ + CoH6O2- Ka2 = 1.6×10-12
pH
=
[C6H606²-] =
M

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