A1.00 L buffer solution is 0.250 M in HCN and 0.250 M in NACN and has a pH = 9.31. You add 0.100 moles of solid NaOH with no change in volume. Calculate the new pH (to 2 decimal places) of this buffer solution. (Hint: both HCN and CN- will change concentration)

A1.00 L buffer solution is 0.250 M in HCN and 0.250 M in NACN and has a pH = 9.31. You add 0.100 moles of solid NaOH with no change in volume. Calculate the new pH (to 2 decimal places) of this buffer solution. (Hint: both HCN and CN- will change concentration)

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 112CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...

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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.

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A 1.00 L buffer solution is 0.250 M in HCN and 0.250 M in NACN and has a pH = 9.31.
You add 0.100 moles of solid NaOH with no change in volume. Calculate the new pH (to 2 decimal
places) of this buffer solution. (Hint: both HCN and CN- will change concentration)

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