Answered: How does the Henderson Hadeelbalch…

How does the Henderson Hadeelbalch equation prove that the pka of a weak acid is equal to the pH of the solution at the midpoint of it's titration?

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 50SSC

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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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Show that the pH at the halfway point is equivalent to titration of a weak acid with a strong base equal to pKa. 0.01M
Use the titration curve to calculate the pKa of HA at the equivalence point. What value did you obtain for pKa?
Using the Henderson-Hasselbalch equation, demonstrate that the pH at 50% neutralisation for a monoprotic acid/base titration is equal to the pKa for the acid.
The pH at the half-equivalence point of a weak acid-strong base titration is 5.23. What is the pKa value for this acid?
What is the effective pH range of a buffer (relative to the pKa of the weak acid component)?
Which one of the following is equal to the pKa of a weak acid? A. The pH of a solution containing equal amounts of the acid and its conjugate base B. The equilibrium concentration of its conjugate base C. The pKb of its conjugate base D. Its relative molar mass E. The equivalence point in a titration with a stong base
Mathematically prove that the pH at the halfway point of a titration of a weak acid with a strong base (where the volume of added base is half of that needed to reach the equivalence point) is equal to pKa for the acid.
How the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acid
At half-titration point of a weak acid with a strong base, the pH is equivalent to ½ of its pKa. True or False?
Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak acid.Round the pKa to the nearest whole number for the calculation, and enter your answer for the pH to two significant figures.
Derive an equation similar to the Henderson–Hasselbalch equation for a buffer composed of a weak base and its conjugate acid. Instead of relating pH to pKa and the relative concentrations of an acid and its conjugate base (as the Henderson–Hasselbalch equation does), the equation should relate pOH to pKb and the relative concentrations of a base and its conjugate acid.
If the concentration of the weak base ammonia is 0.10 M and it is titrated with 0.1 M HCl, and the Kb of ammonia is 1.8 x 10^-5, calculate the pre-titration pH