For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer? Accerding to Hendeeson Hasselbalch equation 7pH= pka+ log (conjugate Ber)Step 2ro ef mdes of conjugate20 X 3= 60 mmolesno.base%3D·e moles of acid50 X 2100 mmolesno:%3DKa = 4.30 X 1o-7%3DKa(4:30 X10*6.3665pha=PH = 6.3665 tlog Go100= 6.335 -0.2218pH = 6:1447or

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Answered: For the buffer system in Problem no. 1,…

For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.9QAP

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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 the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?

Accerding to Hendeeson Hasselbalch equation 7
pH= pka+ log (conjugate Ber)
Step 2
ro ef mdes of conjugate
20 X 3
= 60 mmoles
no.
base
%3D
·e moles of acid
50 X 2
100 mmoles
no:
%3D
Ka = 4.30 X 1o-7
%3D
Ka
(4:30 X10*
6.3665
pha=
PH = 6.3665 t
log Go
100
= 6.335 -0.2218
pH = 6:1447
or

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