Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Page 272
Henderson-Hasselbalch Equations
Equilibrium equation for acidic buffer containing weak acid, HB(aq), and its conjugate
base, B (aq), and governed by acid ionization constant K, is written as:
+
HB(aq) + H,O() B (aq) + H,O*(aq),
K =
(1HB), - [*,0°])
If both initial concentrations, [HB], and [B-1,> K, and at the same time K, << 1, then the
pH of the buffer solution is calculated as:
pH,
%3D
"buffer pK, + log
[HB],
Equilibrium equation for basic buffer containing weak base, B(aq), and its conjugate
acid, BH" (aq), and governed by base ionization constant K, is written as:
([a* ]o • [Ox"])[on"]
(18), - [OH"])
B(aq) + H,O) 2 BH"(aq) + OH (aq),
%3D
If both initial concentrations, [B], and BH* Jo >> K,, and at the same time K, << 1, then the
pH of the buffer solution is calculated as:
BH 0
'buffer pKw- pK,- log
[B],
pH,
%3D](https://content.bartleby.com/qna-images/question/1c5462d2-50b2-4fa5-aeb8-e18d65e2fc1a/f7a19a4b-dce6-40a9-9e75-a0181c34e852/npu359p_processed.png)
Transcribed Image Text:Page 272
Henderson-Hasselbalch Equations
Equilibrium equation for acidic buffer containing weak acid, HB(aq), and its conjugate
base, B (aq), and governed by acid ionization constant K, is written as:
+
HB(aq) + H,O() B (aq) + H,O*(aq),
K =
(1HB), - [*,0°])
If both initial concentrations, [HB], and [B-1,> K, and at the same time K, << 1, then the
pH of the buffer solution is calculated as:
pH,
%3D
"buffer pK, + log
[HB],
Equilibrium equation for basic buffer containing weak base, B(aq), and its conjugate
acid, BH" (aq), and governed by base ionization constant K, is written as:
([a* ]o • [Ox"])[on"]
(18), - [OH"])
B(aq) + H,O) 2 BH"(aq) + OH (aq),
%3D
If both initial concentrations, [B], and BH* Jo >> K,, and at the same time K, << 1, then the
pH of the buffer solution is calculated as:
BH 0
'buffer pKw- pK,- log
[B],
pH,
%3D
Transcribed Image Text:A buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with
10 mL of 1.44 M NH Cl(aq). What is the pH of the buffer at 25°C, if the base ionization constant
of ammonia is 1.8x10° and the ion product of water is 1.0x10-14 at this temperature?. Enter
your answer in the box provided with correct units and sig. figs.:
Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the
next page.
Answer: pH,
'buffer
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