Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. • View Available Hint(s) ? pH = Submit Previous Answers Incorrect; Try Again; 3 attempts remaining Part C What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal places.
Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. • View Available Hint(s) ? pH = Submit Previous Answers Incorrect; Try Again; 3 attempts remaining Part C What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal places.
General Chemistry - Standalone book (MindTap Course List)
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.149QP: A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the...
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I need help with part b and c for 5
![I Review | Constants Periodic Table
d and its
Part B
its conjugate
ers resist
of acid or base.
eak acid (HA)
resented as
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the
acid.
Express the pH numerically to three decimal places.
A (aq)
• View Available Hint(s)
s principle. If acid
sume the added
se is added, the
its concentration.
e H* through the
A. In both
pH =
constant.
Previous Answers
by using the
on:
Submit
[A]
og HA
X Incorrect; Try Again; 3 attempts remaining
Part C
What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of
the base.
Express the pH numerically to three decimal places.
• View Available Hint(s)
Πν ΑΣΦ
4:51 PM
pH =
3/21/2021](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F01604a07-1abb-47f3-85be-4093016fdea3%2Fb3197986-537a-4682-9206-9f9fe2697d40%2Fnsvuvci_processed.jpeg&w=3840&q=75)
Transcribed Image Text:I Review | Constants Periodic Table
d and its
Part B
its conjugate
ers resist
of acid or base.
eak acid (HA)
resented as
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the
acid.
Express the pH numerically to three decimal places.
A (aq)
• View Available Hint(s)
s principle. If acid
sume the added
se is added, the
its concentration.
e H* through the
A. In both
pH =
constant.
Previous Answers
by using the
on:
Submit
[A]
og HA
X Incorrect; Try Again; 3 attempts remaining
Part C
What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of
the base.
Express the pH numerically to three decimal places.
• View Available Hint(s)
Πν ΑΣΦ
4:51 PM
pH =
3/21/2021
![When a solution contains a weak acid and its
conjugate base or a weak base and its conjugate
acid, it will be a buffer solution. Buffers resist
change in pH following the addition of acid or base.
A buffer solution prepared from a weak acid (HA)
and its conjugate base (A ) is represented as
Part A
What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution?
The dissociation.constant K, of HA is 5.66 x 10
-7
HA(aq) =H'(aq) + A (aq)
Express the pH numerically to three decimal places.
The buffer will follow Le Châtelier's principle. If acid
is added, the reaction shifts to consume the added
H, forming more HA. When base is added, the
base will react with H, reducing its concentration.
The reaction then shifts to replace H* through the
dissociation of HA into Ht and A . In both
instances, (H+] tends to remain constant.
» View Available Hint(s)
pH = 5.823
Previous Answers
The pH of a buffer is calculated by using the
Henderson-Hasselbalch equation:
v Correct
[A"]
pH = pKa+log HAJ
Correct answer is shown. Your answer 5.83 was either rounded differently or used a different number of significant
figures than required for this part.
Important: If you use this answer in later parts, use the full unrounded value in your calculations.
Since both the acid and base exist in the same volume, we can skip the concentration calculations and use the
number of moles in the Henderson-Hasselbalch equation to calculate the pH. The answer will be the same.
Part B
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the
acid.
Express the pH numerically to three decimal places.
> View Available Hint(s)
4:50 PM
3/21/2021
pe here to search
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Transcribed Image Text:When a solution contains a weak acid and its
conjugate base or a weak base and its conjugate
acid, it will be a buffer solution. Buffers resist
change in pH following the addition of acid or base.
A buffer solution prepared from a weak acid (HA)
and its conjugate base (A ) is represented as
Part A
What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution?
The dissociation.constant K, of HA is 5.66 x 10
-7
HA(aq) =H'(aq) + A (aq)
Express the pH numerically to three decimal places.
The buffer will follow Le Châtelier's principle. If acid
is added, the reaction shifts to consume the added
H, forming more HA. When base is added, the
base will react with H, reducing its concentration.
The reaction then shifts to replace H* through the
dissociation of HA into Ht and A . In both
instances, (H+] tends to remain constant.
» View Available Hint(s)
pH = 5.823
Previous Answers
The pH of a buffer is calculated by using the
Henderson-Hasselbalch equation:
v Correct
[A"]
pH = pKa+log HAJ
Correct answer is shown. Your answer 5.83 was either rounded differently or used a different number of significant
figures than required for this part.
Important: If you use this answer in later parts, use the full unrounded value in your calculations.
Since both the acid and base exist in the same volume, we can skip the concentration calculations and use the
number of moles in the Henderson-Hasselbalch equation to calculate the pH. The answer will be the same.
Part B
What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the
acid.
Express the pH numerically to three decimal places.
> View Available Hint(s)
4:50 PM
3/21/2021
pe here to search
Del
End
F10
PgUp
Ins
Home
F9
F12
PrtScn
F8
F1
DII
F5
F6
F7
F2
F3
F4
FI
1.
@
%23
24
&
Backs
7
8
2
4
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