Part A Calculate the pH of the solution made by adding 0.50 mol of HOBR and 0.30 mol of KOB to 1.00 L of water. The value of K for HOBR is 2.0 x 10-9. Express your answer numerically using two decimal places.
Part A Calculate the pH of the solution made by adding 0.50 mol of HOBR and 0.30 mol of KOB to 1.00 L of water. The value of K for HOBR is 2.0 x 10-9. Express your answer numerically using two decimal places.
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
Chapter1: Chemical Foundations
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![2 of 15
I Review | Constants | Periodic Table
Visualizing buffers
You can visualize a buffer solution containing approximately equal concentrations of HA and A in action using the following equation, where Ka
is the equilibrium constant:
[H3O ][A]
[HA]
K.
[H;O*]
[HA]
K.
[A]
When the concentrations of HA and A are relatively large, the addition of a small amount of acid or base changes their concentration negligibly.
The result is that the ratio (HA]/[A maintains a value approximately equal to 1, and the (H30+] is approximately equal to the Ka value under
buffer conditions.
Part A
Calculate the pH of the solution made by adding 0.50 mol of HOBR and 0.30 mol of KOBR to 1.00 L of water. The value of K, for HOBR is
2.0 x 10-9
Express your answer numerically using two decimal places.
• View Available Hint(s)
pH =
Submit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F01604a07-1abb-47f3-85be-4093016fdea3%2Fd2c5aab8-f22e-4f93-8f86-46e13ff9651a%2F8jt14h9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2 of 15
I Review | Constants | Periodic Table
Visualizing buffers
You can visualize a buffer solution containing approximately equal concentrations of HA and A in action using the following equation, where Ka
is the equilibrium constant:
[H3O ][A]
[HA]
K.
[H;O*]
[HA]
K.
[A]
When the concentrations of HA and A are relatively large, the addition of a small amount of acid or base changes their concentration negligibly.
The result is that the ratio (HA]/[A maintains a value approximately equal to 1, and the (H30+] is approximately equal to the Ka value under
buffer conditions.
Part A
Calculate the pH of the solution made by adding 0.50 mol of HOBR and 0.30 mol of KOBR to 1.00 L of water. The value of K, for HOBR is
2.0 x 10-9
Express your answer numerically using two decimal places.
• View Available Hint(s)
pH =
Submit
![Solutions that contain a weak acid, HA, and its conjugate
base, A
drastic changes in pH. 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. For buffers
containing a weak acid, the principal reaction is
are called buffer solutions because they resist
HA(aq) + H20(1)= H30*(aq) + A (aq)
Unbuffered, a weak acid would ionize and the net reaction
would proceed forward to reach equilibrium. However, when
a significant amount of conjugate base is already present,
the extent of the net reaction forward is diminished. Thus,
equilibrium concentrations of HA and A are
approximately equal to their initial concentrations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F01604a07-1abb-47f3-85be-4093016fdea3%2Fd2c5aab8-f22e-4f93-8f86-46e13ff9651a%2F0wy0e5r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Solutions that contain a weak acid, HA, and its conjugate
base, A
drastic changes in pH. 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. For buffers
containing a weak acid, the principal reaction is
are called buffer solutions because they resist
HA(aq) + H20(1)= H30*(aq) + A (aq)
Unbuffered, a weak acid would ionize and the net reaction
would proceed forward to reach equilibrium. However, when
a significant amount of conjugate base is already present,
the extent of the net reaction forward is diminished. Thus,
equilibrium concentrations of HA and A are
approximately equal to their initial concentrations.
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