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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
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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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
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.
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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