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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 Ka for HOBr is 2.0 x 10-9 Express your answer numerically using two decimal places. • View Available Hint(s) pH =

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 Ka for HOBr is 2.0 x 10-9 Express your answer numerically using two decimal places. • View Available Hint(s) pH =

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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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Solutions that contain a weak acid, HA, and its conjugate base, A¯, are called buffer solutions because they resist 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 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 AT are approximately equal to their initial concentrations.
Transcribed Image Text:Solutions that contain a weak acid, HA, and its conjugate base, A¯, are called buffer solutions because they resist 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 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 AT are approximately equal to their initial concentrations.
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 HA K. H;O] = K. [A"] When the concentrations of HA and A concentration negligibly. The result is that the ratio (HA]/[A ] maintains a value approximately equal to 1, and the [H3O*] is approximately equal to the Ka value under buffer conditions. are relatively large, the addition of a small amount of acid or base changes their 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 Ka for HOBr is 2.0 x 10- Express your answer numerically using two decimal places. • View Available Hint(s) AZO ? pH = Submit Previous Answers
Transcribed Image Text: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 HA K. H;O] = K. [A"] When the concentrations of HA and A concentration negligibly. The result is that the ratio (HA]/[A ] maintains a value approximately equal to 1, and the [H3O*] is approximately equal to the Ka value under buffer conditions. are relatively large, the addition of a small amount of acid or base changes their 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 Ka for HOBr is 2.0 x 10- Express your answer numerically using two decimal places. • View Available Hint(s) AZO ? pH = Submit Previous Answers
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