A solution of a weak acid (H A ) and its conjugate base (A - ), HA (aq) H + (aq)

Question

A solution of a weak acid (H A ) and its conjugate base (A - ), HA (aq) H + (aq) + A- (aq) is called a buffer and will resist a change in pH. 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 H+ and A - . In both instances. [H+] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH = p Ka + log [A - ]/[HA] What is the pH of a buffer prepared by adding 0.405mol of the weak acid H A to 0.406mol of N in 2.00 L of solution? The dissociation constant Ka of H A is 5.66 Times 10- 7 . Express the pH numerically to three decimal places. What is the pH after 0.150mol of HC1 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 solution of a weak acid (H A ) and its conjugate base (A - ), HA (aq) H + (aq) + A- (aq) is called a buffer and will resist a change in pH. 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 H+ and A - . In both instances. [H+] tends to remain constant. The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH = p Ka + log [A - ]/[HA] What is the pH after 0.195mol 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.

Explanation / Answer

Part A

ph=6.25

part B

pH=6.05

Part C

pH=6.53

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