Worksheet: Buffer Capacity

In this worksheet, we will practice calculating the maximum amount of acid/base a buffer can neutralize before pH is significantly affected.

Q1:

What mass of solid N a C H C O · 3 H O 3 2 2 in grams must be added to 0.300 L of a 0.50 M acetic acid solution to produce a buffer with a pH of 5.00? Assume a negligible change in volume as the solid is added. The 𝐾 a of acetic acid is 1 . 8 × 1 0 .

Q2:

Which of the following, if added to a buffer of acetic acid and sodium acetate, would decrease the concentration of C H C O H 3 2 ?

  • A C H C O H 3 2
  • B N a C l
  • C K C H C O 3 2
  • D H C l
  • E K O H

Q3:

Which of the following, if added to a buffer of acetic acid and sodium acetate, would decrease the concentration of C H C O 3 2 ?

  • A N a C l
  • B K C H C O 3 2
  • C C H C O H 3 2
  • D H C l
  • E K O H

Q4:

Which of the following, if added to a buffer of ammonia and ammonium nitrate, would decrease the concentration of N H 3 ?

  • A H I
  • B N H 3
  • C K I
  • D N H C l 4
  • E N a O H

Q5:

Which of the following, if added to a buffer of ammonia and ammonium nitrate, would decrease the concentration of N H 4 + ?

  • A N a O H
  • B H I
  • C K I
  • D N H 3
  • E N H C l 4

Q6:

Why does the pH not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H P O 3 4 and N a H P O 2 4 , a salt of its conjugate base?

  • A H P O 3 4 is amphiprotic and reacts with and neutralizes both acids and bases; N a H P O 2 4 then converts to H P O 3 4 , restoring the pH.
  • B N a H P O 2 4 reacts with excess base, while H P O 3 4 reacts with excess acid.
  • CExcess base is removed by reaction with H P O 3 4 , while excess acid is removed by reaction with N a H P O 2 4 .

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