The pH of a buffer solution that is 0.50 M in NH 3 and 0.20 M in NH 4 Cl is 9.65
ID: 589182 • Letter: T
Question
The pH of a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl is 9.65. If 0.0150 mole of solid NaOH is added to 500.0 mL of the buffer, then which statement best explains what happened to the pH of the system?
A.
NaOH reacts with NH4Cl to produce more NH3. The ratio of NH3 to NH4Cl in the Henderson-Hasselbalch equation decreases, so the pH decreases slightly.
B.
NaOH reacts with NH4Cl to produce more NH3. The ratio of NH3 to NH4Cl in the Henderson-Hasselbalch equation increases, so the pH increases slightly.
C.
The pH of the system increases significantly because strong base is added.
D.
NaOH reacts with NH3 to produce more NH4Cl. The ratio of NH3 to NH4Cl in the Henderson-Hasselbalch equation increases, so the pH increases slightly.
E.
The pH of the system does not change because it is a buffer.
F.
The pH of the system decreases significantly because strong acid is added.
G.
NaOH reacts with NH3 to produce more NH4Cl. The ratio of NH3 to NH4Cl in the Henderson-Hasselbalch equation decreases, so the pH decreases slightly.
Explanation / Answer
Ans is E. Ph does not change as it is a buffer solution.
Because base which we add has very less concentrated though it is a strong base but it can.be nullified by buffer system.
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