Calculate the buffer ratio for pH = 9.
Recall the Henderson-Hasselbalch equation:
pKa of NH4+= 9.24
A 100.0-ml buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. What mass of HCl can this buffer neutralize before the pH falls below 9.00?
If the same volume of the buffer were 0.250 M in NH3 and 0.400 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
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