Which solution should be mixed with 50.0 mL of 0.100M ammonia, (NH3), to make
an effective buffer?
50.0 mL of 0.200 M HCl |
25.0 mL of 0.200 M HCl |
50.0 mL of 0.100 M HCl |
25.0 mL of 0.100 M HCl |
NH3 is base here
So, we need some conjugate acid NH4+
So, if we add HCl such that number of moles of HCl is less than number of mol of NH3, then some of NH3 will convert to NH4+.
So, finally we will have NH3 and NH4+
mol of NH3 present = 0.100 M * 50.0 mL = 5 mmol
option 1:
mol of HCl = 0.200 M * 50.0 mL = 10 mmol
option 2:
mol of HCl = 0.200 M * 25.0 mL = 5 mmol
option 3:
mol of HCl = 0.100 M * 50.0 mL = 5 mmol
option 4:
mol of HCl = 0.100 M * 25.0 mL = 2.5 mmol
option 4 is correct
Answer: 25.0 mL of 0.100 M HCl
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