How many moles of NH3 are required in a 1.00L solution to create a buffer with a pH of 9.13 if the solution contains 0.61 moles of NH4Cl? Kb NH3 = 1.8 x 10-5?
For NH4Cl/NH3 (i.e. NH4Cl/NH4OH) buffer,
NH3 + H-OH <------> NH4+ + OH- . For NH3, Kb = 1.8 x 10-5 .
pH = 9.13 hence, pOH = 14 - 9.13 = 4.87,.........( pH+ pOH = 14)
Kb = 1.8 x 10-5,
pKb = -log(Kb)
pKb = -log(1.8x 10-5)
pKb = 4.74
[NH4Cl] = 0.61
[NH3] = ?
WE have Handerson's equation as,
pOH = pKb + log{[Salt]/[Base]}
pOH = pKb + log{[NH4Cl]/[NH3]}
Let us put all the known values,
4.87 = 4.74 + log(0.61 / [NH3])
log(0.61 / [NH3] ) = 4.87-4.74
log(0.61 / [NH3] ) = 0.13
0.61 / [NH3] = Antilog(0.13)..........(say 100.13 i.e. antilog to the base 10)
0.61 / [NH3] = 1.349
[NH3] = 0.61 / 1.349
[NH3] = 0.45 mole.
Hence 0.45 moles of NH3 are required in a 1 L solution to create a buffer of pH 9.13 if solution contains 0.61 moles of NH4Cl.
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