A mixture is prepared by dissolving 1.70 g of ammonia gas and 5.35 g of ammonium chloride in distilled water and making up the volume to 100 mL.
Kb= 1.75 x10-5 at the particular temperature for NH3(aq)
The pH of the mixture would be:
a) 2.38
b) 9.24
c) 4.76
d) 11.68
e) 10.45
first calculate Molarity of NH3 and NH4Cl
Molarity = (W/MW) (1000 / V in mL)
[NH3] = (1.70 / 17)(1000 / 100) = 1.0 M
[NH4Cl] = (5.35 / 53.49) (1000/100) = 1.0 M
mixture of NH3 and NH4Cl act as basic buffer
pOH = pKb + log [NH4Cl] / [NH3]
pKb = - log Kb = - log [1.75 x10-5] = 4.75
pOH = 4.75 + log [1]/ [1]
pOH = 4.76
pH = 14 - 4.76
pH = 9.24
answer = option b = 9.24
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