Determine the pH (to two decimal places) of the following solutions. If the 5% approximation is valid, use the assumption to compute pH.
8.72×10-3 M sodium hydrogen sulfate
pKa hydrogen sulfate ion is 1.92
8.73×10-3 M trifluoroacetic acid
pKa trifluoroacetic acid is 0.20
8.20×10-3 M ethylamine
pKa ethylammonium ion is 10.87
2.51×10-1 M sodium nitrite
pKa nitrous acid is 3.37
sodium hydrogen sulfate:
PH = 1/2Pka-1/2 log[C]
PH = 1/2x 1.92- 1/2log[8.72x10-3]
PH = 0.96 - 1/2[log8.72-3]
PH = 0.96- 1/2 [0.9405-3]
PH = 0.96+1.029
PH =1.98
Trifluoroacetic acid:
pKa trifluoroacetic acid is 0.20
concentration 8.73×10-3 M
PH = 1/2Pka-1/2 log[C]
PH = 1/2x 0.20- 1/2log[8.73x10-3]
PH = 0.1 - 1/2[log8.73-3]
PH = 0.1- 1/2 [0.9410-3]
PH = 0.1+1.029
PH = 1.129
Ethylamine:
pKa ethylammonium ion is 10.87
concentration 8.20×10-3 M
PH = 1/2Pka-1/2 log[C]
PH = 1/2x 10.87- 1/2log[8.20x10-3]
PH = 0.1 - 1/2[log8.20-3]
PH = 0.1- 1/2 [0.9138-3]
PH = 0.1+1.043
PH = 1.143
sodium nitrite:
pKa nitrous acid is 3.37
concentration 2.51×10-1 M
PH = 1/2Pka-1/2 log[C]
PH = 1/2x 3.37- 1/2log[2.51x10-1]
PH = 1.685 - 1/2[log2.51 -1]
PH =1.685- 1/2 [0.3996-1]
PH = 1.685+0.3002
PH = 1.985
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