A certain weak acid, HA, has a Ka value of 7.4×10−7. Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. Part B Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures, and include the appropriate units.
part A)
Ka = 7.4 x 10^-7
C = 0.10 M
x = [H+] = sqrt (Ka x C)
x = sqrt (7.4×10^−7 x 0.1)
x = 2.72 x 10^-4
percent ionization of HA = (2.72 x 10^-4 ) x 100 / 0.1
= 0.27%
part B)
x = sqrt (7.4×10^−7 x 0.01)
x = 8.60 x 10^-5
percent ionization = 8.60 x 10^-5 x 100 / 0.01
= 0.86 %
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