What is the pH of a 0.10M solution of methylamine (:NH2CH3) From Table 15.8, Kb = 4.4 x 10-4.
Please show me how to work it out, thank you!
ans)
Here
CH3NH2 + H2O -----> CH3NH3+ + OH-
0.10 ............................x.................x
Kb = [Ch3NH3+][OH-]/[CH3NH2]
4.4*10^-4 = (x)*(x)/0.10
x = [OH-] = 0.663*10^-2
As we know that
pH = 14 - p[OH]
= 14 - (- log[OH-])
= 14 + log[OH-]
= 14 + log(0.663*10^-2)
= 11.82
What is the pH of a 0.10M solution of methylamine (:NH2CH3) From Table 15.8, Kb =...
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