Calculate the pH of a 1.40×10-1 M aqueous solution of hydrazine hydrochloride (H2NNH3Cl).
(For hydrazine, H2NNH2, Kb = 3.00×10-6.)
H2NNH3+ => H2NNH2 + H+ ; Ka = Kw/Kb = (10^-14)/(3.00*10^-6) = 3.34 * 10^-9
0.140 0 0
-x +x +x
(0.140-x) (x) (x)
Ka = (3.34*10^-9) = (x^2) / (0.140-x)
Rearrange and quadratic formula gives => x = 2.16 * 10^-5 M
pH = -log(2.16*10^-5) = 4.7
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