A 0.18 M solution of a weak base A‑ reacts with H2O such that at equilibrium...
A 0.18 M solution of a weak base A‑ reacts with H2O such that at equilibrium 99.7% of the compound remains in the A- form. Given this information, what is the pH of this solution to the nearest tenths?
Homework Answers
A- + H2O —> AH + OH-
99.7 % is remaining as A-
so,
[OH-] = 0.3 % of initial concentration
[OH-] = 0.3 % of 0.18 M
[OH-] = 0.3 * 0.18 / 100 = 5.4*10^-4 M
use:
pOH = -log [OH-]
= -log (5.4*10^-4)
= 3.3
use:
PH = 14 - pOH
= 14 - 3.3
= 10.7
Answer: 10.7
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