A 0.20M solution of a weak monoprotic acid is 3.0% ionized. What is the approximate pH...
A 0.20M solution of a weak monoprotic acid is 3.0% ionized. What is the approximate pH of the solution? show step by step solution. type solution. I won't give a 5 star rating if you scribble it down and i can't read your writing.
a) 11.0 to 12.0
b) 2.0 to 3.0
c) 4.0 to 5.0
d) 9.0 to 10.0
Homework Answers
Let the acid be HA and it dissociates as:
% ionisation = x*100/0.20
3.0 = x*100/0.20
x = 0.006 M
use:
pH = -log [H+]
= -log (0.006)
= 2.22
Answer: b
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