In terms of #pK_a#, which acid will be stronger? How does #pK_a# relate to #pK_b#?
2 Answers
Explanation:
We recall (i) that
and that
And (ii) in aqueous solution under standard conditions,
- .1 M of a weak acid
2 . Ka =#8 xx 10-6# - pKb =
# 4.5 #
Explanation:
Acid have a low pH the stronger the acid the lower the pH.
Bases have a high pH the strong the base the higher the pH.
-
The .1 Molar solution of weak acid will have a higher pH than a strong acid.
-
The Ka of
# 10^-6# will be a weaker acid than one with a Ka of# 2xx 10^-3# so have a higher pH. -
The pkb of 4.5 is stronger than than a base with a pkb of 6.5.
so the pkb of 4.5 will have a higher pH.