The degree of dissociation of 1.0 M weak acid, HA 0.5. If 2m of 1.0M HA solution is diluted to 32 ml,the degree of dissociation of the acid and H3O+ concentration in th resulting solution will respectively?
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The degree of dissociation of 1.0 M weak acid, HA 0.5. If 2m of 1.0M HA solution is diluted to 32 ml,the degree of dissociation of the acid and H3O+ concentration in th resulting solution will respectively?
Explanation:
Given,
α=0.5%=0.005 and C=0.1 M
The expression for the degree of dissociation is
α= √K a/C
0.005= √K a/0.1
K a =2.5×10 −6
When the solution is diluted, the molarity of the solution is given by the following expression.
M 1 V 1=M 2V 2
or 2×1=32×M 2
Therefore, M 2 = 1/16
For this diluted solution, α=√Ka/ C
=0.632%.
The hydrogen ion concentration is [H
+ ]=cα=
1/16×0.00632=3.955×10 −4
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