nicotinic acid (Ka =1.4 * 10 raise to power -5) is represented by the formula HNiC. calculate its percentage dissociation in a solution which contains 0.10 mole of nicotinic acid per 2 litre of solution ?
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H NiC <=========> H+ + NiC-
(0.05 - x) M. ... .. . .. .. .. . x M. . . . x M
Initial concentration of acid = 0.1/2 =0.05 Molar.
Let x moles dissociate into ions.
Ka = [ H+] * [ Ni C-] ÷ [ H Ni C]
1.4*10^-5= x *x /(0.05-x).
You can solve this quadratic.
OR: : x is very small compared to 0.05. So take 0.05 -x = 0.05. Find answer approximately.
Concentration of H+ = x = 0.05 * sqrt (14) *10^-3 Molar. ...
% dissociation = x/0.05 ×100 = sqrt(0.14) %
(0.05 - x) M. ... .. . .. .. .. . x M. . . . x M
Initial concentration of acid = 0.1/2 =0.05 Molar.
Let x moles dissociate into ions.
Ka = [ H+] * [ Ni C-] ÷ [ H Ni C]
1.4*10^-5= x *x /(0.05-x).
You can solve this quadratic.
OR: : x is very small compared to 0.05. So take 0.05 -x = 0.05. Find answer approximately.
Concentration of H+ = x = 0.05 * sqrt (14) *10^-3 Molar. ...
% dissociation = x/0.05 ×100 = sqrt(0.14) %
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