# What is degree of ionization is respect of weak acids and weak bases? Derive the relationship between degree of ionization (`alpha`) and ionization constant `(K_(a))` for thke weak acid HX.

Updated On: 24-8-2021

700+

000+

Answer

Text Solution

Degree of Ionization

(alpha)

: <br> The extent of ionization (or) dissociation of a weak acid or weak base is termed as its Degree of ionization

(alpha)

."Let the concentration of weak acid (HX).be.c molès/it and the degree of ionization be

.alpha.

. Hence at equilibrium, <br>

{:(HX hArr, H^(+) ,+X^(-)),(C(1-alpha),C alpha ,C alpha):}

<br> If

.alpha

. is neglected compared to one in denominator, <br> We have

K_(a)=Calpha^(2) rArr alpha^(2)=(K_(a))/(C) rArr alpha= sqrt((K_(a))/(C))

<br> Similar equation can be written for the ionization of weak base (BOH) in aq. solution. <br>

{:(BOH, overset(H_(2)O) hArr, B^(+)+OH^(-)),(C(1-alpha), C alpha, C alpha):}

<br>

K_(b)=([B^(+)][OH^(-)])/([BOH])=(C alpha xx C alpha)/(C(1-alpha))=(Calpha^(2))/((1-alpha))

<br>

:. K_(b)=(Calpha^(2))/((1-alpha))

<br> Neglecting .a. in the denominator, we have <br>

K_(b)=Calpha^(2) rArr alpha^(2) =(K_(b))/(C)

<br>

:. alpha= sqrt((K_(b))/(C))

<br> Therefore strengths of two acids or two bases are compared generally by their

K_(a)

or

k_(b)

values: Higher

K_(a)

or

k_(b)

value, stronger is the acid or base.

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