How does the degree of ionization (assum...

How does the degree of ionization (assuming lt lt 1)` of a weak electroyte vary with concentration ? Give exact relationship.

Text Solution

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`alpha=sqrt(K_(a)//C) or alpha prop 1//sqrt(C)`, i.e., degree of dissociation is inversely proportional to the square root of molar concentration of the solution.

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If alpha is the degree of ionization, C the concentration of a weak electrolyte and K_(a) the acid ionization constant , then the correct relationship between alpha and C is

`alpha^(2) = sqrt(K_(a)/C)`

`alpha^(2) = sqrt(C/K_(a))`

`alpha= sqrt(K_(a)/C)`

`alpha = sqrt(C/K_(a))`

If alpha is the degree of ionization, C the concenr=tration of a weak electrolyte and K_(a) the acid ionization constant, then the correct relationship between alpha , C and K_(a) is

`alpha^(2) = sqrt((K_(a))/(C))`

`alpha^(2) = sqrt((C)/(K_(a))`

`alpha = sqrt((K_(a))/(C))`

`alpha = sqrt((C)/(K_(a))`

If C the concentration of a weak electrolyte , alpha is the degree of ionization and K_a is the acid ionization constant , then the correct relationship between alpha , C and K_a is

`a^2=sqrt((K_a)/C)`

`a^2=sqrt((C)/(K_a))`

`alpha = sqrt((C)/(K_a))`

`alpha = sqrt ((K_a)/(C))`