Define degree of dissociation.

Conductivity of 0.00241 M acetic acid solution is 7.896 xx 10^(-5) S cm^(-1) . Calculate its molar conductivity in this solution. If Lambda_(m)^(@) for acetic acid be 390.5 S cm^(2) "mol"^(-1) , what would be its dissociation constant? (i) First , find molar conductivity using the formula,, Lambda_(m) = ( K xx 1000)/( C ) (ii) Then find degree of dissociation ( alpha) and dissociation constant ( K_(a)) by using formula alpha = ( Lambda_(m))/( Lambda_(m)^(@)) and K_(a) = ( C alpha^(2))/( 1-alpha) respectively.

Find the pH of a 0.01 M solution of acetic acid having degree of dissociation 12.5%.

State Ostwald dilution law? Derive the relationship between degree of dissociation and concentration of weak electrolyte.

From Kohlrausch's law how can you find the degree of dissociation of a weak electrolyte ?

If alpha is the degree of dissociation of Na_2SO_4 . Van’t Hoff’s factor (i) used for calculating the molecular mass is

The molecular weight of NaCl determined by studying freezing point depression of its 0.5% aqueous solution is 30. The apparent degree of dissociation of NaCl is:

Calculate the amount of acetic acid present in one litre, having degree of dissociation equal 1% and K_(a) = 1.8 xx 10^(-5) .