(a) Calculate the Delta T_f (depression in freezing point) of 0.4 m solution of CH_3 COOH in benzene solution. K_f = x K kg mol^-1 . (b) Calculate the Delta T_f of 0.2 m solution of an acid (RCOOH) is conc. H_2 SO_4 , in which (Rc -= O^(oplus)) acylium ion is formed. K_f = x K kg mol^-1 . ( c) Calculate the Delta T_f of 0.3 m solution of an acid (RCOOH) in conc. H_2 SO_4 in which a protonated acid (R-underset(.^o+OH)underset(||)(C)-OH) (I) is formed. K_f = x K kg mol^-1 .
Molal depression constant for a solvent is 4.0 K kg "mol"^(-1) The depression in the freezing point of the solvent for 0.03 "mol kg^(-1) solution of K_(2)SO_(4) is: (Assume complete dissociation of the electrolyte)
if the elevation in boiling point of a solution of non-volatile, non-electrolytic and non-associanting solute in solvent ( K_(b) =xK.kgt."mol"^(-1) )is yK,then the depression in freezing point of solution of same concentration would be ( K_(f) )of the sovent = zk.kg"mol"^(-1) )
What is the depression in freezing point of a solution of non-electrolyte if elevation in boiling point is 0.13K ? (k_(b)=0.52 mol^(-1) kg, k_(f)= 1.86 mol^(-1) kg)
Elevation in boiling point of a solution of non-electrolyte in CCl_(4) is 0.60^(@)C . What is the depression in freezing point for the same solution? K_(f)(CCl_(4)) = 30.00 K kg mol^(-1), k_(b)(CCl_(4)) = 5.02 k kg mol^(-1)
