When `20 g` of naphthoic acid `(C_(11)H_(8)O_(2))` is dissolved in `50 g` of benzene `(K_(f)=1.72 K kg mol^(-1))`, a freezing point depression of `2 K` is observed. The Van't Hoff factor (i) is
When 20g of naphtholic acid (C_(11)H_(8)O_(2)) is dissolved in 50g of benzene (K_(f) = 1.72 K kg mol^(-1)) a freezing point depression of 2K is observed. The van'f Hoff factor (i) is
When 20 g of napthanoic acid (C_(11)H_(8)O_(2)) is dissolved in 50 g of benzene (K_(f)=1.72 K kg/mol) a freezing point depression of 2 K is observed. The van't Hoff factor (i) is
1575.2 g of C_(6)H_(5)OH (phenol) is dissolved in 960 g of a solvent of solvent of K_(f)=14 K kg mol^(-1) . If the depression in freezing point is 7 K , then find the percentage of phenol that dimerizes.
Two grams of benzoic acid (C_(6)H_(5)COOH) dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K . Molal depression constant for benzene is 4.9 K kg^(-1)"mol^-1 . What is the percentage association of acid if it forms dimer in solution?
Two grams of benzoic acid (C_(6)H_(5)COOH) dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K . Molal depression constant for benzene is 4.9 K kg^(-1)"mol^-1 . What is the percentage association of acid if it forms dimer in solution?
When 0.4 g of acetic acid is dissolved in 40 g of benzene, the freezing point of the solution is lowered by 0.45 K. Calculate the degree of association of acetic acid. Acetic acid forms dimer when dissolved in benzene. ( K_(f) for benzene = 5.12 K kg mol^(-1) at.wt. C = 12, H = 1, O = 16)
2g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62K .Molal depression constant for benzene is 4.9Kkgmol^(-1) .What is the percentage association of acid if it forms dimer in solution?
2g of benzoic acid (C_(6)H_(5)COOH) dissolved in 25g of benzene shows a depression in freezing point equal to 1.62K .Molal depression constant for benzene is 4.9Kkgmol^(-1) .What is the percentage association of acid if it forms dimer in solution?
K_(2)HgI_(4) is 40% ionised in aqueous solution. The value of its van't Hoff factor (i) is :
The freezing point of a solution containing of 0.2g of acetic acid in 20.0g of benzene is lowered 0.45^(@)C . Calculate. (i) the molar mass of acetic acid from this data (ii) Van't Hoff factor [For benzene, K_(f)=5.12K kg "mol"^(-1) ] What conclusion can you draw from the value of Van't Hoff factor obtained ?
