Advertisements
Advertisements
Question
Calculate Van't Hoff factor for an aqueous solution of K3 [Fe(CN)6] if the degree of dissociation (α) is 0.852. What will be boiling point of this solution if its concentration is 1 molal? (Kb = 0.52 K kg/mol)
Advertisements
Solution
K3 [Fe(CN)6] gives 4 ions in aqueous solution
i = 1 + (n - 1) α
i = 1 + (4 - 1) × 0.852
i = 3.556
ΔTb = iKb m
= 3.556 × 0.52 × 1
= 1.85
Tb = 101.85°C
APPEARS IN
RELATED QUESTIONS
Derive van’t Hoff general solution equation.
Define the term Abnormal molar mass
Give reasons for the following
Elevation of the boiling point of 1 M KCl solution is nearly double than that of 1 M sugar solution.
The Van't Hoff factor (i) for a dilute aqueous solution of the strong elecrolyte barium hydroxide is (NEET) ______.
Phenol dimerizes in benzene having van’t Hoff factor 0.54. What is the degree of association?
Van't Hoff factor I is given by expression.
Maximum lowering of vapour pressure is observed in the case of ______.
Geraniol, a volatile organic compound, is a component of rose oil. The density of the vapour is 0.46 g L–1 at 257°C and 100 mm Hg. The molar mass of geraniol is ______ g mol–1. (Nearest Integer)
[Given: R = 0.082 L atm K–1 mol–1]
A storage battery contains a solution of H2SO4 38% by weight. At this concentration, Van't Hoff Factor is 2.50. At the battery content freeze temperature will be ______ K.
(Kf = 1.86 K Kg mol−1)
A molecule M associates in a given solvent according to the equation \[\ce{M <=> (M)_n}\]. For a certain concentration of M, the van't Hoff factor was found to be 0.9 and the fraction of associated molecules was 0.2. The value of n is ______.
