Advertisements
Advertisements
Question
The values of Van’t Hoff factors for KCl, NaCl and K2SO4, respectively, are ______.
Options
2, 2 and 2
2, 2 and 3
1, 1 and 2
1, 1 and 1
Advertisements
Solution
The values of Van’t Hoff factors for KCl, NaCl and K2SO4, respectively, are 2, 2 and 3.
Explanation:
\[\ce{KCl (K+ + Cl)}\] and \[\ce{NaCl (Na+ + Cl)}\] ionize to give 2 ions and \[\ce{K2SO4(2K+ + SO^{-}4)}\] ionizes to give 3 ions thus, van’t Hoff factors for \[\ce{KCl}\], \[\ce{NaCl}\] and \[\ce{K2SO4}\] are 2, 2 and 3 respectively.
APPEARS IN
RELATED QUESTIONS
The substance ‘X’, when dissolved in solvent water gave molar mass corresponding to the molecular formula ‘X3’. The van’t Hoff factor (i) is _______.
(A) 3
(B) 0.33
(C) 1.3
(D) 1
Calculate the amount of benzoic acid (C6H5COOH) required for preparing 250 mL of 0.15 M solution in methanol.
Phenol dimerizes in benzene having van’t Hoff factor 0.54. What is the degree of association?
The van’t Hoff factor (i) accounts for ____________.
We have three aqueous solutions of NaCl labelled as ‘A’, ‘B’ and ‘C’ with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van’t Hoff factor for these solutions will be in the order ______.
Van’t Hoff factor i is given by the expression:
(i) i = `"Normal molar mass"/"Abnormal molar mass"`
(ii) i = `"Abnormal molar mass"/"Normal molar mass"`
(iii) i = `"Observed colligative property"/"Calculated colligative property"`
(iv) i = `"Calculated colligative property"/"Observed colligative property"`
Van't Hoff factor I is given by expression.
What is the expected each water van't Hoff factor for and K4[F4(CN6)] when it completely dissociated in waters.
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 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 ______.
When 19.5 g of F – CH2 – COOH (Molar mass = 78 g mol−1), is dissolved in 500 g of water, the depression in freezing point is observed to be 1°C. Calculate the degree of dissociation of F – CH2 – COOH.
[Given: Kf for water = 1.86 K kg mol−1]
Why is the value of van't Hoff factor for ethanoic acid in benzene close to 0.5?
Why is boiling point of 1 M NaCl solution more than that of 1 M glucose solution?
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)
