A 0.1 molal aqueous solution of a weak electrolyte, HX, freezes at -0.208 °C. Assuming ideal behavior, what is the van't Hoff factor (i) for HX in this solution? (K$_f$ for water = 1.86 K kg mol$^{-1}$)

Consider the following aqueous solutions and assume 100% ionisation in electrolytes

I. 0.1 m urea

II. 0.04 m ${\rm{A}}{{\rm{l}}_2}{\left( {{\rm{S}}{{\rm{O}}_4}} \right)_3}$

III. 0.05 m ${\rm{CaC}}{{\rm{l}}_2}$

IV. 0.005 m NaCl

The correct statement regarding the above solution is

A solution of protein (extracted from crabs) was prepared by dissolving 0.75 g in $125\;{\rm{c}}{{\rm{m}}^3}$ of an aqueous solution. At $4^\circ C$ an osmotic pressure rise of 2.6 mm of the solution was observed. Then molecular weight of protein is : (Assume density of solution is $1.00\;g/{\rm{c}}{{\rm{m}}^3}$)

A solution of 4.5 g of a pure non-electrolyte in 100 g of water was found to freeze at $0.465^\circ C$. The molecular weight of the solute closest to $({k_f} = 1.86)$

${\rm{0}}{\rm{.004}}\;{\rm{M}}\;{\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is isotonic with 0.01 M glucose.Degree of dissociation of ${\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If ${K_f}$ for water is $1.86\,K.Kg.mo{l^{ - 2}}$, the lowering in freezing point of the solution is

The freezing point depression of $0.001\;m$, ${{\rm{K}}_x}\left[ {{\rm{Fe}}{{\left( {{\rm{CN}}} \right)}_6}} \right]$ is $7.10 imes {10^{ - 3}}\;K\;$. If for water, ${k_f}\;is\;1.86\;K\;kg\;\;{\rm{mo}}{{\rm{l}}^{ - 1}}$, value of x will be

What is the amount of urea dissolved per litre if its aqueous solution is isotonic with 10% cane sugar solution? (mol.wt.of urea =60)

20g of glucose, 10g of urea, and 30g of sucrose are dissolved separately in 500ml of water each. Arrange these solutions in decreasing order of their osmotic pressure.

A solution containing 1.8 g of a compound (empirical formula $C{H_2}O$) in 40 g of water is observed to freeze at $- 0.465^\circ C.$ The molecular formula of the compound is

$({K_f}\;of\;{\rm{ }}water = 1.86\;kg\;{\rm{ }}K\;{\rm{ }}mo{l^{ - 1}})$

When a substance is distributed between two immiscible solvents and remains in the same state in the solvent I, while, dissociates in the solvent II. If the concentration of solute are ${c_{\rm{I}}}\;{\rm{and}}\;{c_{{\rm{II}}}}$ in phase I and II respectively then :