Solutions practice · Mixed difficulty

The K for ${\mathrm{I}_2}$ between $\mathrm{C}{\mathrm{S}_2}$ and ${\mathrm{H}_2}\mathrm{O}$ is 588 in favour of $\mathrm{C}{\mathrm{S}_2}$. One litre of aqueous solution containing 1 g of ${\mathrm{I}_2}$ is shaken with 50 mL of $\mathrm{C}{\mathrm{S}_2}$. What will be the amount of ${\mathrm{I}_2}$ in aqueous layer?

On mixing $10\,mL$ of carbon tetrachloride with $10\,mL$ of benzene the total volume of the solution is:

What is the molality of ethyl alcohol (mol. wt. = 416) in aqueous solution which freezes at $- 10^\circ \mathrm{C}?.\;\left( {{K_f}\;\mathrm{for}\;\mathrm{ water} = 1.86\;\mathrm{K}\;\mathrm{ molalit}{\mathrm{y}^{ - 1}}} \right)$

${{K_f}}$ for water is ${1.86\;K\;kg\;\mathrm{mo}{\mathrm{l}^{ - 1}}}$. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol $\left( {{\mathrm{C}_2}{\mathrm{H}_6}{\mathrm{O}_2}} \right)$ must you add to get the freezing point of the solution lowered to $\mathrm{ - 2}\mathrm{.8}^\circ \mathrm{C}$?

Which of the following statements is false?

Two solutions of different osmotic pressure. The solution of lower osmotic pressure is called

Which of the following statements is true about bends?

Assertion (A): Van't Hoff factor for benzoic acid in aqueous medium is 2 assuming complete ionisation.

Reason (R): Van't Hoff factor for $100 \%$ ionised solute equal to the number of ions produced.

18g glucose $\left( {{C_6}{H_{22}}{O_6}} \right)$ is added to 178.2 g water. The vapor pressure of water (in torr) for this aqueous solution is.

Which one of the following electrolyte has the same value of the vant Hoff factor (i) as that of ${A_2}{\left( {S{O_4}} \right)_3}$ (if all are 100% ionised)

Which is correct representation of phase rule?

Assume a living cell with $0.9 \%(\omega / \omega)$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.

(Consider the data upto first decimal place only)

The cell will:

One mole of non-volatile solute is dissolved in two mole of water. The vapour pressure of the solution relative to that of water is :

Vapour pressure of a solvent containing non-volatile solute is :

If the temperature increase from $0^\circ C\;to\;50^\circ C\;$ at atmospheric pressure, which of the following processes is expected to take place more in case of liquids?

The natural semipermeable membrane is :

Which of the given solutions has highest osmotic pressure?

A solution containing 10 g per ${\mathrm{d}{\mathrm{m}^3}}$ of urea (mol. mass = 60) is isotonic with a 5% (wt.by vol.) solution of a non-volatile solute. The molecular mass (in $\mathrm{g}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$) of non-volatile solute is :

Colligative properties are used for the determination of

The relationship which describes the variation of vapour pressure of a liquid with temperature is called :

What happen at increasing pressure at constant temperature

Assertion (A): Experimentally determined molar mass is always lower than the true value.

Reason (R): Lower molar mass is due to dissociation of solute into ions.

The energy that opposes the dissolution of a solute in a solvent is called :

If 0.2 m aqueous solution of ${K_4}\left[ {Fe{{\left( {CN} \right)}_6}} \right]$ is 100% ionized then the freezing point of the solution will be $\left( {{K_f} = 1.86\,K\,kg\,mo{l^{ - 1}}} \right)$

The freezing point of an aqueous solution of ${KCN}$ containing 0.2 mole/kg water was $-0.8^{\circ} \mathrm{C}$. On addition of 0.1 mole of ${Hg}({CN})_2$ in the solution containing 1 kg of water, the freezing point of the solution was $-0.6^{\circ} \mathrm{C}$. Assuming that the complex is formed according to the following equation:
${Hg}({CN})_2+{mCN}^{-} \longrightarrow {Hg}({CN})_{{m}+2}^{-{m}}$ and ${Hg}({CN})_2$ is the limiting reagent, the value of $4 \mathrm{~m}$ is:

The melting point of most of the solid substances increase with an increase of pressure acting on them. However, ice melts at a temperature lower than its usual melting point, when the pressure increase. This is because :

Molarity of a given orthophosphoric acid solution is 3 M. It’s normality is

The van't Hoff factor (i) for a dilute aqueous solution of glucose is:

Density of a 2.05 M solution of acetic acid in water is 1.02 g/mL. The molality of the solution is

Assertion (A): Molality is independent of temperature.

Reason (R): There is no volume factor in the expression of molality.