Van't Hoff's Factor

The osmotic pressure of equimolar solutions of ${\mathrm{BaCl}}_2,\mathrm{NaCl}$ and glucose will be in the order

Helium is added to oxygen used by deep sea divers because :

Which one of the following electrolytes has the same value of van’t Hoff factor $\mathrm{i}$ as that of ${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3$ (if all are $100\%$ ionised)?

$200 \mathrm{ml}$ of aqueous solution of protein contains its $1.26 \mathrm{g}.$ The osmotic pressure of this solution at is $2.57\times {10}^{-3} \mathrm{bar}.$ The molar mass of protein will be

During osmosis, flow of water through a semipermeable membrane is:

Assertion:- At high altitude cooking food is difficult.
Reason:- Water boils at high temprature.

Assertion:- When two volatile liquids are mixed then vapour pressure of one increases and other decreases.

Reason:- Vapour pressure of solution decreases.

Assertion: Elevation in boiling point of $0.1\mathrm{MKCl}$ and $0.1{\mathrm{MCaCl}}_2$ is same.
Reason: Because colligative properties depends on molarity only.

Assertion:- Isotonic solutions don't show net phenomenon of osmosis.

Reason:- Isotonic solutions have equal osmotic pressure at constant temp.

Assertion:- A solution which contains one gram equivalent of solute per litre of the solution is called normal solution.

Reason:- A normal solution mean a solutions in which the solute doesn't associate or dissociate.

Assertion:- The sum of the mole fraction of all the components is unity.

Reason:- Mole fraction is a temperature dependent mode of concentraction.

The molar mass of $\mathrm{NaCl}$ determined by the osmotic pressure method will be:-

The substance when dissolved in water would decrease the vapour pressure of water to the greatest extent is:-

$0.5$mol $\mathrm{NaCl}$ is dissolved in $500{\mathrm{gH}}_2\mathrm{O}$. Then determine freezing point and boiling point of solution.

Given ${\left({\mathrm{K}}_{\mathrm{f}}\right)}_{{\mathrm{H}}_2\mathrm{O}}=1.8 {\mathrm{Kkgmol}}^{-1}$

${\left({\mathrm{K}}_{\mathrm{b}}\right)}_{{\mathrm{H}}_2\mathrm{O}}=0.5 {\mathrm{Kkgmol}}^{-1}$

Strength of ${\mathrm{H}}_2{\mathrm{O}}_2$ is $15.18 {\mathrm{gL}}^{-1}$, then it is equal to:-

$0.5$ molal aqueous solution of a weak acid $\left(\mathrm{HX}\right)$ is $20\%$ ionised. If ${\mathrm{K}}_{\mathrm{f}}$ for water is $1.86{\mathrm{Kkgmol}}^{-1},$ the lowering in freezing point of the solution is:

The following solutions have equal concentrations. Which one will show minimum osmotic pressure?

The molarity of $0.2{\mathrm{NNa}}_2{\mathrm{CO}}_3$ solution will be:

Mole fraction of glycerine $\left({\mathrm{C}}_3{\mathrm{H}}_5(\mathrm{OH}{)}_3\right)$ in a solution of $36\mathrm{g}$ of water and $46\mathrm{g}$ of glycerine is:

$A 5\%$ solution (by mass) of cane sugar in water has freezing point of $271\mathrm{K}$ and freezing point of pure water is $273.15\mathrm{K}$. The freezing point of a $5\%$ solution (by mass) of glucose in water is: