Which solution has the highest osmotic pressure?

1. 0.1 M NaCl                2. 0.5 M Urea

3. 0.1 M MgCl₂              4. 0.2 M NaCl   

Assertion : Perfectly ideal solution is not possible with respect to binary solution of two liquids.

Reason : No two substances can have exactly the same nature of intermolecular forces & also of the same magnitude.

Assertion :  When a cell is placed in hypertonic solution, it shrinks.

Reason : Reverse osmosis is used for desalination of water.

Assertion(A): The difference in the boiling points of equimolar solution of HCI and HF decreases as their molarity is decreased.

Reason(R): The extent of dissociation decreases steadily with increasing dilution.

1. Both assertion and reason are true and the reason is the correct explanation of the assertion 
2. Both assertion and reason are true but the reason is not the correct explanation of the assertion 
3. Assertion is true but the reason is false 
4. Both assertion and reason are false 

Assertion : The molar mass obtained for benzoic acid in benzene is found to be nearly twice

Reason : Benzoic acid has the formula $\mathrm{HOOC}$

Assertion : When 'a' mL of a 0.1 molal urea solution is mixed with another 'b' mL of 0.1 molal glucose

                   solution, the boiling point of the solution is no different from the boiling points of the

                   samples prior to mixing but if 'a' mL of 0.1 molal urea is mixed with 'b' mL of 0.1 molal HF

                   the boiling point of the mixture is different from the boiling points of the separate

                   samples.

Reason : HF is an electrolyte (weak) whereas glucose is a non electrolyte.

The equal weight of a solute is dissolved in an equal weight of two solvents A and B to form a very dilute solution. The relative lowering of vapour pressure for solution B has twice the relative lowering of vapour pressure for solution A.

If ${\mathrm{M}}_{\mathrm{A}}$ and ${\mathrm{M}}_{\mathrm{B}}$ are the molecular weights of solvents A and B respectively, then:

1. ${\mathrm{M}}_{\mathrm{A}}$ = ${\mathrm{M}}_{\mathrm{B}}$

2. ${\mathrm{M}}_{\mathrm{B}}$ = 2${\mathrm{M}}_{\mathrm{A}}$

3. ${\mathrm{M}}_{\mathrm{A}}$ = 4${\mathrm{M}}_{\mathrm{B}}$

4. ${\mathrm{M}}_{\mathrm{A}}$ = 2${\mathrm{M}}_{\mathrm{B}}$

Calculate the boiling point of solution when 4 g of MgSO₄ (M = 120 g mol^-1) was dissolved in 100 g of water, assuming MgSO₄ undergoes complete ionization 

(K_b for water is 0.052 K kg mol²¹)                                                           (3)

Freezing point of an aqueous solution is -0.166$°$C. Elevation of boiling point of same solution would be-

(K_b = 0.512 K m^-1 and K_f = 1.66 K m^-1)

Mole fraction of solute in an aqueous solution that boils at 100.104 is :

( $K_b$ for $H_{2}O$ = 0.52 K $molalit{y}^{-1}$)

1.  0.008

2.  0.004

3.  0.061

4.  0.996