The molarity of a $0.2\mathrm{N}{\mathrm{Na}}_2{\mathrm{CO}}_3$ solution will be [MP PMT 1987]

If 20 ml of 0.4 N NaOH solution completely neutralises 40 ml of dibasic acid. The molarity of acid solution is

H₂SO₄ solution whose specific gravity is 1.98 g ml^–1 and H₂SO₄ by volume is 95%. The molality of the solution will be

The density of H₂SO₄ solution is 1.84 gm ml^–1. In 1 litre solution H₂SO₄ is 93% by (w/v) then, the molality of solution is -

A solution contains 16 gm of methanol and 90 gm of water, mole fraction of methanol is

A solution has 25% of water, 25% ethanol and 50% acetic acid by mass. The mole fraction of each component respectivelywill be

34.2 g of cane sugar is dissolved in 180 g of water. The relative lowering of vapour pressure will be

Lowering in vapour pressure is the highest for -

The Vapour pressure of CCl₄ at 25°C is 143 mm Hg, 0.5 g of a non-volatile solute (mol. wt. 65) is dissolved in 100 ml of CCl₄. The vapor pressure of the solution is-

(Density of ${\mathrm{CCl}}_4=1.58\mathrm{g}/{\mathrm{cm}}^3)$ 

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour pressure in contact with an equimolar solution of benzene and toluene is -

The vapour pressure of a solvent decreases by 10 mm of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be if the decrease in vapour pressure is to be 20 mm of mercury then the mole fraction of the solvent is [CBSE PMT 1998]

A solution containing 3.3 g of a substance in 125 g of benzene (b.p. 80°C) boils at 80.66°C. If K_b for one litre of benzene is 3.28°C, the molecular weight of the substance shall be 

The molal b.p. constant for water is $0{.513}^{o}Ckgmo{l}^{-1}$. When 0.1 mole of sugar is dissolved in 200 g of water, the solution boils under a pressure of 1 atm at

An aqueous solution containing 1 g of urea boils at 100.25°C. The aqueous solution containing 3 g of glucose in the same volume will boil at-

Solution of sucrose (Mol. Mass = 342) is prepared by dissolving 34.2 gm of it in 1000 gm of water. Freezing point of the solution is (K_f for water is 1.86 K kg mol^–1) [AIEEE 2003]

An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7 g of water freezes at 272.817K. If the value of K_f for water is 1.86 K kg mol^–1, the molecular mass of the acid is [AMU 2002]

What is the molality of the solution of a certain solute in a solvent if there is a freezing point depression of 0.184° and if the freezing point constant is 18.4 K kg mol⁻¹

A solution containing 6.8 g of a non ionic solute in 100 g of water was found to freeze at $-0{.93}^{o}C$. The freezing point depression constant of water is 1.86. The molecular weight of the solute is-

The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ is dissolved in 1000 g of water, the solution will freeze at 

The molal freezing point constant for water is 1.86°C/m. Therefore, the freezing point of 0.1 m NaCl solution in water is expected to be [MLNR 1994]

The depression in freezing point of 0.01 M aqueous solutions of urea, sodium chloride and sodium sulphate is in the ratio of [Roorkee 1990; DCE 1994]

The Van't Hoff factor for 0.1 M $\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ solution is 2.74. The degree of dissociation is [IIT 1999]

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

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

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

$(K_b=0.512 and K_f=1.66 K molalit{y}^{-1})$

Which solution has the highest osmotic pressure?

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 : The difference in the boiling points of equimolar solution of HCI and HF decreases as their

                  molarity is decreased.

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

At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. Concentration at which osmotic pressure of the solution becomes 1.52 bar at the same temperature, would be -

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

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