The molality of a solution containing 1.8g of glucose dissolved in 250 g of water is _____________

(a)

0.2 M

(b)

0.01 M

(c)

0.02 M

(d)

0.04 M

Which one of the following gases has the lowest value of Henry's law constant ?

(a)

N₂

(b)

He

(c)

CO₂

(d)

H₂

According to Raoults law, the relative lowering of vapour pressure for a solution is equal to __________

(a)

mole fraction of solvent

(b)

mole fraction of solute

(c)

number of moles of solute

(d)

number of moles of solvent

The empirical formula of a nonelectrolyte(X) is CH₂O. A solution containing six gram of X exerts the same osmotic pressure as that of 0.025 M glucose solution at the same temperature. The molecular formula of X is ____________

(a)

C₂H₄O₂

(b)

C₈H₁₆O₈

(c)

C₄H₈O₄

(d)

CH₂O

Normality of 1.25M sulphuric acid is ___________

(a)

1.25 N

(b)

3.75 N

(c)

2.5 N

(d)

2.25 N

For a solution, the plot of osmotic pressure (\(\pi\)) verses the concentration (c in mol L^–1) gives a straight line with slope 310R where 'R' is the gas constant. The temperature at which osmotic pressure measured is ____________

(a)

310 x 0.082 K

(b)

310^oC

(c)

37^oC

(d)

\({310\over 0.082}K\)

The correct equation for the degree of an associating solute, 'n' molecules of which undergoes association in solution, is _____________

(a)

\(\alpha=\frac{n(i-1)}{n-1}\)

(b)

\(\alpha^2=\frac{n(1-i)}{(n-1)}\)

(c)

\(\alpha=\frac{n(i-1)}{1-\mathrm{n}}\)

(d)

\(\alpha=\frac{n(1-i)}{n(1-i)}\)

The example of solid solution is __________

(a)

glucose in water

(b)

copper in gold

(c)

camphor in nitrogen

(d)

oxygen in nitrogen

The blocking of capillaires due to sudden release of bubbles of N₂ gas in blood is known as ______

(a)

bends

(b)

blends

(c)

mends

(d)

all of these

The temperature at which the vapour pressure of a liquid equals external pressure is called __________

(a)

freezing point

(b)

boiling point

(c)

melting point

(d)

critical temperature

Vapour pressure is the pressure exerted by vapours ____________

(a)

in equilibrium with liquid

(b)

in any condition

(c)

in an open system

(d)

in atmospheric conditions

The value of ebulllescopic constant depends upon ______________

(a)

\(\triangle\)H_solution

(b)

nature of solvent

(c)

nature of solute

(d)

freezing point of solution

Depression in freezing point for 1 M urea, 1 M NaCI and 1 M CaCI₂ are in the ratio of ____________

(a)

1: 2 : 3

(b)

1: 1 : 1

(c)

3: 2 : 1

(d)

Data insufficient

Which of the following has maximum freezing point?

(a)

Pure H₂0

(b)

0.1 M NaCl (aq)

(c)

0.01 M NaCl (aq)

(d)

0.5 M NaCl (aq)

What is the boillng point of 1 molal aqueous solution of NaCI [K_b = 0.52 K molal^-I].

(a)

99.48°C

(b)

98.96°C

(c)

100.52°C

(d)

101.04°C

The normality of 10% weight/volume) acetic and is ____________

(a)

1 N

(b)

10 N

(c)

1.7 N

(d)

0.83 N

If solute and solvent interactions are more than solute - solute and solvent - solvent interactions then ___________

(a)

It is ideal solution

(b)

It is non-ideal solution with positive deviation

(c)

It is non-ideal solution with negative deviation

(d)

Can't be predicted

Which of the following statment is true?

(a)

Molarity of solution is idependent of temperature

(b)

Molality of solution is independent of temperature

(c)

Mole fraction of solute is dependent on temperature

(d)

The unit of molality is mol dm^-3

An azeotropic solution of two liquids has a boiling point lower than either of the boiling points of the two liquids when it __________

(a)

shows negative deviation

(b)

shows positive deviation

(c)

shows no deviation

(d)

is unsaturated

Equimolar solution of non-electrolyte in the same solvent have ____________

(a)

same boiling point and same freezing point

(b)

different boiling point. and different freezing point

(c)

same boiling point but different freezing point

(d)

same freezing point but different boiling point