Concentrated aqueous sulphuric acid is 98% H₂SO₄by mass and has a  density of 1.80 g mL^-1.Volume of acid required to make one litre of 0.1 M H₂SO₄ solution is:

• 11.10 mL

• 16.65 mL

• 22.20 mL

• 22.20 mL

0.5 Molal aqueous solution of aweak acid (HX) is 20% ionised. If K_f for water is1.86 K kg mol^-1, the lowering in freezing point of the solution is:

• -1.12 K 

• 0.56 K 

• 1.12 K 

• 1.12 K 

A solution containing 10 g per dm³ is urea (molecular mass = 60 g mol^-1) is isotonic with a molecular mass of this non-volatile solute. The molecular mass of this of this non-volatile solute is:

• 250 g mol^-1

• 300 g mol^-1

• 350 g mol^-1

• 350 g mol^-1

1.00 g of a non- electrolyte solute (molar mass 250 g mol^-1) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K Kg mol^-1, the freezing point of benzene will be lowered  by:

• 0.4 K

• 0.3 K

• 0.5 K

• 0.5 K

A solution of acetone in ethanol:

• shows a negative deviation from Raoult's law

• shows a positive deviation from Raoult's law

• behave likea near ideal solution

• behave likea near ideal solution

During osmosis, flow of water through a semi-permeable membrane is: 

• from a solution having higher concentration only

• from both sides of a semi-permeable membrane with equal flow rates

• from both sides of a semi-permeable membrane with unequal flow rates

• from both sides of a semi-permeable membrane with unequal flow rates

If molality of the dilute solution is doubled, the value of molal depression constant (K_f) will be

• Doubled

• Halved

• Tripled

• Tripled

Which of the following is dependent on temperature?

• Molality

• Molarity

• Mole fraction

• Mole fraction

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :

$$\begin{gathered} a) 60 mL \frac{M}{10} HCl + 40 mL \frac{M}{10} NaOH \\ b) 55 mL \frac{M}{10}HCl + 45 mL \frac{M}{10} NaOH \\ c) 75 mL \frac{M}{5} HCl + 25 mL \frac{M}{5} NaOH \\ d)\hspace{0.17em}100 mL \frac{M}{10} HCl + 100 mL\frac{M}{10} NaOH \end{gathered}$$

pH of which one of them will be equal to 1?

• b

• a

• c

• d

The solubility of BaSO₄ in water is 2.42 × 10^–3 gL^–1 at 298 K. The value of its solubility product (K_sp) will be
(Given the molar mass of BaSO₄ = 233 g mol^–1)

• 1.08 x 10^-10 mol²L^-2

• 1.08 x 10^-12 mol²L^-2

• 1.08 x 10^-8 mol²L^-2

• 1.08 x 10^-14 mol²L^-2