BOARD MOST IMPORTANT QUESTION

The density of a solution containing 13% by mass of sulphuric acid is 1.09 g/ml. Calculate the molarity and normality of the solution-

(A) 1.445 M (B) 14.45 M

Calculate the molarity of pure water (d = 1 g/L)

(A) 555 M (B) 5.55 M

Calculate the quantity of sodium carbonate (anhydrous) required to prepare 250 ml solution.

(A) 2.65 gram (B) 4.95 gram

20 ml of 0.02 M KMnO₄ was required to completely oxides 10 ml of oxalic acid solution. What is the molarity of the oxalic acid solution ?

(A) 0.1 M (B) 0.4 M

Find the molarity of H₂SO₄ solution whose specific gravity is 1.98 g ml^-1 and 95% by volume H₂SO₄.

(A) 7.412 (B) 8.412

Calculate molarity of 1 litre solution of 93% H₂SO₄ by volume. The density of solution is 1.84 gm ml^-1

(A) 0.0025 M, 0.025 N (B) 0.025 M, 0.025 N

Calculate the molarity and normality of a solution contain 0.5 gm of NaOH dissolved in 500 ml solution.

(A) 0.2 m, 0.00357 (B) 0.4 m, 0.00357

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

(A) 0.50, 0.3, 0.19 (B) 0.19, 0.3, 0.50

15 gm of methyl alcohol is dissolved in 35 gram of water. What is the mass percentage of methyl alcohol in solution ?

(A) 30 % (B) 50 %

Calculate normality of the mixture obtained by mixing 100 ml of 0.1 N HCl and 50 ml of 0.25 N NaOH solution.

(A) 0.0467 N (B) 0.0367 N

Calculate the vapour pressure of a solution at 100^oC containing 3g of cane sugar in 33g of water. (At. wt. C= 12, H=1, O= 16)

(A) 760 mm (B) 756.90 mm

Osmotic pressure of a sugar solution at 24^oC is 2.5 atmospheres. Determine the concentration of the solution in gm mole per litre.

(A) 0.0821 moles/ litre (B) 1.082 moles/litre

0.15 g of a substance dissolved in 15g of solvent boiled at a temperature higher by 0.216^oC than that of the pure solvent. Calculate the molecular weight of the substance. Molal elevation constant for the solvent is 2.16^oC.

(A) 216 (B) 100

A solution of 0.450 gm of urea (mol. wt 60) in 22.5 g of water showed 0.170^oC of elevation in boiling point. Calculate the molal elevation constant of water.

(A) 0.17^oC (B) 0.45 ^oC

Calculate the boiling point of a solution containing 0.45g of camphor (mol. wt. 152) dissolved in 35.4g of acetone (b.p. 56.3^oC); K_b per 100 gm of acetone is 17.2^oC.

(A) 56.446 ^oC (B) 52.401^oC

The molarity of a glucose solution containing 36g of glucose per 400 ml. of the solution is –

(A) 1.0 (B) 0.5 (C) 2.0 (D) 0.05

Molarity of a solution relates the –

(A) Moles of solute and solvent

(B) Moles of solute and mass of solution

(D) Volume of solution and moles of solute

The units of mole fraction of a compound in solution are –

(A) mol kg^-1 (B) mol litre^-1

The hardness of water is usually expressed in –

(A) ppm (B) g/litre (C) Mol/litre (D) None

Density of water is 1 g/ml. The concentration of water in mol/litre is –

(A) 1000 (B) 18 (C) 0.01 (D) 55.5

How many gram of NaOH will be needed to prepare 250 mL of 0.1 M solution –

(A) 1 g (B) 10 g (C) 4 g (D) 6 g

How many grams of glucose should be dissolved to make one litre solution of 10% (w/v) glucose –

(A) 10 g (B) 180 g (C) 100 g (D) 1.8 g

2.3 g of C2H5OH (mol. wt. 46) are dissolved in water to form 500 mL solution. The molarity of the solution is –

(A) 0.01 (B) 0.1 (C) 0.05 (D) 2.0

The number of moles present in 2 litre of 0.5 M NaOH is –

(A) 2 (B) 1 (C) 0.1 (D) 0.5

3.0 molal NaOH solution has a density of 1.110 g/ml. The molarity of the solution is –

(A) 2.9732 (B) 3.05 (C) 3.64 (D) 3.0504

A solution contains one mole of alcohol and four moles of water. What are the mole fractions of water and alcohol –

(A) 1/4, 4/1 (B) 4/1, 1/4 (C) 4/5, 1/5 (D) 1/5, 4/5

In the aqueous solution of sulphuric acid the mole fraction of water is 0.85. The molarity of the solution is –

(A) 8.9 m (B) 0.19 m (C) 9.8 m (D) 15 m

The amound of H2SO4 present in 400 mL of 0.1 M solution of the acid is –

(A) 2.45 g (B) 3.92 g (C) 9.80 g (D) 4.9 g

10 gram of glucose are dissolved in 150 gram of water. the mass % of glucose is –

(A) 5 % (B) 6.25 % (C) 93.75 % (D) 15 %

The vapour pressure of ethanol and methanol are 42.0 mm and 88.5 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 46.0 g of ethanol with 16.0 g of methanol. The mole fraction of methanol in the vapour is –

(A) 0.467 (B) 0.502 (C) 0.513 (D) 0.556

Vapour pressure of a solvent containing nonvolatile solute is –

(A) More than the vapour pressure of a solvent

(B) Less than the vapour pressure of solvent

(D) None of these

The relative lowering in vapour pressure is –

(A) (B) (C) (D)

Which of the following is not correct for ideal solution –

(A) Raoult’s law is obeyed for entire concentration range and temperatures

(B) (C) (D)

Which of the following conditions is not correct for ideal solution –

(A) no change in volume of mixing

(B) no change in enthalpy on mixing

(D) lionization of solute should occurs to a small extent.

When one mole of non-volatile solute is dissolved in three moles of solvent, the vapour pressure of the solution relative to the vapour pressure of the pure solvent is–

(A) 1/3 (B) 1/4 (C) 3/4 (D) 1

Which of the following is not a colligative property-

(A) (B) (C) T_b (D) K_B

Solute when dissolved in water-

(A) Increases the vapour pressure of water

(B) Decreases the boiling point of water

(D) All of the above

Which statement is corrext ofr the boiling point of solvent containing a dissolved solid substance-

(A) Boiling point of the liquid is depressed

(D) Boiling point of the liquid is elevated

(D) The change depends upon the polarity of the liquid

The molal elevation/deprcession constant depends upon-

(A) Nature of solvent (B) Boiling point

An example of colligative property is-

(A) Freezing point (B) Boiling point

The passing of solvent particles through semi permeable membrane is called-

(A) Osmosis (B) Electro dialysis

If mole fraction of the solvent in a solution decreases then-

(A) Vapour pressure of solution increases

(B) b.pt decreases

(D) All are correct

Two solutions have different osmotic pressures. The solution of higher osmotic pressure is called-

(A) Isotonic solution (B) Hypotonic solution

According to Byle-Vant Hoff law for solutions the osmotic pressure of a dilute solution is-

(A) Inversely proportional to its volume

(B) Directly proportional to its volume

(D) None of the above

Which solution will show maximum elevation in b.pt-

(A) 0.1 M KCl (B) 0.1 N Cacl₂

Which of the following 0.1 m aqueous solution ill have the lowest freezing point.

(A) Potassium sulphate (B) Sodium chloride

The correct relationship between the boiling points of very dilute solutions of AICL₃ (t₁) and CaCl₂ (t₂) having the same molar concentration is-

(A) t₁= t₂ (B) t₁>t₂ (C) t₂>t₁ (D) t₂ t₁

0.5 M solution of urea is isotonic with

(A) 0.5 M NaCl solution (B) 0.5 M sugar solution

Which aqueous solution has minimum freezing

(A) 0.01 M NaCl (B) 0.005 M C₂H₅OH

Vant Hoff factor (i)-

(A) Is less than one in case of dissociation

(B) Is more than one in case of association

Which one of the following pairs of solution can we expect to be isotonic at the same temperature-

(A) 0.1 M urea and 0.1 M NaCl

(B) 0.1 M urea and 0.2 M MgCl₂

(D) 0.1 M Ca(NO₃)₂ and 0.1 M Na₂SO₄

25 mL of M HCL were added to to 75 mL of 0.305 M HCL. The molarity of HCL in the resulting solution is approximately-

(A) 0.055 M (B) 0.35 M (C) .787 M (D) 3.05 M

Molaity of the solution is –

(A) The number of moles of the solute dissolved per kilogram of solvent

(B) The number of gram mole of the solute dissolved per ml of the solution

(D) The number of moles iof the solute dissolved per litre of the solution

When mango is placed in dilute aqueous solution of hydrochloride acid, it-

(A) Shrinks (B) Swells

The osmotic pressure of a solution is given by the relation-

(A) π=RT/C (B) π=CT/R

(C)π=RC/T (D) π/C = RT

blood cells retain their normal shapes in solutions which are-

(A) isotonic to blood (B) hypotonic to blood

The osmotic pressure of a dilute solution is given by-

(A) P= P₀X (B) V = nRT

The solution having same osmotic pressure at constant (given) temperature are called-

(A) Equivalent solutions (B) Ideal solutions

A property which depends primarily on the number of molecules of a system and lnot on their nature is known to be-

(A) Constitutive (B) Additive

Which of the following concentration factor is affected by change in temperature?

(A) Molarity (B) Molality

For an aqueous solution, freezing point is 0.186. Boiling point of the same solution is (K_f =1.86⁰K mol^-1 kg) and

k_b = 0.512⁰K mol^-1 gk)

186⁰ (B) 100.0512⁰(C) 1.86⁰ (D) 5.12⁰

`In a mixture of A and B, components show negative deviation when-

(A) A-B interaction is stronger than A –A and B-B interaction

(B) A- B interaction is weaker than A- A and B- B interaction

(D) POSITIVE

If liquids A and B form an ideal solution-

(A) The free energy of mixing is Zero

(B) The free energy as well as the entropy of mixing are each zero

(D) The entropy of mixing is Zero

If liquid A and B form ideal solution than

(A) G_mix =0 (B) H_mixing =0

Which one of the following aqueous solutions will exhibit highest building point?

(A) 0.01 M Na₂SO₄ (B) 0.01 M KNO₃

Which aqueous solution exhibits highest boiling point-

(A) 0.015 M glucose (B) 0.01 M KNO₃

Density of a 2.05 M solution of acetic acid in water is 1.02 g/mL. The molality of the solution is-

(A) 3.28 mol kg^-1 (B) 2.28 mol kg^-1

When mercuric iodide is added to the aqueous solution of potassium iodide, the-

freezing point is raised
freezing point is lowered
freezing point does not change
boiling point does not change

Increasing the temperature of an aqueous solution will cause-

(A) decrease on molality (B) decrease in molarity

The normality of 0.3 M phosphorous acid (H₃PO₃) is-

(A) 0.1 (B) 0.9 (C) 0.3 (D) 0.6

Dissolving 120 g of urea (mol Wt. 60) in 1000 g of water gave a solution of density 1.15 g/ml.

(A) 1.78M (B) 2.00 M (C) 2.05 (D) 2.22M

Concentration of solution and Colligatives properties

BOARD MOST IMPORTANT QUESTION

Leave a Comment Cancel Reply