# Solution Test 3

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:The amount of anhydrous $$N{a_2}C{O_3}$$ present in 250 ml of 0.25 M solution is

6.225 g

66.25 g

6.0 g

6.625 g

## Questions 2 of 50

Question:Dilute one litre 1 molar $${H_2}S{O_4}$$ solution by 5 litre water, the normality of that solution is

$$0.2N$$

$$5\,N$$

$$10\,N$$

0.33 N

## Questions 3 of 50

Question:When a solute is present in trace quantities the following expression is used

Gram per million

Milligram percent

Microgram percent

Nano gram percent

Parts per million

## Questions 4 of 50

Question:When the concentration is expressed as the number of moles of a solute per litre of solution it known as

Normality

Molarity

Mole fraction

Mass percentage

Molality

## Questions 5 of 50

Question:What will be the normality of a solution containing 4.9 g. $${H_3}P{O_4}$$ dissolved in 500 ml water

0.3

1

3

0.1

## Questions 6 of 50

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

3.0504

3.64

3.05

2.9732

## Questions 7 of 50

Question:Conc. $${H_2}S{O_4}$$ has a density of 1.98 gm/ml and is 98% $${H_2}S{O_4}$$ by weight. Its normality is

2 N

19.8 N

39.6 N

98 N

## Questions 8 of 50

Question:The mole fraction of the solute in one molal aqueous solution is

0.027

0.036

0.018

0.009

## Questions 9 of 50

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

Molarity

Molality

Mole fraction

Weight fraction

## Questions 10 of 50

Question:The distribution law is applied for the distribution of basic acid between

Water and ethyl alcohol

Water and amyl alcohol

Water and sulphuric acid

Water and liquor ammonia

## Questions 11 of 50

Question:Volume of water needed to mix with 10 ml 10N $$HN{O_3}$$ to get 0.1 N $$HN{O_3}$$

1000 ml

990 ml

1010 ml

10 ml

## Questions 12 of 50

Question:The sum of the mole fraction of the components of a solution is

0

1

2

4

## Questions 13 of 50

Question:$$NaClO$$ solution reacts with $${H_2}S{O_3}$$ as, $$NaClO + {H_2}S{O_3} \to NaCl + {H_2}S{O_4}$$ . A solution of $$NaClO$$ used in the above reaction contained 15g of $$NaClO$$ per litre. The normality of the solution would be

0.8

0.6

0.2

0.33

## Questions 14 of 50

Question:A solution contains $$1.2046 \times {10^{24}}$$ hydrochloric acid molecules in one $$d{m^3}$$ of the solution. The strength of the solution is

6 N

2 N

4 N

8 N

## Questions 15 of 50

Question:The normality of 10 lit. volume hydrogen peroxide is

0.176

3.52

1.78

0.88

17.8

## Questions 16 of 50

Question:Essential quantity of ammonium sulphate taken for preparation of 1 molar solution in 2 litres is

$$132\,gm$$

$$264\,gm$$

$$198\,gm$$

$$212\,gm$$

## Questions 17 of 50

Question:The formula weight of $${H_2}S{O_4}$$ is 98. The weight of the acid in $$400ml$$ of $$0.1M$$ solution is

$$2.45\,g$$

$$3.92\,g$$

$$4.90\,g$$

$$9.8\,g$$

## Questions 18 of 50

Question:The molarity of pure water is

55.6

5.56

100

18

## Questions 19 of 50

Question:Equimolar solutions in the same solvent have

Same boiling point but different freezing point

Same freezing point but different boiling point

Same boiling and same freezing points

Different boiling and different freezing points

## Questions 20 of 50

Question:Which of the following is a colligative property

Osmotic pressure

Boiling point

Vapour pressure

Freezing point

## Questions 21 of 50

Question:When a substance is dissolved in a solvent the vapour pressure of the solvent is decreased. This results in

An increase in the b.p. of the solution

A decrease in the b.p. of the solvent

The solution having a higher freezing point than the solvent

The solution having a lower osmotic pressure than the solvent

## Questions 22 of 50

Question:If $${P^o}$$ and $$P$$ are the vapour pressure of a solvent and its solution respectively and $${N_1}$$ and $${N_2}$$ are the mole fractions of the solvent and solute respectively, then correct relation is

$$P = {P^o}{N_1}$$

$$P = {P^o}{N_2}$$

$${P^o} = P\,{N_2}$$

$$P = {P^o}\,({N_1}/{N_2})$$

## Questions 23 of 50

Question:Which one of the statements given below concerning properties of solutions, describes a colligative effect

Boiling point of pure water decreases by the addition of ethanol

Vapour pressure of pure water decreases by the addition of nitric acid

Vapour pressure of pure benzene decreases by the addition of naphthalene

Boiling point of pure benzene increases by the addition of toluene

## Questions 24 of 50

Question:The atmospheric pressure is sum of the

Pressure of the biomolecules

Vapour pressure of atmospheric constituents

Vapour pressure of chemicals and vapour pressure of volatiles

Pressure created on to atmospheric molecules

## Questions 25 of 50

Question:The vapour pressure of a solvent decreased by $$10mm$$ 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 the mole fraction of the solvent, if decrease in the vapour pressure is to be $$20\,mm$$ of mercury

0.8

0.6

0.4

0.2

## Questions 26 of 50

Question:For a dilute solution, Raoult's law states that

The lowering of vapour pressure is equal to mole fraction of solute

The relative lowering of vapour pressure is equal to mole fraction of solute

The relative lowering of vapour pressure is proportional to the amount of solute in solution

The vapour pressure of the solution is equal to the mole fraction of solvent

## Questions 27 of 50

Question:In which case Raoult's law is not applicable

$$1M\,NaCl$$

1 M urea

1 M glucose

1 M sucrose

## Questions 28 of 50

Question:A solution that obeys Raoult's law is

Normal

Molar

Ideal

Saturated

## Questions 29 of 50

Question:A mixture of benzene and toluene forms

An ideal solution

Non-ideal solution

Suspension

Emulsion

## Questions 30 of 50

Question:Which of the following is an ideal solution

Water + ethanol

Chloroform + carbon tetrachloride

Benzene + toluene

Water + hydrochloric acid

## Questions 31 of 50

Question:In osmosis

Solvent molecules move from higher concentration to lower concentration

Solvent molecules move from lower to higher concentration

Solute molecules move from higher to lower concentration

Solute molecules move from lower to higher concentration

## Questions 32 of 50

Question:Semipermeable membrane is that which permits the passage of

Solute molecules only

Solvent molecules only

Solute and solvent molecules both

Neither solute nor solvent molecules

## Questions 33 of 50

Question:The osmotic pressure of a solution is directly proportional to

The molecular concentration of solute

The absolute temperature at a given concentration

The lowering of vapour pressure

All of the above

## Questions 34 of 50

Question:What would happen if a thin slice of sugar beet is placed in a concentrated solution of $$NaCl$$

Sugar beet will lose water from its cells

Sugar beet will absorb water from solution

Sugar beet will neither absorb nor lose water

Sugar beet will dissolve in solution

## Questions 35 of 50

Question:The osmotic pressure of a decinormal solution of $$BaC{l_2}$$ in water is

Inversely proportional to its celsius temperature

Inversely proportional to its absolute temperature

Directly proportional to its celsius temperature

Directly proportional to its absolute temperature

## Questions 36 of 50

Question:Blood cells will remain as such in

Hypertonic solution

Hypotonic solution

Isotonic solution

None of these

## Questions 37 of 50

Question:In osmosis reaction, the volume of solution

Decreases slowly

Increases slowly

Suddenly increases

No change

## Questions 38 of 50

Question:As a result of osmosis the volume of solution

Increases

Decreases

Remains constant

Increases or decreases

## Questions 39 of 50

Question:The molal elevation constant is the ratio of the elevation in B.P. to

Molarity

Molality

Mole fraction of solute

Mole fraction of solvent

## Questions 40 of 50

Question:The molal boiling point constant for water is $${0.513^o}C\,kg\,mo{l^{ - 1}}$$. When 0.1 mole of sugar is dissolved in $$200ml$$ of water, the solution boils under a pressure of one atmosphere at

$${100.513^o}C$$

$${100.0513^o}C$$

$${100.256^o}C$$

$${101.025^o}C$$

## Questions 41 of 50

Question:Which one of the following statements is FALSE

The correct order of osmotic pressure for 0.01 M aqueous solution of each compound is $$BaC{l_2} > KCl > C{H_3}COOH >$$ sucrose.

The osmotic pressure $$(\pi )$$ of a solution is given by the equation $$\pi = MRT$$ where M is the molarity of the solution.

Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction.

Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression.

## Questions 42 of 50

Question:Solute when dissolved in water

Increases the vapour pressure of water

Decreases the boiling point of water

Decreases the freezing point of water

All of the above

## Questions 43 of 50

Question:1.00 gm of a non-electrolyte solute dissolved in 50 gm of benzene lowered the freezing point of benzene by 0.40 K. $${K_f}$$ for benzene is 5.12 kg mol$$^{ - 1}$$. Molecular mass of the solute will be

$$256\,g\,mo{l^{ - 1}}$$

$$2.56\,g\,mo{l^{ - 1}}$$

$$512 \times {10^3}\,g\,mo{l^{ - 1}}$$

$$2.56 \times {10^4}\,g\,mo{l^{ - 1}}$$

## Questions 44 of 50

Question:0.440 g of a substance dissolved in 22.2 g of benzene lowered the freezing point of benzene by $${0.567^o}C$$. The molecular mass of the substance $$({K_f} = {5.12^o}C\,mo{l^{ - 1}})$$

178.9

177.8

176.7

175.6

## Questions 45 of 50

Question:The osmotic pressure of which solution is maximum (consider that deci-molar solution of each 90% dissociated)

Aluminium sulphate

Barium chloride

Sodium sulphate

A mixture of equal volumes of 1 and 3

## Questions 46 of 50

Question:At $${25^o}C$$, the highest osmotic pressure is exhibited by $$0.1M$$ solution of

$$CaC{l_2}$$

$$KCl$$

Glucose

Urea

## Questions 47 of 50

Question:Which of the following has the lowest freezing point

0.1 m sucrose

0.1 m urea

0.1 m ethanol

0.1 m glucose

## Questions 48 of 50

Question:Which of the following has minimum freezing point

$$0.1M$$$${K_2}C{r_2}{O_7}$$

0.1 M $$N{H_4}Cl$$

0.1 M $$BaS{O_4}$$

0.1 M $$A{l_2}{(S{O_4})_3}$$

## Questions 49 of 50

Question:One mole of a solute $$A$$ is dissolved in a given volume of a solvent. The association of the solute take place according to $$nA$$?$${(A)_n}$$. The Van't Hoff factor $$i$$is expressed as

$$i = 1 - x$$

$$i = 1 + \frac{x}{n}$$

$$i = \frac{{1 - x + \frac{x}{n}}}{1}$$

$$i = 1$$

## Questions 50 of 50

Question:Acetic acid dissolved in benzene shows a molecular weight of