# Solution Test 7

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:The solubility of a gas in water depends on

Nature of the gas

Temperature

Pressure of the gas

All of the above

## Questions 2 of 50

Question:Which of the following is not correct for $${D_2}O$$

Boiling point is higher than $${H_2}O$$

$${D_2}O$$ reacts slowly than $${H_2}O$$

Viscosity is higher than $${H_2}O$$ at $${25^o}$$

Solubility of NaCl in it is more than $${H_2}O$$

## Questions 3 of 50

Question:Molarity is expressed as

Gram/litre

Moles/litre

Litre/mole

Moles/1000 gms

## Questions 4 of 50

Question:$$20\,ml$$ of $$HCl$$ solution requires $$19.85\,ml$$ of $$0.01\,M\,NaOH$$ solution for complete neutralization. The molarity of $$HCl$$ solution is

0.0099

0.099

0.99

9.9

## Questions 5 of 50

Question:5 ml of N HCl, 20 ml of N/2 $${H_2}S{O_4}$$ and 30 ml of N/3 HNO3 are mixed together and volume made to one litre. The normally of the resulting solution is

$$\frac{N}{5}$$

$$\frac{N}{{10}}$$

$$\frac{N}{{20}}$$

$$\frac{N}{{40}}$$

$$\frac{N}{{25}}$$

## Questions 6 of 50

Question:The amount of $${K_2}C{r_2}{O_7}$$ (eq. wt. 49.04) required to prepare 100 ml of its 0.05 N solution is

2.9424 g

0.4904 g

1.4712 g

0.2452 g

## Questions 7 of 50

Question:The normal amount of glucose in $$100ml$$ of blood (8-12 hours after a meal) is

$$8\,mg$$

$$80\,mg$$

$$200\,mg$$

$$800\,mg$$

## Questions 8 of 50

Question:Molar solution means 1 mole of solute present in

1000g of solvent

1 litre of solvent

1 litre of solution

1000g of solution

## Questions 9 of 50

Question:Normality $$(N)$$ of a solution is equal to

$$\frac{{{\rm{No}}{\rm{. of moles of solute}}}}{{{\rm{Volume of solution in litre}}}}$$

$$\frac{{{\rm{No}}{\rm{. of gram equivalent of solute}}}}{{{\rm{Volume of solution in litre }}}}$$

$$\frac{{{\rm{No}}{\rm{. of moles of solute}}}}{{{\rm{Mass of solvent in kg}}}}$$

None of these

## Questions 10 of 50

Question:The volume strength of $$1.5\,N\,{H_2}{O_2}$$ solution is

4.8

5.2

8.8

8.4

## Questions 11 of 50

Question:0.5 M of $${H_2}S{O_4}$$ is diluted from 1 litre to 10 litre, normality of resulting solution is

1 N

0.1 N

10 N

11 N

## Questions 12 of 50

Question:If one mole of a substance is present in $$1\,kg$$ of solvent, then

It shows molar concentration

It shows molal concentration

It shows normality

It shows strength $$gm/gm$$

## Questions 13 of 50

Question:$$6.02 \times {10^{20}}$$ molecules of urea are present in 100 ml of its solution. The concentration of urea solution is (Avogadro constant, $${N_A} = 6.02 \times {10^{23}}mo{l^{ - 1}})$$

0.02 M

0.01 M

0.001 M

0.1 M

## Questions 14 of 50

Question:The number of moles of $$S{O_2}C{l_2}$$ in $$13.5gm$$ is

0.1

0.2

0.3

0.4

## Questions 15 of 50

Question:Normality of $$2M$$ sulphuric acid is

$$2N$$

$$4N$$

$$N/2$$

$$N/4$$

## Questions 16 of 50

Question:Molar concentration $$(M)$$ of any solution =

$$\frac{{{\rm{No}}{\rm{. of moles of solute}}}}{{{\rm{Volume of solution in litre}}}}$$

$$\frac{{{\rm{No}}{\rm{. of gram equivalent of solute}}}}{{{\rm{Volume of solution in litre}}}}$$

$$\frac{{{\rm{No}}{\rm{. of moles of solute}}}}{{{\rm{Mass of solvent in kg}}}}$$

$$\frac{{{\rm{No}}{\rm{. of moles of any constituent}}}}{{{\rm{Total no}}{\rm{. of moles of all constituents}}}}$$

## Questions 17 of 50

Question:Molecular weight of urea is 60. A solution of urea containing $$6g$$ urea in one litre is

1 molar

1.5 molar

0.1 molar

0.01 molar

## Questions 18 of 50

Question:The molar solution of sulphuric acid is equal to

$$N$$solution

$$2N$$solution

$$N/2$$ solution

$$3N$$solution

## Questions 19 of 50

Question:When 90 gm of water is mixed with 300 gm of acetic acid. The total number of moles will be

5

10

15

20

## Questions 20 of 50

Question:A molal solution is one that contains one mole of a solute in

1000 gm of the solvent

One litre of the solvent

One litre of the solution

22.4 litres of the solution

## Questions 21 of 50

Question:Colligative properties are used for the determination of

Molar Mass

Equivalent weight

Arrangement of molecules

Melting point and boiling point

Both 1 and 2

## Questions 22 of 50

Question:What does not change on changing temperature

Mole fraction

Normality

Molality

None of these

1 and 3 are correct

## Questions 23 of 50

Question:A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressure of the pure hydrocarbons at 20$$^\circ$$C are 440 mmHg for pentane and 120 mmHg for hexane. The mole fraction of pentane in the vapour phase would be

0.549

0.2

0.786

0.478

## Questions 24 of 50

Question:Benzene and toluene form nearly ideal solutions. At 20$$^\circ$$C, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The parial vapour pressure of benzene at 20$$^\circ$$C for a solution containing 78g of benzene and 46g of toluene in torr is

50

25

37.5

53.5

## Questions 25 of 50

Question:The vapour pressure of benzene at a certain temperature is $$640\,mm$$ of $$Hg$$. A non-volatile and non-electrolyte solid weighing $$2.175g$$ is added to $$39.08g$$ of benzene. The vapour pressure of the solution is $$600mm$$ of $$Hg$$. What is the molecular weight of solid substance

49.5

59.6

69.5

79.8

## Questions 26 of 50

Question:Which one of the following is the expression of Raoult's law $$p =$$vapour pressure of pure solvent $${p_s} =$$vapour pressure of the solution $$n =$$number of moles of the solute $$N =$$number of moles of the solvent

$$\frac{{p - {p_s}}}{p} = \frac{n}{{n + N}}$$

$$\frac{{{p_s} - p}}{p} = \frac{N}{{N + n}}$$

$$\frac{{p - {p_s}}}{{{p_s}}} = \frac{N}{{N - n}}$$

$$\frac{{{p_s} - p}}{{{p_s}}} = \frac{{N - n}}{N}$$

## Questions 27 of 50

Question:A non ideal solution was prepared by mixing 30 ml chloroform and 50 ml acetone. The volume of mixture will be

> 80 ml

< 80 ml

= 80 ml

$$\ge \lambda \mu 08$$

## Questions 28 of 50

Question:Which pair from the following will not form an ideal solution

$$CC{l_4} + SiC{l_4}$$

$${H_2}O + {C_4}{H_9}OH$$

$${C_2}{H_5}Br + {C_2}{H_5}I$$

$${C_6}{H_{14}} + {C_7}{H_{16}}$$

## Questions 29 of 50

Question:Which of the following is true when components forming an ideal solution are mixed

$$\Delta {H_m} = \Delta {V_m} = 0$$

$$\Delta {H_m} > \Delta {V_m}$$

$$\Delta {H_m} < \Delta {V_m}$$

$$\Delta {H_m} = \Delta {V_m} = 1$$

## Questions 30 of 50

Question:The liquid pair benzene-toluene shows

Irregular deviation from Raoult's law

Negative deviation from Raoult's law

Positive deviation from Raoult's law

Practically no deviation from Raoult's law

## Questions 31 of 50

Question:A mixture of two completely miscible non-ideal liquids which distil as such without change in its composition at a constant temperature as though it were a pure liquid. This mixture is known as

Binary liquid mixture

Azeotropic mixture

Eutectic mixture

Ideal mixture

## Questions 32 of 50

Question:If 3 gm of glucose (mol. wt. 180) is dissolved in 60 gm of water at $${15^o}C$$. Then the osmotic pressure of this solution will be

0.34 atm

0.65 atm

6.57 atm

5.57 atm

## Questions 33 of 50

Question:If 20 g of a solute was dissolved in 500 ml of water and osmotic pressure of the solution was found to be 600 mm of Hg at $${15^o}C,$$ then molecular weight of the solute is

1000

1200

1400

1800

## Questions 34 of 50

Question:The osmotic pressure of 0.4% urea solution is 1.66 atm and. that of a solution of suger of 3.42 % is 2.46 atm. When both the solution are mixed then the osmotic pressure of the resultant solution will be

1.64 atm

2.46 atm

2.06 atm

0.82 atm

## Questions 35 of 50

Question:The value of osmotic pressure of a 0.2 M aqueous solution at 293K is

8.4 atm

0.48atm

4.8 atm

4.0 atm

## Questions 36 of 50

Question:Diffusion of solvent through a semi permeable membrane is called

Diffusion

Osmosis

Active absorption

Plasmolysis

## Questions 37 of 50

Question:If a $$0.1M$$ solution of glucose (mol. wt. 180) and $$0.1\,{\rm{molar}}$$ solution of urea (mol. wt. 60) are placed on the two sides of a semipermeable membrane to equal heights, then it will be correct to say

There will be no net movement across the membrane

Glucose will flow across the membrane into urea solution

Urea will flow across the membrane into glucose solution

Water will flow from urea solution into glucose solution

## Questions 38 of 50

Question:At constant temperature, the osmotic pressure of a solution

Directly proportional to the concentration

Inversely proportional to the concentration

Directly proportional to the square of the concentration

Directly proportional to the square root of the concentration

## Questions 39 of 50

Question:The rise in the boiling point of a solution containing 1.8 gram of glucose in $$100g$$ of a solvent in $${0.1^o}C$$. The molal elevation constant of the liquid is

0.01 $$K/m$$

$$0.1\,K/m$$

$$1\,K/m$$

$$10\,K/m$$

## Questions 40 of 50

Question:If $$0.15\,g$$ of a solute dissolved in $$15\,g$$ of solvent is boiled at a temperature higher by $${0.216^o}C$$ than that of the pure solvent. The molecular weight of the substance (molal elevation constant for the solvent is $${2.16^o}C$$) is

1.01

10

10.1

100

## Questions 41 of 50

Question:During the evaporation of liquid

The temperature of the liquid will rise

The temperature of the liquid will fall

May rise or fall depending on the nature

The temperature remains unaffected

## Questions 42 of 50

Question:At higher altitudes the boiling point of water lowers because

Atmospheric pressure is low

Temperature is low

Atmospheric pressure is high

None of these

## Questions 43 of 50

Question:An aqueous solution of a non-electrolyte boils at $${100.52^o}C$$. The freezing point of the solution will be

$${0^o}C$$

$$- {1.86^o}C$$

$${1.86^o}C$$

None of the above

## Questions 44 of 50

Question:The freezing point of one molal $$NaCl$$ solution assuming $$NaCl$$ to be 100% dissociated in water is (molal depression constant = 1.86)

$$- {1.86^o}C$$

$$- {3.72^o}C$$

$$+ {1.86^o}C$$

$$+ {3.72^o}C$$

## Questions 45 of 50

Question:If O.P. of 1 M of the following in water can be measured, which one will show the maximum O.P.

$$AgN{O_3}$$

$$MgC{l_2}$$

$${(N{H_4})_3}P{O_4}$$

$$N{a_2}S{O_4}$$

## Questions 46 of 50

Question:Which of the following solution in water possesses the lowest vapour pressure

$$0.1\,(M)\,NaCl$$

$$0.1\,(N)\,BaC{l_2}$$

$$0.1\,(M)\,KCl$$

None of these

## Questions 47 of 50

Question:Which one has the highest boiling point

$$0.1N\,N{a_2}S{O_4}$$

$$0.1N\,MgS{O_4}$$

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

$$0.1M\,BaS{O_4}$$

## Questions 48 of 50

Question:Which of the following solutions boils at the highest temperature

0.1 M glucose

0.1 M NaCl

0.1 M $$BaC{l_2}$$

0.1 M Urea

## Questions 49 of 50

Question:The ratio of the value of any colligative property for $$KCl$$ solution to that for sugar solution is nearly

1

0.5

2

3

## Questions 50 of 50

Question:Van't Hoff factor of $$Ca{(N{O_3})_2}$$ is