# Solution Test 4

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:If 5.85 gms of $$NaCl$$ are dissolved in 90 gms of water, the mole fraction of $$NaCl$$is

0.1

0.2

0.3

0.01

0.0196

## Questions 2 of 50

Question:The molarity of 0.006 mole of $$NaCl$$ in $$100ml$$ solution is

0.6

0.06

0.006

0.066

None of these

## Questions 3 of 50

Question:The normality of 2.3 M $${H_2}S{O_4}$$ solution is

2.3 N

4.6 N

0.46 N

0.23 N

## Questions 4 of 50

Question:The molarity of a solution made by mixing 50ml of conc. $${H_2}S{O_4}$$ (36N) with 50 ml of water is

36 M

18 M

9 M

6 M

## Questions 5 of 50

Question:Which of the following modes of expressing concentration is independent of temperature

Molarity

Molality

Formality

Normality

## Questions 6 of 50

Question:The molality of a solution is

Number of moles of solute per $$1000\,ml$$ of the solvent

Number of moles of solute per $$1000\,gm$$of the solvent

Number of moles of solute per $$1000\,ml$$ of the solution

Number of gram equivalents of solute per $$1000\,ml$$ of the solution

## Questions 7 of 50

Question:With 63 gm of oxalic acid how many litres of $$\frac{N}{{10}}$$ solution can be prepared

100 litre

10 litre

1 litre

1000 litre

## Questions 8 of 50

Question:Molarity of $$0.2N\,{H_2}S{O_4}$$ is

0.2

0.4

0.6

0.1

## Questions 9 of 50

Question:Which is heaviest

25 gm of mercury

2 moles of water

2 moles of carbon dioxide

4 gm atoms of oxygen

## Questions 10 of 50

Question:The molarity of a solution of $$N{a_2}C{O_3}$$ having $$10.6g/500ml$$ of solution is

$$0.2M$$

$$2M$$

$$20M$$

$$0.02M$$

## Questions 11 of 50

Question:Increasing the temperature of an aqueous solution will cause

Decrease in molality

Decrease in molarity

Decrease in mole fraction

Decrease in % w/w

## Questions 12 of 50

Question:1000 gms aqueous solution of $$CaC{O_3}$$ contains 10 gms of carbonate. Concentration of the solution is

10 ppm

100 ppm

1000 ppm

10000 ppm

## Questions 13 of 50

Question:$$10N$$ and $$\frac{1}{{10}}N$$ solution is called

Decinormal and decanormal solution

Normal and decinormal solution

Normal and decanormal solution

Decanormal and decinormal solution

## Questions 14 of 50

Question:When $$7.1gm\,N{a_2}S{O_4}$$ (molecular mass 142) dissolves in $$100\,ml\,{H_2}O$$ , the molarity of the solution is

2.0 M

1.0 M

0.5 M

0.05 M

## Questions 15 of 50

Question:In a mixture of 1 gm $${H_2}$$ and 8 gm $${O_2}$$ , the mole fraction of hydrogen is

0.667

0.5

0.33

None of these

## Questions 16 of 50

Question:A solution of $$CaC{l_2}$$ is $$0.5\,mol/litre$$ , then the moles of chloride ion in $$500ml$$ will be

0.25

0.5

0.75

1

## Questions 17 of 50

Question:The molarity of a $$0.2\,N\,N{a_2}C{O_3}$$ solution will be

0.05 M

0.2 M

0.1 M

0.4 M

## Questions 18 of 50

Question:How many moles of water are present in 180 $$g$$ of water

1 mole

18 mole

10 mole

100 mole

## Questions 19 of 50

Question:The colligative properties of a solution depend on

Nature of solute particles present in it

Nature of solvent used

Number of solute particles present in it

Number of moles of solvent only

## Questions 20 of 50

Question:Which of the following is not a colligative property

Osmotic pressure

Elevation in B.P.

Vapour pressure

Depression in freezing point

## Questions 21 of 50

Question:An aqueous solution of methanol in water has vapour pressure

Equal to that of water

Equal to that of methanol

More than that of water

Less than that of water

## Questions 22 of 50

Question:The pressure under which liquid and vapour can coexist at equilibrium is called the

Limiting vapour pressure

Real vapour pressure

Normal vapour pressure

Saturated vapour pressure

## Questions 23 of 50

Question:The vapour pressure of pure liquid A is 0.80 atm. On mixing a non-volatile B to A, its vapour pressure becomes 0.6 atm. The mole fraction of B in the solution is

0.15

0.25

0.5

0.75

## Questions 24 of 50

Question:Lowering of vapour pressure is highest for

Urea

$$0.1M$$ glucose

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

$$0.1\,M\,BaC{l_2}$$

## Questions 25 of 50

Question:The vapour pressure of a solvent A is 0.80 atm When a non-volatile substance B is added to this solvent its vapour pressure drops to 0.6 atm. What is mole fraction of B in solution

0.25

0.5

0.75

0.9

## Questions 26 of 50

Question:Determination of correct molecular mass from Raoult's law is applicable to

An electrolyte in solution

A non-electrolyte in a dilute solution

A non-electrolyte in a concentrated solution

An electrolyte in a liquid solvent

## Questions 27 of 50

Question:An example of near ideal solution is

$$n$$-heptane and $$n$$-hexane

$$C{H_3}COOH + {C_5}{H_5}N$$

$$CHC{l_3} + {({C_2}{H_5})_2}O$$

$${H_2}O + HN{O_3}$$

## Questions 28 of 50

Question:A mixture of liquid showing positive deviation in Raoult's law is

$${(C{H_3})_2}CO + {C_2}{H_5}OH$$

$${(C{H_3})_2}CO + CHC{l_3}$$

$${({C_2}{H_5})_2}O + CHC{l_3}$$

$${(C{H_3})_2}CO + {C_6}{H_5}N{H_2}$$

## Questions 29 of 50

Question:When ethanol mixes in cyclohexane; cyclohexane reduces the intermolecular forces between ethanol molecule. In this, liquid pair shows

Positive deviation by Raoult's law

Negative deviation by Raoult's law

No deviation by Raoult's law

Decrease in volume

## Questions 30 of 50

Question:Liquids A and B form an ideal solution

The enthalpy of mixing is zero

The entropy of mixing is zero

The free energy of mixing is zero

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

## Questions 31 of 50

Question:Two solutions A and B are separated by semi- permeable membrane. If liquid flows form A to B then

A is less concentrated than B

A is more concentrated than B

Both have same concentration

None of these

## Questions 32 of 50

Question:A 5% solution of canesugar (mol. wt. =342) is isotonic with 1% solution of a substance $$X$$. The molecular weight of $$X$$ is

34.2

171.2

68.4

136.8

## Questions 33 of 50

Question:The osmotic pressure of a dilute solution is given by

$$P = {P_o}x$$

$$\pi V = nRT$$

$$\Delta P = {P_o}{N_2}$$

$$\frac{{\Delta P}}{{{P_o}}} = \frac{{{P_o} - P}}{{{P_o}}}$$

## Questions 34 of 50

Question:Which statement is wrong regarding osmotic pressure (P), volume (V) and temperature (T)

$$P \propto \frac{1}{V}$$ if $$T$$ is constant

$$P \propto T$$ if $$V$$ is constant

$$P \propto V$$ if $$T$$ is constant

$$PV$$is constant if $$T$$ is constant

## Questions 35 of 50

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

Diffusion rate of the solute

Ionic concentration

Elevation of B.P.

Flow of solvent from a concentrated to a dilute solution

## Questions 36 of 50

Question:The osmotic pressure in atmospheres of 10% solution of canesugar at $${69^o}C$$ is

724

824

8.21

7.21

## Questions 37 of 50

Question:A solution of urea contain 8.6 gm/litre (mol. wt. 60.0). It is isotonic with a 5% solution of a non-volatile solute. The molecular weight of the solute will be

348.9

34.89

3489

861.2

## Questions 38 of 50

Question:One mole each of urea, glucose and sodium chloride were dissolved in one litre of water Equal osmotic pressure will be produced by solutions of

Glucose and sodium chloride

Urea and glucose

Sodium chloride and urea

None of these

## Questions 39 of 50

Question:Value of gas constant R is

0.082 litre atm

0.987 cal $$mo{l^{ - 1}}{K^{ - 1}}$$

8.3 J $$mo{l^{ - 1}}{K^{ - 1}}$$

83 erg $$mo{l^{ - 1}}{K^{ - 1}}$$

## Questions 40 of 50

Question:The temperature, at which the vapour pressure of a liquid becomes equal to the atmospheric pressure is known as

Freezing point

Boiling point

Absolute temperature

None of these

## Questions 41 of 50

Question:The freezing point of a solution prepared from $$1.25\,gm$$ of a non-electrolyte and $$20\,gm$$ of water is $$271.9\,K$$. If molar depression constant is $$1.86K\,mol{e^{ - 1}}$$, then molar mass of the solute will be

105.7

106.7

115.3

93.9

## Questions 42 of 50

Question:What is the freezing point of a solution containing $$8.1\,g\,HBr$$ in $$100g$$ water assuming the acid to be 90% ionised $$({K_f}$$ for water $$= 1.86\,K\,mol{e^{ - 1}})$$

$${0.85^o}C$$

$$- {3.53^o}C$$

$${0^o}C$$

$$- {0.35^o}C$$

## Questions 43 of 50

Question:Which of the following aqueous molal solution have highest freezing point

Urea

Barium chloride

Potassium bromide

Aluminium sulphate

## Questions 44 of 50

Question:Which will show maximum depression in freezing point when concentration is 0.1M

NaCl

Urea

Glucose

$${K_2}S{O_4}$$

## Questions 45 of 50

Question:Which of the following will have the highest boiling point at 1 atm pressure

$$0.1\,M\,NaCl$$

$$0.1M$$sucrose

$$0.1M\,BaC{l_2}$$

$$0.1M$$ glucose

## Questions 46 of 50

Question:Which one of the following would produce maximum elevation in boiling point

0.1 M glucose

0.2 M sucrose

0.1 M barium chloride

0.1 M magnesium sulphate

## Questions 47 of 50

Question:Which of the following $$0.10\,m$$ aqueous solution will have the lowest freezing point

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

$${C_5}{H_{10}}{O_5}$$

$$KI$$

$${C_{12}}{H_{22}}{O_{11}}$$

## Questions 48 of 50

Question:For 0.1 M solution, the colligative property will follow the order

$$NaCl > N{a_2}S{O_4} > N{a_3}P{O_4}$$

$$NaCl < N{a_2}S{O_4} < N{a_3}P{O_4}$$

$$NaCl > N{a_2}S{O_4}\,\, \approx \,\,N{a_3}P{O_4}$$

$$NaCl < N{a_2}S{O_4} = N{a_3}P{O_4}$$

## Questions 49 of 50

Question:The observed osmotic pressure of a solution of benzoic acid in benzene is less than its expected value because

Benzene is a non-polar solvent

Benzoic acid molecules are associated in benzene

Benzoic acid molecules are dissociated in benzene

Benzoic acid is an organic compound

## Questions 50 of 50

Question:The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor 'i' is