# Solution Test 1

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:Which is correct about Henry's law

The gas in contact with the liquid should behave as an ideal gas

There should not be any chemical interaction between the gas and liquid

The pressure applied should be high

All of these

## Questions 2 of 50

Question:The statement : If 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere, 0.006 moles will be dissolved under a pressure of 2 atmospheres", illustrates

Dalton's law of partial pressure

Graham's law

Raoult's law

Henry's law

## Questions 3 of 50

Question:A mixture has 18g water and 414g ethanol. The mole fraction of water in mixture is (assume ideal behaviour of the mixture)

0.1

0.4

0.7

0.9

## Questions 4 of 50

Question:The number of molecules in 4.25 g of ammonia is approximately

$$0.5 \times {10^{23}}$$

$$1.5 \times {10^{23}}$$

$$3.5 \times {10^{23}}$$

$$2.5 \times {10^{23}}$$

## Questions 5 of 50

Question:2.0 molar solution is obtained , when 0.5 mole solute is dissolved in

250 ml solvent

250 g solvent

250 ml solution

1000 ml solvent

## Questions 6 of 50

Question:How many gram of HCl will be present in $$150\,ml$$ of its 0.52 M solution

2.84 gm

5.70 gm

8.50 gm

3.65 gm

## Questions 7 of 50

Question:Which of the following should be done in order to prepare $$0.40M\,NaCl$$ starting with $$100\,ml$$ of $$0.30M\,NaCl$$ (mol.wt. of $$NaCl = 58.5$$)

Add $$0.585\,g\,NaCl$$

Add $$20\,ml$$ water

Add $$0.010ml\,NaCl$$

Evaporate $$10ml$$ water

1 and 3 are correct

## Questions 8 of 50

Question:Which of the following solutions has the highest normality

8 gm of $$KOH$$/ litre

$$N$$ phosphoric acid

6 gm of $$NaOH$$/ 100 m

l$$0.5M\,{H_2}S{O_4}$$

## Questions 9 of 50

Question:To prepare a solution of concentration of 0.03 g/ml of $$AgN{O_3}$$, what amount of $$AgN{O_3}$$ should be added in 60 ml of solution

1.8

0.8

0.18

None of these

## Questions 10 of 50

Question:How many grams of dibasic acid (mol. wt. 200) should be present in $$100ml$$ of its aqueous solution to give decinormal strength

$$1g$$

$$2g$$

$$10g$$

$$20g$$

## Questions 11 of 50

Question:If 25 ml of 0.25 M NaCl solution is diluted with water to a volume of 500ml the new concentration of the solution is

0.167 M

0.0125 M

0.833 M

0.0167 M

## Questions 12 of 50

Question:10 grams of a solute is dissolved in 90 grams of a solvent. Its mass percent in solution is

0.01

11.1

10

9

## Questions 13 of 50

Question:A solution contains $$25\% {H_2}O$$ ,$$25\% {C_2}{H_5}OH$$ and $$50\% \,C{H_3}\,COOH$$ by mass. The mole fraction of $${H_2}O$$ would be

0.25

2.5

0.503

5.03

## Questions 14 of 50

Question:A 5 molar solution of $${H_2}S{O_4}$$ is diluted from 1 litre to 10 litres. What is the normality of the solution

0.25 N

1 N

2 N

7 N

## Questions 15 of 50

Question:To neutralise completely 20 mL of 0.1 M aqueous solution of phosphorous acid $$({H_3}P{O_3}),$$ the volume of 0.1 M aqueous KOH solution required is

40 mL

20 mL

10 mL

60 mL

## Questions 16 of 50

Question:On dissolving 1 mole of each of the following acids in 1 litre water, the acid which does not give a solution of strength $$1N$$ is

$$HCl$$

Perchloric acid

$$HN{O_3}$$

Phosphoric acid

## Questions 17 of 50

Question:Molarity of a solution prepared by dissolving 75.5 g of pure KOH in 540 ml solution is

3.05 M

1.35 M

2.50 M

4.50 M

## Questions 18 of 50

Question:Which one of the following is an extensive property

Molar volume

Molarity

Number of moles

Mole fraction

## Questions 19 of 50

Question:The number of moles of $$KCl$$ in $$1000\,ml$$ of 3 molar solution is

1

2

3

1.5

## Questions 20 of 50

Question:The unit of molality is

Mole per litre

Mole per kilogram

Per mole per litre

Mole litre

## Questions 21 of 50

Question:The relative lowering of the vapour pressure is equal to the mole fraction of the solute." This law is called

Henry's law

Raoult's law

Ostwald's law

Arrhenius's law

## Questions 22 of 50

Question:The relative lowering of vapour pressure produced by dissolving 71.5 g of a substance in 1000 g of water is 0.00713. The molecular weight of the substance will be

18

342

60

180

## Questions 23 of 50

Question:Among the following substances the lowest vapour pressure is exerted by

Water

Mercury

Kerosene

Rectified spirit

## Questions 24 of 50

Question:According to Raoult's law the relative lowering of vapour pressure of a solution of volatile substance is equal to

Mole fraction of the solvent

Mole fraction of the solute

Weight percentage of a solute

Weight percentage of a solvent

## Questions 25 of 50

Question:60 gm of Urea (Mol. wt 60) was dissolved in 9.9 moles, of water. If the vapour pressure of pure water is $${P_o}$$, the vapour pressure of solution is

0.10 $${P_o}$$

1.10 $${P_o}$$

0.90 $${P_o}$$

0.99 $${P_o}$$

## Questions 26 of 50

Question:The vapour pressure of water at $${20^o}C$$ is 17.54 mm. When 20g of a non-ionic, substance is dissolved in 100g of water, the vapour pressure is lowered by 0.30 mm. What is the molecular weight of the substances

210.2

206.88

215.2

200.8

## Questions 27 of 50

Question:All form ideal solutions except

$${C_2}{H_5}Br$$ and $${C_2}{H_5}I$$

$${C_6}{H_5}Cl$$ and $${C_6}{H_5}Br$$

$${C_6}{H_6}$$ and $${C_6}{H_5}C{H_3}$$

$${C_2}{H_5}I$$ and $${C_2}{H_5}OH$$

## Questions 28 of 50

Question:Which property is shown by an ideal solution

It follows Raoult's law

$$\Delta {H_{mix}} = 0$$

$$\Delta {V_{mix}} = 0$$

All of these

## Questions 29 of 50

Question:Which of the following mixture shows positive deviation by ideal behavior

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

$${C_6}{H_6} + {C_6}{H_5}C{H_3}$$

$${H_2}O + HCl$$

$$CC{l_4} + CHC{l_3}$$

## Questions 30 of 50

$${P_A} \ne P_A^o \times {X_A}$$

$$\Delta {H_{mix}} \ne 0$$

$$\Delta {V_{mix}} \ne 0$$

All of these

## Questions 31 of 50

Question:Osmotic pressure of a solution containing 0.1 mole of solute per litre at $$273K$$ is (in atm)

$$\frac{{0.1}}{1} \times 0.08205 \times 273$$

$$0.1 \times 1 \times 0.08205 \times 273$$

$$\frac{1}{{0.1}} \times 0.08205 \times 273$$

$$\frac{{0.1}}{1} \times \frac{{273}}{{0.08205}}$$

## Questions 32 of 50

Question:A solution contains non-volatile solute of molecular mass $${M_p}$$. Which of the following can be used to calculate molecular mass of the solute in terms of osmotic pressure (m = Mass of solute, V = Volume of solution and p = Osmotic pressure)

$$Mp = \left( {\frac{m}{\pi }} \right)\,VRT$$

$$Mp = \left( {\frac{m}{V}} \right)\frac{{RT}}{\pi }$$

$$Mp = \left( {\frac{m}{V}} \right)\frac{\pi }{{RT}}$$

$$Mp = \left( {\frac{m}{V}} \right)\,\pi RT$$

## Questions 33 of 50

Question:The osmotic pressure of $$1\,m$$ solution at $${27^o}C$$ is

2.46 atm

24.6 atm

1.21 atm

12.1 atm

## Questions 34 of 50

Question:Osmotic pressure of a solution can be measured quickly and accurately by

Berkeley and Hartley's method

Morse's method

Pfeffer's method

De Vries method

## Questions 35 of 50

Question:Which one of the following would lose weight on exposure to atmosphere

Concentrated $${H_2}S{O_4}$$

Solid $$NaOH$$

A saturated solution of $$C{O_2}$$

Anhydrous sodium carbonate

## Questions 36 of 50

Question:The molecular weight of $$NaCl$$ determined by osmotic pressure method will be

Same as theoritical value

Higher than theoritical value

Lower than theoritical value

None of these

## Questions 37 of 50

Question:If molecular weight of compound is increased then sensitivity is decreased in which of the following methods

Elevation in boiling point

Viscosity

Osmosis

Dialysis

## Questions 38 of 50

Question:If solubility of $$NaCl$$ at $${20^o}C$$ is 35 $$gm$$ per 100 gm of water. Then on adding 50 gm of $$NaCl$$ to the same volume at same temperature the salt remains undissolved is

15 gm

20 gm

50 gm

35 gm

## Questions 39 of 50

Question:When a substance is dissolved in a solvent, the vapour pressure of solvent decreases. It brings

A decrease in boiling point of solution

An increase in boiling point of the solution

A decrease in freezing point of the solution

An increase in freezing point of the solution

## Questions 40 of 50

Question:Elevation in boiling point was $${0.52^o}C$$ when $$6\,gm$$ of a compound $$X$$ was dissolved in $$100\,gm$$ of water. Molecular weight of $$X$$ is $$({K_b}$$ for water is 0.52 per 1000 gm of water)

120

60

180

600

## Questions 41 of 50

Question:Mark the correct relationship between the boiling points of very dilute solutions of $$BaC{l_2}\,({t_1})$$ and $$KCl\,({t_2})$$, having the same molarity

$${t_1} = {t_2}$$

$${t_1} > {t_2}$$

$${t_2} > {t_1}$$

$${t_2}$$ is approximately equal to $${t_1}$$

## Questions 42 of 50

Question:Molal depression constant for water is $${1.86^o}C$$. The freezing point of a 0.05 molal solution of a non-electrolyte in water is

$$- {1.86^o}C$$

$$- {0.93^o}C$$

$$- {0.093^o}C$$

$${0.93^o}C$$

## Questions 43 of 50

Question:Given that $$\Delta {T_f}$$ is the depression in freezing point of the solvent in a solution of a non-volatile solute of molality $$m$$, the quantity $$\mathop {\lim }\limits_{m \to 0} \left( {\frac{{\Delta {T_f}}}{m}} \right)$$ is equal to

Zero

One

Three

None of the above

## Questions 44 of 50

Question:The freezing point of 1 percent solution of lead nitrate in water will be

Below $${0^o}C$$

$${0^o}C$$

$${1^o}C$$

$${2^o}C$$

## Questions 45 of 50

Question:Osmotic pressure of 0.1 M solution of $$NaCl$$ and $$N{a_2}S{O_4}$$ will be

Same

Osmotic pressure of $$NaCl$$ solution will be more than $$N{a_2}S{O_4}$$ solution

Osmotic pressure of $$N{a_2}S{O_4}$$ solution will be more than $$NaCl$$

Osmotic pressure of $$NaS{O_4}$$ will be less than that of $$NaCl$$ solution

## Questions 46 of 50

Question:Which of the following solutions has highest osmotic pressure

$$1\,M\,NaCl$$

1 M urea

1 M sucrose

1 M glucose

## Questions 47 of 50

Question:Which of the following has lowest freezing point

$$0.1\,M$$ aqueous solution of glucose

$$0.1\,M$$ aqueous solution of $$NaCl$$

$$0.1M$$ aqueous solution of $$ZnS{O_4}$$

$$0.1\,M$$ aqueous solution of urea

## Questions 48 of 50

Question:The freezing points of equimolar solutions of glucose, $$KN{O_3}$$ and $$AlC{l_3}$$ are in the order of

$$AlC{l_3} < KN{O_3} < {\rm{Glucose}}$$

$${\rm{Glucose}} < KN{O_3} < AlC{l_3}$$

$${\rm{Glucose}} < AlC{l_3} < KN{O_3}$$

$$AlC{l_3} < {\rm{Glucose}} < KN{O_3}$$

## Questions 49 of 50

Question:If $$\alpha$$ is the degree of dissociation of $$N{a_2}S{O_4}$$, the Vant Hoff's factor (i) used for calculating the molecular mass is

$$1 + \alpha$$

$$1 + 2\alpha$$

$$1 - 2\alpha$$

None of these

## Questions 50 of 50

Question:Van't Hoff factor $$i$$

$$= \frac{{{\rm{Normal molecular mass}}}}{{{\rm{Observed molecular mass}}}}$$
$$= \frac{{{\rm{Observed molecular mass}}}}{{{\rm{Normal molecular mass}}}}$$