IIT JEE/IIT JEE Solutions Mcq Questions part 2 Sample Test,Sample questions

Question:
0.1 M solution of glucose and 0.1 M solute of urea are placed on two sides of semipermeable membrane to equal heights. Which of the following is correct?     

1.There will be flow of water from glucose side to urea.

2.There will be flow of water from urea side to glucose.

3.There will be no net flow across the membrane.

4.Glucose solution will move into urea solution.


Question:
18% (W/V) solution of urea (Mol. Mass = 60) is     

1.1 M

2.2 M

3.0.3 M

4.3 M.


Question:
3% solution of glucose is isotonic with 1% solution of a non-volatile non-electrolyte substance. The molecular mass of the substance would be 

1.180

2.360

3.420

4.60


Question:
34.2 gm of sugar (mol. wt. 342) is dissolved in 90 gm of water at the boiling point of water vapour pressure of solution at that very temperature will be     

1.720 mm Hg

2.345.1 mm Hg

3.765.1 mm Hg

4.745.1 mm Hg


Question:
4 L of 0.2 M aqueous solution of KOH is mixed with 2 L of 0.5 M aqueous solution of KOH. The molarity of the resulting solution is     

1.0.7 M

2.0.3 M

3.0.2 M

4.1.8 M.


Question:
45% solution of glucose would be isotonic with respect to ?? solution of urea     9%

1.4.50%

2.13.50%

3.1.50%

4.9%.


Question:
5.85 g of NaCl is dissolved in 500 ml of water. The molarity is     

1.0.1

2.0.2

3.0.3

4.0.4.


Question:
?Partial vapour pressure of a solution component is directly proportional to its mole fraction?. This statement is known as     

1.Henrys law

2.Raoults law

3.Distribution law

4.Ostwalds dilution law.


Question:
A 500 g tooth paste sample has 02 g fluoride concentration What is the concentration of fluoride in terms of ppm     

1.250

2.200

3.400

4.1000


Question:
A colligative property depends upon      

1.number of particles in solution

2.number of molecules in solution

3.number of ions of solute

4.None of the above


Question:
A colligative property is     

1.electrical conductivity

2.conductivity

3.osmotic pressure

4.molecular pressure


Question:
A crystal of blue vitriol is placed in its saturated solution. Which of the following observations would you expect to make provided the temperature is constant?  A super ? saturated solution will be formed   

1.A super ? saturated solution will be formed

2.The crystals will be dissolved

3.No change will occur

4.Crystals will separate out


Question:
A liquid is in equilibrium with its vapour at its boiling point. On the average  the molecules of the two phases will have     

1.same magnitude of Interparticle forces

2.same potential energy

3.same total energy

4.same free energy.


Question:
A non-volatile electrolyte dissolved in an aqueous solution in same molal proportion as non-electrolyte produces     

1.same colligative effect

2.higher colligative effect

3.lower colligative effect

4.no colligative effect.


Question:
A non-volatile electrolyte dissolved in equimolal proportion as non-volatile non-electrolyte produces     

1.same colligative effect

2.lower colligative effect

3.higher colligative effect

4.no colligative effect.


Question:
A solution containing one gram of substance in 100 ml of water is found to be isotonic with a solution of 3 grams of glucose in 100 ml of water. The molecular mass of the substance is     

1.110

2.54

3.60

4.45


Question:
A supersaturated solution is a metastable solution whose solute concentration     

1.continuously changes

2.exceeds the solubility

3.is less than the solubility

4.is equal to the solubility of that substance in water


Question:
According to Raoults law  the relative lowering of vapour pressure of a solution of non-volatile solute is  equal to mole fraction of solvent   

1.equal to mole fraction of solvent

2.equal to mole fraction of solute

3.directly proportional to mole fraction of solute

4.equal to normality of the solution.


Question:
According to Raoults law for solution containing non-volatile solution the relative lowering of vapour pressure for solution is     

1.inversely proportional to mole fraction of the solute

2.directly proportional to mole fraction of solute

3.equal to mole fraction of solute

4.equal to mole fraction of solvent


Question:
Acetic acid exists as dimers in benzene if on dissolving 1.65 gm of acetic acid in 100 gm of benzene the Vant Hoff factor i comes out to be 0.508 then extent of association of acetic acid in benzene is     

1.205%

2.95%

3.98.30%

4.20%


Question:
An aqueous solution containing 6 g of urea in 500 ml of solution has a density equal to 1.052. If the molecular mass of urea is 60 then the molality of solution is     

1.0.192

2.0.96

3.0.2

4.2


Question:
An aqueous solution of glucose is 10% in strength. The volume in which 1 gm mole of it is dissolved will be     

1.18 L

2.9 L

3.0.9 L

4.1.8 L.


Question:
An azeotropic solution of two liquids has boiling point lower than ether when it     

1.shows no deviation from Raoults law

2.shows a positive deviation from Raoults law

3.is saturated.

4.None of them


Question:
At 298 K the vapour pressure of pure X is 50 mm Hg and that of pure Y is 60 mm Hg. If 1 mole of X and 1 mole of Y are mixed than vapour pressure of the solution was found out to be 57.5 mm Hg. The solution     

1.shows negative deviation

2.shows positive deviation

3.forms a constant boiling

4.behaves ideally


Question:
Certain substance trimerises when dissolved in a solvent A. The vant Hoffs factor i for the solutions is     

1.1

2.3-Jan

3.3

4.unpredictable


Question:
During molecular weight determination of non-volatile solute by cryoscopic method Beckmann Thermometer is used to determine the     

1.depression in freezing point or elevation in boiling point

2.exact freezing point of the solution

3.exact boiling point of the solution

4.lowering in vapour pressure


Question:
Ebullioscopic constant depends upon     

1.nature of solvent

2.nature of solute

3.conditions of temperature and pressure

4.all the above factors.


Question:
For a solution containing non-volatile solute the relative lowering of vapour pressure is 02 If the solution contains 5 moles in all which of the following are true?I Mole fraction of solute in the solution is02II No of moles of solute in the solution is 02III No of moles of solvent in the solution is 4IV Mole fraction of solvent is02    

1.I IV

2.II III

3.I III

4.II IV.


Question:
For dilute solutions  Raoults law states that     

1.the relative lowering in vapour pressure is equal to the mole fraction of the solute

2.the relative lowering in vapour pressure is equal to the amount of solvent in the solution

3.the vapour pressure of the solution is proportional to that of the solvent

4.lowering of vapour pressure is equal to the mole fraction of the solution


Question:
For which of the following solutes i is greater than 1?     

1.Urea

2.Sucrose

3.Sodium chloride

4.glucose.


Question:
Freezing point of an aqueous solution is 272.48 K. The osmotic pressure of the same solution at 310 K will be     

1.7.1 pka

2.56 torr

3.7.1 atm

4.6.1 atm


Question:
How many grams of a dibasic acid (Molecular mass = 200) should be present in 100 ml of its aqueous solution to give decinormal strength? 

1.1g

2.2g

3.10 g

4.20 g


Question:
Hydrochloric acid solutions A and B have concentrations 0.5 N and 0.1 N respectively. The volumes of solutions A and B required to make 2 litres of 0.2 N hydrochloric acid are     

1.0.5 L of A + 1.5 L of B

2.1.5 L of A + 0.5 L of B

3.1.0 L of A + 1.0 L of B

4.0.75 L of A + 1.25 L of B.


Question:
If 0.1 M solution of glucose and 0.1 M solution of urea are placed on two sides of the semipermeable membrane to equal heights then it will be correct to say that     

1.There will be no net movement across the membrane

2.Glucose will flow towards urea towards urea solution

3.Urea will flow towards glucose solution

4.Water will flow from urea solution to glucose solution.


Question:
In dilute solution the depression in freezing point is directly proportional to     

1.morality

2.normality

3.molality

4.boiling point


Question:
In the phenomenon of osmosis  the semipermeable membrane allows the passage if     

1.solute particles

2.solvent molecules only

3.both solute and solvent

4.None.


Question:
In which of the following cases 1% aq Solution will have the lowest freezing point?     

1.Glucose

2.Fructose

3.Urea

4.Potassium acetate


Question:
Increasing the temperature of an aqueous solution will cause decrease in     

1.Molality

2.Molarity

3.Mole fraction

4.% (W/V).


Question:
Isotonic solutions are those which have same     

1.osmotic pressure

2.vapour pressure

3.boiling points

4.velocity


Question:
Molality of a solution is the number of moles of solute in     

1.1 kg of solvent

2.1 litre of solvent

3.1 litre of solute

4.1 mole of solute


Question:
On dissolving 8.8 gm of non-volatile solute to 100 gm of water the vapour pressure of ice becomes 4.559 mm Hg. If vapour pressure of pure ice is 4.58 mm Hg than molecular weight of the substance should be     

1.345.46

2.245.46 gm

3.34.576 gm

4.360


Question:
or solutions the relation PV = nRT is called     

1.Ideal equation of state

2.Charles equation

3.Vant Hoff equation

4.Boyle-Vanst Hoff equation


Question:
Osmotic pressure of a solution increases by     

1.decreasing the temperature

2.increasing the volume

3.increasing the number of molecules of the solute

4.none of the above.


Question:
Osmotic pressure of a solution of electrolyte does not depend onI. Nature of solute II. Nature of solventIII. Temperature IV. Molar conc. of solute.    

1.I

2.I II

3.II III

4.III IV.


Question:
Osmotic pressure of blood is 7.65 atm at 310 K. An aqueous solution of glucose that will be isotonic with blood will be     

1.2.71 gm

2.54.30%

3.5.43%

4.3%


Question:
Raoults law for solutions containing non-volatile solute is concerned with lowering of     

1.boiling point

2.vapour pressure

3.osmotic pressure

4.melting point


Question:
Solutions with same vapour pressures are called     

1.isotonic

2.isopiestic

3.hypertonic

4.isomorphic.


Question:
The addition of a non-volatile solute to the solvent results in lowering of     

1.vapour pressure as well as boiling point

2.vapour pressure as well as density

3.vapour pressure as well as freezing point

4.boiling point as well as freezing point.


Question:
The amount of a solute required to prepare 10 litres of its decinomrla solution is     

1.0.1 mole

2.0.01 mole

3.1.0 mole

4.1.5 mole


Question:
The amount of gas dissolving in a given volume of the liquid decreases when     

1.temperature and pressure both are decreased

2.temperature and pressure both are increased

3.temperature is increased

4.pressure is decreased


Question:
The boiling point of a 0.1 molal aqueous solution of urea is 100.180C under one atmospheric pressure. The molal elevation constant of water is     

1.5.4

2.0.18

3.1.8

4.3.6


Question:
The cryoscopic constant for water is      

1.1.86

2.2.86

3.1.58

4.3.95


Question:
The enthalpy change on mixing water and ethanol at room temperature is     

1.Zero

2.Positive

3.Negative

4.Depends on proportion of alcohol in the solution.


Question:
The molality of 2% (w/w) aqueous solution of sodium chloride is     

1.0.17 m

2.0.7 m

3.1 m

4.0.34 m.


Question:
The molality of an aqueous solution of NaOH containing 8 gram in 2 litres of solution is:     

1.1.5 M

2.1.0 M

3.0.4 M

4.0.1 M


Question:
The molarity of 6% (W/V) solution of acetic acid is     

1.0.01 M

2.0.1 M

3.1 M

4.0.5 M.


Question:
The molarity of decinormal aqueous solution of sodium hydroxide is     

1.M/5

2.M/10

3.M/2

4.M/100.


Question:
The molarity of pure water is     

1.90

2.556

3.55.6

4.9


Question:
The molarity of solution obtained by dissolving 001 moles of NaCl in 500 ml of solution is     

1.0.01 M

2.0.005 M

3.0.02 M

4.0.10 M.


Question:
The molecular mass of ethyl alcohol is 46. The molality of a solution of ethyl alcohol in water containing 23.0 g of ethyl alcohol in 500 ml solution is     

1.2.5 M

2.3.0 M

3.1.0 M

4.1.5 M


Question:
The normality of a 2.3 M sulphuric acid solution is     

1.0.46 N

2.0.23 N

3.2.3 N

4.4.6 N.


Question:
The number of moles of sodium hydroxide present in 25 L of 05 M aqueous solution is  

1.1.25

2.0.5

3.12.5

4.5


Question:
The osmotic pressure of a solution of benzoic acid in benzene is found to be half the expected value. This is due to the     

1.association of benzoic acid molecules forming dimmers

2.wrong method of measurement of osmotic pressure

3.limitation of the theory of osmotic pressure

4.ionization of benzoic acid


Question:
The ratio of elevation in boiling point of aqueous solution of sodium chloride to that of an aqueous solution of glucose of same molalities is approximately  

1.1

2.2

3.0.5

4.2.5


Question:
The solution that can distil with change in composition is called     

1.saturated solution

2.azeotrope

3.zerotrope

4.none-ideal solution


Question:
The vapour pressure of pure benzene at 298 K is 97.0 mm Hg. The vapour pressure of solution containing 10.0 gm of napthalene (mol. wt. 128) in 100 gm of benzene at 398 K will be     

1.79.5 mm Hg

2.91.43 mm Hg

3.81.45 mm Hg

4.66.5 mm Hg


Question:
The vapour pressure of water at room temperature is 23.8 mm Hg. The vapour pressure of an aqueous solution of mole fraction 0.1 is equal to     

1.11.22 mm Hg

2.21.42 mm Hg

3.24.2 mm Hg

4.11.42 mm Hg


Question:
The vapour pressure of water at room temperature is 30 mm. If the mole fraction of the solvent in solution is 0.9 the vapour pressure of aqueous solution at room temperature will be     

1.18 mm

2.36 mm

3.72 mm

4.27 mm


Question:
The volume of water that must be added to a mixture of 250 ml of M HCl and 750 ml of 2 M HCl to obtain 2.5 M solution is     

1.75 ml

2.150 ml

3.100 ml

4.200 ml


Question:
Two beakers contain 1 L and 250 ml of pure water respectively. What is same in them?     

1.number of moles

2.number of molecules

3.molarity

4.mass.


Question:
Two liquids A and B form an ideal solution At 300 K the vapour pressure of a solution of 1 mole of A and x moles of B is 550 mm If the vapour pressures of pure A and B are 400 mm and 600 mm respectively  then x is     

1.1

2.2

3.3

4.4


Question:
Two solutions A and B are separated by a semipermeable membrane. Solution B has greater vapour pressure than solution A. Water will flow from     

1.A to B

2.B to A

3.No flow of water

4.Direction of flow cannot be predicted.


Question:
What volume of 0.8 M solution contains 0.1 mole of the solute?     

1.100 ml

2.125 ml

3.500 ml

4.62.5 ml.


Question:
When 18 g of a compound was dissolved in 100 g of water the vapour pressure of the latter was lowered from 17.54 mm to 17.23 mm of mercury. The molecular mass of compound is     

1.2900

2.368

3.184

4.92


Question:
When a saturated solution of sodium chloride is heated  it becomes     

1.unsaturated

2.supersaturated

3.remains saturated

4.attains equilibrium conditions


Question:
Which is an example of colligative property?     

1.Boiling point

2.osmosis

3.freezing point

4.osmotic pressure.


Question:
Which of the following are not colligative properties?     

1.Relative lowering of vapour pressure

2.Surface tension

3.Osmosis

4.Both b and c.


Question:
Which of the following change with increase in temperatureI Molality II MolarityIII Mole fraction IV Normality     

1.I II

2.II

3.I IV

4.II IV.


Question:
Which of the following is not a colligative property?     

1.Boiling pressure

2.Lowering of freezing point

3.Vapour pressure

4.Osmotic pressure


Question:
Which of the following solutions will have highest value of depression in freezing point?     

1.6% aqueous solution of glucose

2.6% aqueous solution of urea

3.6% aqueous solution of sucrose

4.all the above will have same value.


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