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.
3% solution of glucose is isotonic with 1% solution of a non-volatile non-electrolyte substance. The molecular mass of the substance would be
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
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
?Partial vapour pressure of a solution component is directly proportional to its mole fraction?. This statement is known as
4.Ostwalds dilution law.
A 500 g tooth paste sample has 02 g fluoride concentration What is the concentration of fluoride in terms of ppm
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
A colligative property is
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
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.
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.
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.
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
2.exceeds the solubility
3.is less than the solubility
4.is equal to the solubility of that substance in water
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.
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
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
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
An aqueous solution of glucose is 10% in strength. The volume in which 1 gm mole of it is dissolved will be
1.shows no deviation from Raoults law
2.shows a positive deviation from Raoults law
4.None of them
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
Certain substance trimerises when dissolved in a solvent A. The vant Hoffs factor i for the solutions is
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
Ebullioscopic constant depends upon
1.nature of solvent
2.nature of solute
3.conditions of temperature and pressure
4.all the above factors.
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.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
Freezing point of an aqueous solution is 272.48 K. The osmotic pressure of the same solution at 310 K will be
How many grams of a dibasic acid (Molecular mass = 200) should be present in 100 ml of its aqueous solution to give decinormal strength?
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.
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.
2.solvent molecules only
3.both solute and solvent
1.1 kg of solvent
2.1 litre of solvent
3.1 litre of solute
4.1 mole of solute
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.Ideal equation of state
3.Vant Hoff equation
4.Boyle-Vanst Hoff equation
1.decreasing the temperature
2.increasing the volume
3.increasing the number of molecules of the solute
4.none of the above.
Osmotic pressure of a solution of electrolyte does not depend onI. Nature of solute II. Nature of solventIII. Temperature IV. Molar conc. of solute.
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.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.
1.temperature and pressure both are decreased
2.temperature and pressure both are increased
3.temperature is increased
4.pressure is decreased
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
The cryoscopic constant for water is
4.Depends on proportion of alcohol in the solution.
The molarity of pure water is
The molarity of solution obtained by dissolving 001 moles of NaCl in 500 ml of solution is
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
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
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
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
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
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
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.number of moles
2.number of molecules
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
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.
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
4.attains equilibrium conditions
1.Relative lowering of vapour pressure
4.Both b and c.
Which of the following change with increase in temperatureI Molality II MolarityIII Mole fraction IV Normality
2.Lowering of 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.