JEE Questions for Chemistry Solutions Quiz 15 - MCQExams.com

90 gm glucose and 120 gm urea dissolved in 1.46 kg aqueous solution, then what will be the boiling point of the solution at 1 bar pressure ? (Kb = 0.512o C -kg – mole-1, molecular weight of glucose and urea are 180 and 60 gm/mole respectively)
  • 100.876oC
  • 101.024oC
  • 100.248oC
  • 100.007oC
pH of 0.2M dibasic acid H2A is 1.699; then, what will be its osmotic pressure at T K temperature ?
  • 0.22 RT
  • 0.02 RT
  • 0.4 RT
  • 0.1 RT
Boiling point of an aqueous soultion of 0.4m AlCl3 is 100.7oC; then what would be the pressure of ionization of AlCl3 ? Kb – 0.512o C - kg - mole-1.
  • 80.67%
  • 60.5%
  • 76.54%
  • 84.75%
The vapour pressure of homogenous mixture of 10 mole of liquid X and 30 mole of liquid Y at constant temperature is 550 mm. In this solution, 10 mole of liquid Y increases, hence, increase in vapour pressure is 10 mm. Then, find the vapor pressure of pure liquid X and Y at that temperature.
  • Pox = 200 mm, Poy = 500 mm
  • Pox = 400 mm, Poy = 600 mm
  • Pox = 600 mm, Poy = 300 mm
  • Pox = 350 mm, Poy = 500 mm
What amount of urea dissolved in 1 kg water at constant temperature, so that vapour pressure of the solution reduced by 2% ? ( M.W of urea = 60 gm/mole)
  • 68 gm
  • 60 gm
  • 50 gm
  • 75 gm
What would be tne volume of 15% w/v and 5% w/v NaOH solution required to prepare 1 litre aqueous solution of 2M NaOH ? (M.w of Naoh = 40 gram/mole)
  • 300 ml, 700ml
  • 250 ml, 750ml
  • 400 ml, 600ml
  • 280 ml, 720ml
At constant temperature, vapour pressure of an aqueous solution of 1.5 kg glucose decreases to 0.98% in comparision with vapour pressure of pure water then, what quantity of glucose in gram dissolved in the solution ? (Molecular weight of glucose = 180 gm/mole)
  • 148.5 gm
  • 14.85 gm
  • 125 gm
  • 135 gm
At constant pressure, 0.5 m NaCl aqueous solution is diluted by adding water in it. Which of the following statement is correct in this reference ?
  • Van’t Hoff factor (i) and boiling point of the solution both decreases
  • Van’t Hoff factor (i) and boiling point of the solution both increases
  • Van’t Hoff factor (i) decreases while boiling point of the solution both increases
  • Van’t Hoff factor (i) increases while boiling point of the solution both decreases
Boiling point of an aqueous solution of 0.5 m ionic solid substance is 100.5oC; then state the value of i ? (Kb = 0.512oC -kg – mole-1)
  • 1.95
  • 1.85
  • 1.25
  • 0.85
Aqueous solution of substance boils at 100.5oC at 1 bar pressure; then at what temperature it freezes ? (Kb = 0.512oC -kg - mole-1, Kf = 1.86oC - kg – mole-1)
  • 11.2o C
  • 29.84o F
  • 271.8o K
  • -1.2o C
1.4 m aqueous solution of a weak electrolyte AB2 ionizes 20%, then, state boiling point and freezing point of the solution respectively.
  • 100.86o C, -3.12oC
  • 101oC, -3.65oC
  • 274oC, -3.65oC
  • 374oC, -3.65oC
Solute substance in a 1.4 m aqueous solution associates by 25%, then, find the boiling point and freezing point of solution; where, solute exists as trimer in the solution; thus, n = 3. (Kb = 0.512o C • kg • mole-1, Kf = 1.86oC • kg • mole-1)
  • 100.448oC, -2.28oC
  • 373.58oK, -3.65oC
  • 100.59oC, 2.17oC
  • 213oF, 270.83ok
Molecular mass of a weak acid HA is 60gm/mo1 Ifs experimental molecular mass in its 0.7 M aqueous solution obtained from colligative properties is 50gm/mo1. Then calculate ionistion consteint of weak acid HA.
  • 0.023
  • 0.0085
  • 0.035
  • 0.085
At constant temperature, the total pressure of a homogeneous mixture of gas-A and gas-B in a closed container collected on water is 2.0 bar. Their ratio of mole fraction is 1.6 If the values of their KH are 2.4 × 10+4 bur and 4.8 × 104 bar respectively then calculate its ration of mole fraction when dissolved in H2O.
  • 1 : 2
  • 2 : 1
  • 3 : 1
  • 1 : 3
If one of the colligative property of 0.3m aqueous ti sdn. of Na cl and x m aqueous solution of H2SO4 then what would be the approximate vulvae of aqueous solution of H2SO4 ? (Density of ´ m H2So4 solution = 1.185 gm/ml)
  • 0.464 N
  • 0.928 N
  • 0.232 N
  • 0.53 N
At one bar pressure the value of ratio of mole fraction of O2 and N2 gas in air is 1:4 The values of KH of O2 and N2 are 3.3 × 107 Torr and 6.60 × 107 Torr respectively. Then calculate the value of ratio of mole fractions of O2 and N2 gases will be. (1 Torr = 1mm)
  • 3 : 1
  • 2 : 1
  • 1 : 2
  • 1 : 3
According to Boyle-van’t - Hoff law at a consistent temperature, osmotic pressure of a solution is directly proportional to its morality. It means p a C, where C = morality of solution \\ π = Kc Then calculate the value of k in sI unit at 24o c temperature. (R = 8. 314 J/mole k)
  • 24.942 J/mol
  • 2494.2 J/mol
  • 0.024942 J/mol
  • 2.4942 J/mol
Boiling point of an aqueous solution of urea at one bar pressure is 373.41 k. Then at a constant temperature, calculate the percentage decrease in vapour pressure of a solution compared to (kb = 0.512 k.kg. mol-1)
  • 1.42 %
  • 2.56 %
  • 4.17 %
  • 3.44 %
Calculate PH of a solution prepared by mixing equal volume of an aqueous solution of HCI having PH = 2 and PH = 5 at 298 k temp.
  • 3.5
  • 3.0
  • 7.0
  • 2.3
Which of the following is the correct formula for Raoult’s law when non-volatile solute is mixed with liquid solvent. where n=mole traction of solute N= mok fraction of solvent, P= vapour pressure of solution Po = vapour pressure of pure solvent and DP=Decrease in vapour pressure.

  • Chemistry-Solutions-7215.png
  • 2)
    Chemistry-Solutions-7216.png

  • Chemistry-Solutions-7217.png

  • Chemistry-Solutions-7218.png
Decrease in Freezing point of 75.2 gm phenol when dissolved in a solvent having kf = 14 k. kg. mole-1. is 7 k. Calculate the percentage of association of phenol if it is forms a dime in the solution.
  • 62.5 %
  • 80.5 %
  • 70 %
  • 75 %
Which of the following is correct option when kcl is dissolved in H2O. ?
  • ΔH = +ve, ΔS = +ve, ΔG = +ve
  • ΔH = +ve, ΔS = –ve, ΔG = –ve
  • ΔH = +ve, ΔS = +ve, ΔG = –ve
  • ΔH = –ve, ΔS = –ve, ΔG = +ve
Naphthalene is soluble in ether or benzene because. ?
  • dipole-dipole attraction is equal
  • London forces are equal
  • Hydrogen bond
  • Ionic attraction
Four Liquids are given.
(i) Water : more polar and capacity to torm H-bond.
(ii) Hexanol : moderately polar and partial capacity to form H-bond.
(iii) Chloro form : moderately polar and does not capable to form H-bond.
(iv) Octane : non polar and does not capable to form H-bond.
which of the following pair of liquids mixed with each other in very less proportion.
  • I, IV
  • I, II
  • II, III
  • III, IV
Which of the following is applicable for the solubility of gases in liquid.
  • Increases with increase in temperature and pressure
  • decreases with increase in temp and pressure
  • Increases with decrease in temp and increase in pressure
  • Decreases with decrease in temp and increase in pressure
Concentration of lead metal in a blood of any person is more than that of 10 micro gram. dm-1, than that person is considered as on effect of poison section. Then calculate its concentration in ppb (parts per billion)
  • 1
  • 10
  • 100
  • 1000

Chemistry-Solutions-7219.png
  • 60, 90
  • 40, 40
  • 40, 10
  • 10, 40
Decrease in vapour pressure of an aqueous solution. of an electrolyte is 4% what would be the percentage increase in elevation in Boiling point ? (kb = 0.512 k. kg. mol–1)
  • 0.55 %
  • 0.02 %
  • 5.5 %
  • 2 %
For a dilute solution containing 2.5 g of a non-volatile non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm pressure is 2° C . Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take Kb = 0.76 K kg mol-1)
  • 724
  • 740
  • 736
  • 718
Molarity (x) and normality (y) of a solution are related to each other as (M = Molecular mass, E = Equivalent weight)

  • Chemistry-Solutions-7221.png
  • 2)
    Chemistry-Solutions-7222.png

  • Chemistry-Solutions-7223.png

  • Chemistry-Solutions-7224.png
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