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JEE Questions for Chemistry Solutions Quiz 15 - MCQExams.com
JEE
Chemistry
Solutions
Quiz 15
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 = 0.512
o
C -kg – mole
-1
, molecular weight of glucose and urea are 180 and 60 gm/mole respectively)
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0%
100.876oC
0%
101.024oC
0%
100.248oC
0%
100.007oC
pH of 0.2M dibasic acid H
2
A is 1.699; then, what will be its osmotic pressure at T K temperature ?
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0%
0.22 RT
0%
0.02 RT
0%
0.4 RT
0%
0.1 RT
Boiling point of an aqueous soultion of 0.4m AlCl
3
is 100.7
o
C; then what would be the pressure of ionization of AlCl
3
? Kb – 0.512
o
C - kg - mole
-1
.
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0%
80.67%
0%
60.5%
0%
76.54%
0%
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.
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0%
Pox = 200 mm, Poy = 500 mm
0%
Pox = 400 mm, Poy = 600 mm
0%
Pox = 600 mm, Poy = 300 mm
0%
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)
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0%
68 gm
0%
60 gm
0%
50 gm
0%
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)
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0%
300 ml, 700ml
0%
250 ml, 750ml
0%
400 ml, 600ml
0%
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)
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0%
148.5 gm
0%
14.85 gm
0%
125 gm
0%
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 ?
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0%
Van’t Hoff factor (i) and boiling point of the solution both decreases
0%
Van’t Hoff factor (i) and boiling point of the solution both increases
0%
Van’t Hoff factor (i) decreases while boiling point of the solution both increases
0%
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 100.5
o
C; then state the value of i ? (Kb = 0.512
o
C -kg – mole
-1
)
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0%
1.95
0%
1.85
0%
1.25
0%
0.85
Aqueous solution of substance boils at 100.5
o
C at 1 bar pressure; then at what temperature it freezes ? (K
b
= 0.512
o
C -k
g
- mole
-1
, K
f
= 1.86
o
C - k
g
– mole
-1
)
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0%
11.2o C
0%
29.84o F
0%
271.8o K
0%
-1.2o C
1.4 m aqueous solution of a weak electrolyte AB
2
ionizes 20%, then, state boiling point and freezing point of the solution respectively.
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0%
100.86o C, -3.12oC
0%
101oC, -3.65oC
0%
274oC, -3.65oC
0%
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. (K
b
= 0.512
o
C • kg • mole
-1
, K
f
= 1.86
o
C • kg • mole
-1
)
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0%
100.448oC, -2.28oC
0%
373.58oK, -3.65oC
0%
100.59oC, 2.17oC
0%
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.
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0%
0.023
0%
0.0085
0%
0.035
0%
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 K
H
are 2.4 × 10
+4
bur and 4.8 × 10
4
bar respectively then calculate its ration of mole fraction when dissolved in H
2
O.
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0%
1 : 2
0%
2 : 1
0%
3 : 1
0%
1 : 3
If one of the colligative property of 0.3m aqueous ti sdn. of Na cl and x m aqueous solution of H
2
SO
4
then what would be the approximate vulvae of aqueous solution of H
2
SO
4
? (Density of ´ m H2So4 solution = 1.185 gm/ml)
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0%
0.464 N
0%
0.928 N
0%
0.232 N
0%
0.53 N
At one bar pressure the value of ratio of mole fraction of O
2
and N
2
gas in air is 1:4 The values of KH of O
2
and N
2
are 3.3 × 10
7
Torr and 6.60 × 10
7
Torr respectively. Then calculate the value of ratio of mole fractions of O
2
and N
2
gases will be. (1 Torr = 1mm)
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0%
3 : 1
0%
2 : 1
0%
1 : 2
0%
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 24
o
c temperature. (R = 8. 314 J/mole k)
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0%
24.942 J/mol
0%
2494.2 J/mol
0%
0.024942 J/mol
0%
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 (k
b
= 0.512 k.kg. mol
-1
)
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0%
1.42 %
0%
2.56 %
0%
4.17 %
0%
3.44 %
Calculate P
H
of a solution prepared by mixing equal volume of an aqueous solution of HCI having P
H
= 2 and P
H
= 5 at 298 k temp.
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0%
3.5
0%
3.0
0%
7.0
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.
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0%
0%
2)
0%
0%
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.
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0%
62.5 %
0%
80.5 %
0%
70 %
0%
75 %
Which of the following is correct option when kcl is dissolved in H
2
O. ?
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0%
ΔH = +ve, ΔS = +ve, ΔG = +ve
0%
ΔH = +ve, ΔS = –ve, ΔG = –ve
0%
ΔH = +ve, ΔS = +ve, ΔG = –ve
0%
ΔH = –ve, ΔS = –ve, ΔG = +ve
Naphthalene is soluble in ether or benzene because. ?
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0%
dipole-dipole attraction is equal
0%
London forces are equal
0%
Hydrogen bond
0%
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.
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0%
I, IV
0%
I, II
0%
II, III
0%
III, IV
Which of the following is applicable for the solubility of gases in liquid.
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0%
Increases with increase in temperature and pressure
0%
decreases with increase in temp and pressure
0%
Increases with decrease in temp and increase in pressure
0%
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)
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0%
1
0%
10
0%
100
0%
1000
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0%
60, 90
0%
40, 40
0%
40, 10
0%
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 ? (k
b
= 0.512 k. kg. mol
–1
)
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0%
0.55 %
0%
0.02 %
0%
5.5 %
0%
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
K
b
= 0.76 K kg mol
-1
)
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0%
724
0%
740
0%
736
0%
718
Molarity (x) and normality (y) of a solution are related to each other as (M = Molecular mass, E = Equivalent weight)
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0%
0%
2)
0%
0%
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