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question_answer1)
For preparing 0.1 N solution of a compound from its impure sample (percentage purity of which is known) weight of the substance required will be
A)
less than the theoretical weight. done
clear
B)
more than the theoretical weight. done
clear
C)
same as the theoretical weight. done
clear
D)
None of these done
clear
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question_answer2)
A solution is prepared by dissolving \[10g\text{ }NaOH\]in 1250 mL of a solvent of density 0.8 g/mL. The molality of the solution in mol \[k{{g}^{-1}}\]is
A)
0.25 done
clear
B)
0.2 done
clear
C)
0.008 done
clear
D)
0.0064 done
clear
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question_answer3)
Two solutions of a substance (non-electrolyte) are mixed in the following manner. 480 mL of 1.5 M first solution +520 mL of 1.2 M second solution. What is the molarity of the final mixture?
A)
2.70 M done
clear
B)
1.344 M done
clear
C)
1.50 M done
clear
D)
1.20 M done
clear
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question_answer4)
Formation of a solution from two components can be considered as
(i) Pure solvent\[\to \] separated solvent molecules, \[\Delta {{H}_{1}}\] |
(ii) Pure solute \[\to \] separated solute molecules, \[\Delta {{H}_{2}}\] |
(iii) Separated solvent and solute molecules \[\to \] Solution, \[\Delta {{H}_{3}}\] |
Solution so formed will be ideal if |
A)
\[\Delta {{H}_{\text{soln}}}=\Delta {{H}_{3}}-\Delta {{H}_{1}}-\Delta {{H}_{2}}\] done
clear
B)
\[\Delta {{H}_{\text{soln}}}=\Delta {{H}_{1}}+\Delta {{H}_{2}}+\Delta {{H}_{3}}\] done
clear
C)
\[\Delta {{H}_{\text{soln}}}=\Delta {{H}_{1}}+\Delta {{H}_{2}}-\Delta {{H}_{3}}\] done
clear
D)
\[\Delta {{H}_{\text{soln}}}=\Delta {{H}_{1}}-\Delta {{H}_{2}}-\Delta {{H}_{3}}\] done
clear
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question_answer5)
Which of the following liquid pairs shows a positive deviation from Raoult's law?
A)
Water - Nitric acid done
clear
B)
Benzene - Methanol done
clear
C)
Water-Hydrochloric acid done
clear
D)
Acetone - Chloroform done
clear
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question_answer6)
Which will form maximum boiling point azeotrope?
A)
\[HN{{O}_{3}}+{{H}_{2}}O\] solution done
clear
B)
\[{{C}_{2}}{{H}_{5}}OH+{{H}_{2}}O\] solution done
clear
C)
\[{{C}_{6}}{{H}_{6}}+{{C}_{6}}{{H}_{5}}C{{H}_{3}}\] solution done
clear
D)
None of these done
clear
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question_answer7)
A solution of acetone in ethanol
A)
shows a positive deviation from Raoult's law done
clear
B)
behaves like a non ideal solution done
clear
C)
obeys Raoult's law done
clear
D)
shows a negative deviation from Raoult's law done
clear
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question_answer8)
An aqueous solution is 1.00 molal in KI. Which change will cause the vapour pressure of the solution to increase?
A)
Addition of \[NaCl\] done
clear
B)
Addition of \[N{{a}_{2}}S{{O}_{4}}\] done
clear
C)
Addition of 1.00 molal KI done
clear
D)
Addition of water done
clear
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question_answer9)
A binary liquid solution is prepared by mixing n-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution?
A)
The solution is non-ideal, showing -ve deviation from Raoult's Law. done
clear
B)
The solution is non-ideal, showing +ve deviation from Raoult's Law. done
clear
C)
n-heptane shows +ve deviation while ethanol shows -ve deviation from Raoult's Law. done
clear
D)
The solution formed is an ideal solution. done
clear
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question_answer10)
\[{{P}_{A}}\]and \[{{P}_{B}}\] are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution. If \[{{X}_{A}}\]represents the mole fraction of component A, the total pressure of the solution will be.
A)
\[{{P}_{A}}+{{X}_{A}}({{P}_{B}}-{{P}_{A}})\] done
clear
B)
\[{{P}_{A}}+{{X}_{A}}({{P}_{A}}-{{P}_{B}})\] done
clear
C)
\[{{P}_{B}}+{{X}_{A}}({{P}_{B}}-{{P}_{A}})\] done
clear
D)
\[{{P}_{B}}+{{X}_{A}}({{P}_{A}}-{{P}_{B}})\] done
clear
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question_answer11)
Vapour pressure of chloroform \[(CHC{{l}_{3}})\] and dichloromethane \[(C{{H}_{2}}C{{l}_{2}})\] at \[25{}^\circ \]C are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of \[CHC{{l}_{3}}\] and 40 g of\[C{{H}_{2}}C{{l}_{2}}\] at the same temperature will be: (Molecular mass of \[CHC{{l}_{3}}=119.5u\] and molecular mass of \[C{{H}_{2}}C{{l}_{2}}=85u\]).
A)
90.92 mm Hg done
clear
B)
115.0 mm Hg done
clear
C)
147.9 mm Hg done
clear
D)
285.5 mm Hg done
clear
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question_answer12)
The vapour pressure of a solution of the liquids A (\[P{}^\circ =80\] mm Hg and \[{{x}_{A}}=0.4\]) and B (\[P{}^\circ =120\] mm Hg and \[{{X}_{B}}=0.6\]) is found to be \[100mm\]Hg. It shows that the solution exhibits
A)
positive deviation from ideal behaviour done
clear
B)
negative deviation from ideal behaviour done
clear
C)
ideal behaviour done
clear
D)
positive deviation for lower cone. and negative for higher cone. done
clear
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question_answer13)
Vapour pressure (in torr) of an ideal solution of two liquids A and B is given by: \[P=52{{X}_{A}}+114\] where \[{{X}_{A}}\] is the mole fraction of A in the mixture. The vapour pressure (in torr) of equimolar mixture of the two liquids will be:
A)
166 done
clear
B)
83 done
clear
C)
140 done
clear
D)
280 done
clear
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question_answer14)
The vapour pressure (at the standard boiling point of water) of an aqueous solution containing 28% by mass of a non-volatile normal solute (molecular mass = 28) will be
A)
152 torr done
clear
B)
608 torr done
clear
C)
760 torr done
clear
D)
547 torr done
clear
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question_answer15)
Lowering of vapour pressure of 1.00 m solution of a non-volatile solute in a hypothetical solvent of molar mass 40 g at its normal boiling point, is:
A)
29.23 torr done
clear
B)
30.4 torr done
clear
C)
35.00 torr done
clear
D)
40.00 torr done
clear
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question_answer16)
Equal masses of a solute are dissolved in equal amount of two solvents A and B, respective molecular masses being \[{{M}_{A}}\] and \[{{M}_{B}}\]. The relative lowering of vapour pressure of solution in solvent A is twice that of the solution in solvent B. If the solutions are dilute, \[{{M}_{A}}\] and \[{{M}_{B}}\] are related as
A)
\[{{M}_{A}}={{M}_{B}}\] done
clear
B)
\[2{{M}_{A}}={{M}_{B}}\] done
clear
C)
\[{{M}_{A}}=2{{M}_{B}}\] done
clear
D)
\[{{M}_{A}}=4{{M}_{B}}\] done
clear
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question_answer17)
At \[20{}^\circ C\] and 1.00 atm partial pressure of \[{{H}_{2}}\], 18 mL of \[{{H}_{2}}\](STP) dissolves in 1 L of water. If 2 L of water is exposed to a gaseous mixture having a total pressure of 1425 ton- (excluding the vapour pressure of water) and containing 80% \[{{H}_{2}}\] by volume, the volume of \[{{H}_{2}}\](STP) dissolved is
A)
27 mL done
clear
B)
54 mL done
clear
C)
33.75 mL done
clear
D)
67.50 mL done
clear
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question_answer18)
At a particular temperature, the vapour pressures of two liquids A and B are respectively 120 and 180 mm of mercury If 2 moles of A and 3 moles of B are mixed to form an ideal solution, the vapour pressure of the solution at the same temperature will be (in mm of mercury)
A)
156 done
clear
B)
145 done
clear
C)
150 done
clear
D)
108 done
clear
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question_answer19)
Which one of the following gases has the lowest value of Henry's law constant?
A)
\[{{N}_{2}}\] done
clear
B)
He done
clear
C)
\[{{H}_{2}}\] done
clear
D)
\[C{{O}_{2}}\] done
clear
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question_answer20)
Which one of the following binary mixtures forms an azeotrope with minimum boiling point type?
A)
acetone-ethanol done
clear
B)
\[{{H}_{2}}O-HN{{O}_{3}}\] done
clear
C)
benzene-toluene done
clear
D)
n-hexane-n-heptane done
clear
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question_answer21)
The vapour pressure of pure benzene and toluene at a particular temperature are 100 mm and 50 mm respectively. Then the mole fraction of benzene in vapour phase in contact with equimolar solution of benzene and toluene is
A)
0.67 done
clear
B)
0.75 done
clear
C)
0.33 done
clear
D)
0.50 done
clear
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question_answer22)
12 g of urea is dissolved in 1 litre of water and 68.4 g of sucrose is dissolved in 1 litre of water. The lowering of vapour pressure of first case is
A)
equal to second done
clear
B)
greater than second done
clear
C)
less than second done
clear
D)
double that of second done
clear
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question_answer23)
Which of the following statement is correct if the intermolecular forces in liquids A, B and C are in the order A<B<C ?
A)
B evaporates more readily than A done
clear
B)
B evaporates less readily than C done
clear
C)
A and B evaporates at the same rate done
clear
D)
A evaporates more readily than C done
clear
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question_answer24)
At \[80{}^\circ C\], the vapour pressure of pure liquid 'A' is 520 mm Hg and that of pure liquid 'B' is 1000 mm Hg. If a mixture solution of 'A' and 'B' boils at \[80{}^\circ C\] and 1 atm pressure, the amount of 'A' in the mixture is (1 atm = 760 mm Hg)
A)
52 mol percent done
clear
B)
34 mol percent done
clear
C)
48 mol percent done
clear
D)
50 mol percent done
clear
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question_answer25)
A solution at \[20{}^\circ C\] is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr, respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively:
A)
35.8 torr and 0.280 done
clear
B)
38.0 torr and 0.589 done
clear
C)
30.5 torr and 0.389 done
clear
D)
30.5 torr and 0.480 done
clear
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question_answer26)
Choose the correct statement with respect to the vapour pressure of a liquid among the following:
A)
Increases linearly with increasing temperature done
clear
B)
Increases non-linearly with increasing temperature done
clear
C)
Decreases linearly with increasing temperature done
clear
D)
Decreases non-linearly with increasing temperature done
clear
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question_answer27)
For an ideal solution of two components A and B, which of the following is true?
A)
\[\Delta {{H}_{mixing}}<0(zero)\] done
clear
B)
\[\Delta {{H}_{mixing}}>0(zero)\] done
clear
C)
A - B interaction is stronger than A - A and B - B interactions done
clear
D)
A- A, B - B and A - B interactions are identical. done
clear
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question_answer28)
Vapour pressure of pure benzene is 119 torr and that of toluene is 37.0 torr at the same temperature. Mole fraction of toluene in vapour phase which is in equilibrium with a solution of benzene and toluene having a mole fraction of toluene 0.50, will be:
A)
0.137 done
clear
B)
0.237 done
clear
C)
0.435 done
clear
D)
0.205 done
clear
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question_answer29)
How many grams of methyl alcohol should be added to 10 litre tank of water to prevent its freezing at 268K? (\[{{K}_{f}}\]for water is \[1.86Kkgmo{{l}^{-1}}\])
A)
880.07 g done
clear
B)
899.04 g done
clear
C)
886.02 g done
clear
D)
868.06 g done
clear
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question_answer30)
Henry's law constant K of \[C{{O}_{2}}\] in water at \[25{}^\circ C\] is \[3.0\times {{10}^{-2}}mol\,{{L}^{-1}}at{{m}^{-1}}\]. The mass of \[C{{O}_{2}}\] present in 100 L of soft drink bottled with a partial pressure of \[C{{O}_{2}}\] of 4 atm at the same temperature is
A)
5.28 g done
clear
B)
12.0 g done
clear
C)
428 g done
clear
D)
528 g done
clear
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question_answer31)
Vapour pressure of solution containing 2 mol of liquid \[A(P_{A}^{0}=80torr)\]and 3 mol of liquid \[B(P_{B}^{0}=100torr)\]is 87 torr. We can conclude that
A)
there is negative deviation from Raoult's law done
clear
B)
boiling point is higher than that expected for ideal solution done
clear
C)
molecular attractions between unlike molecules are stronger than those between like molecules done
clear
D)
All of these statements are correct done
clear
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question_answer32)
At \[15{}^\circ C\] and 1 atmosphere partial pressure of hydrogen, 20 mL of hydrogen measured at STP dissolves in 1 L of water. If water at \[15{}^\circ C\] is exposed to a gaseous mixture having a total pressure of 1500 mm of Hg (excluding the vapour pressure of water) and containing 80% hydrogen by volumne, then the volume of hydrogen measured at STP that will dissolve in 1 L of water is
A)
20.0 mL done
clear
B)
31.6 mL done
clear
C)
36.1 mL done
clear
D)
26.3 mL done
clear
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question_answer33)
The vapour pressure of two pure liquids A and B that form an ideal solution, are 400 and 800 mm of Hg respectively at a temperature \[t{}^\circ C.\] The mole fraction of A in a solution of A and B whose boiling point is \[t{}^\circ C.\] will be
A)
0.4 done
clear
B)
0.8 done
clear
C)
0.1 done
clear
D)
0.2 done
clear
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question_answer34)
The total vapour pressure of a 4 mole % solution of \[N{{H}_{3}}\] in water at 293 K is 50.0 torr. The vapour pressure of pure water is 17.0 torr at this temperature. Applying Henry's and Raoult's laws, the total vapour pressure for a 5 mole % solution is
A)
58.25 torr done
clear
B)
33 torr done
clear
C)
42.1 torr done
clear
D)
52.25 torr done
clear
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question_answer35)
Which one of the following aqueous solutions will exihibit highest boiling point?
A)
0.015 M urea done
clear
B)
0.01 M K \[N{{O}_{3}}\] done
clear
C)
\[0.01M\,N{{a}_{2}}S{{O}_{4}}\] done
clear
D)
0.015 M glucose done
clear
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question_answer36)
The elevation in boiling point of a solution of 13.44 g of \[CuC{{l}_{2}}\] in 1 kg of water using the following information will be (Molecular weight of \[CuC{{l}_{2}}=134.4g\] and\[{{K}_{b}}=0.52\,Kkg\,mo{{l}^{-1}}\])
A)
0.16 done
clear
B)
0.05 done
clear
C)
0.1 done
clear
D)
0.2 done
clear
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question_answer37)
The temperature at which 10% aqueous solution (w/v) of glucose will exhibit the osmotic pressure of 14 bar is -
A)
\[307.3{}^\circ C\] done
clear
B)
307.3 K done
clear
C)
34 K done
clear
D)
\[-34{}^\circ C\] done
clear
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question_answer38)
KBr is 80% ionized in solution. The freezing point of 0.4 molal solution of KBr is: \[{{K}_{f}}({{H}_{2}}O)=1.86K\text{ }kg/mole\]
A)
274.339K done
clear
B)
\[-1.339K\] done
clear
C)
257.3 K done
clear
D)
\[-1.339{}^\circ C\] done
clear
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question_answer39)
A solution of urea (mol. mass\[56g\text{ }mo{{l}^{-1}}\]) boils at \[100.18{}^\circ C\] at the atmospheric pressure. If \[{{K}_{f}}\] and \[{{K}_{b}}\] for water are 1.86 and \[0.512K\text{ }kg\text{ }mo{{l}^{-1}}\] respectively, the above solution will freeze at
A)
\[0.654\text{ }{}^\circ C\] done
clear
B)
\[-0.654\text{ }{}^\circ C\] done
clear
C)
\[6.54\text{ }{}^\circ C\] done
clear
D)
\[-6.54{}^\circ C\] done
clear
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question_answer40)
The solution containing 4.0 g of a polyvinyl chloride polymer in 1 litre of dioxane was found to have an osmotic pressure \[6.0\times {{10}^{-4}}\] atmosphere at 300K, the value of R used is 0.082 litre atmosphere \[mol{{e}^{-1}}{{K}^{-1}}\]. The molecular mass of the polymer was found to be
A)
\[3.0\times {{10}^{2}}\] done
clear
B)
\[1.6\times {{10}^{5}}\] done
clear
C)
\[5.6\times {{10}^{4}}\] done
clear
D)
\[6.4\times {{10}^{2}}\] done
clear
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question_answer41)
If the various terms in the given below expressions have usual meanings, the van't Hoff factor (i) cannot be calculated by which one of the following expressions
A)
\[\pi V=\sqrt{in}RT\] done
clear
B)
\[\Delta {{T}_{f}}=i{{K}_{f}}.m\] done
clear
C)
\[\Delta {{T}_{b}}=i{{K}_{b}}.m\] done
clear
D)
\[\frac{P_{solvent}^{0}-{{P}_{solution}}}{P_{solvent}^{0}}=i\left( \frac{n}{N+n} \right)\] done
clear
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question_answer42)
A 0.001 molal solution of\[[Pt{{(N{{H}_{3}})}_{4}}C{{l}_{4}}]\] in water had a freezing point depression of\[0.0054{}^\circ C\]. If \[{{K}_{f}}\] for water is 1.80, the correct formulation for the above molecule is
A)
\[[Pt{{(N{{H}_{3}})}_{4}}C{{l}_{3}}]Cl\] done
clear
B)
\[[Pt{{(N{{H}_{3}})}_{4}}C{{l}_{2}}]C{{l}_{2}}\] done
clear
C)
\[[Pt{{(N{{H}_{3}})}_{4}}Cl]C{{l}_{3}}\] done
clear
D)
\[[Pt{{(N{{H}_{3}})}_{4}}C{{l}_{4}}]\] done
clear
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question_answer43)
Which of the following has the lowest freezing point?
A)
0.1 m sucrose done
clear
B)
0.1 m urea done
clear
C)
0.1 m ethanol done
clear
D)
0.1 m glucose done
clear
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question_answer44)
The van't Hoff factor i for a compound which association in other solvent is respectively:
A)
less than one and greater than one. done
clear
B)
less than one and less than one. done
clear
C)
greater than one and less than one. done
clear
D)
greater than one and greater than one. done
clear
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question_answer45)
If 0.1 M solution of glucose and 0.1 M solution semipermeable membrane to equal heights, then it will be correct to say that
A)
there will be no net movement across the membrane done
clear
B)
glucose will flow towards urea solution done
clear
C)
urea will flow towards glucose solution done
clear
D)
water will flow from urea solution to glucose done
clear
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question_answer46)
Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by:
A)
Partial ionization done
clear
B)
Dissociation done
clear
C)
Complex formation done
clear
D)
Association done
clear
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question_answer47)
The observed osmotic pressure for a 0.10 M solution of \[Fe{{(N{{H}_{4}})}_{2}}{{(S{{O}_{4}})}_{2}}\,at\,25{}^\circ C\] is 10.8 atm. The experimental (observed) value of van't Hoff factor will be: \[\left( R=0.082\text{ }L\text{ }atm\text{ }{{k}^{-1}}mo{{l}^{-1}} \right)\]
A)
4.42 done
clear
B)
4.00 done
clear
C)
3.42 done
clear
D)
5.42 done
clear
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question_answer48)
12 g of a nonvolatile solute dissolved in 108 g of water produces the relative lowering of vapour pressure of 0.1. The molecular mass of the solute is:
A)
80 done
clear
B)
60 done
clear
C)
20 done
clear
D)
40 done
clear
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question_answer49)
A molecule M associates in a given solvent according to the equation \[M\rightleftharpoons {{(M)}_{n}}\]. For a certain concentration of M, the van't Hoff factor was found to be 0.9 and the fraction of associated molecules was 0.2. The value of n is:
A)
3 done
clear
B)
5 done
clear
C)
2 done
clear
D)
4 done
clear
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question_answer50)
A solution containing 0.85 g of \[ZnC{{l}_{2}}\] in 125.0 g of water freezes at \[-0.23{}^\circ C\]. The apparent degree of dissociation of the salt is (\[{{K}_{f}}\] for water\[=1.86K\text{ }kg\text{ }mo{{l}^{-1}}\], atomic mass: Zn = 65.3 and Cl = 35.5)
A)
1.36% done
clear
B)
73.5% done
clear
C)
7.35% done
clear
D)
2.47% done
clear
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question_answer51)
0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If \[{{K}_{f}}\] for water is\[1.86K\text{ }kg\text{ }mo{{l}^{-1}}\], the
A)
0.56K done
clear
B)
1.12K done
clear
C)
\[-0.56K\] done
clear
D)
\[-1.12K\] done
clear
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question_answer52)
200 mL of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at 300 K is found to be \[2.57\times {{10}^{-3}}\] bar. The molar mass of protein will be (R = 0.083 L bar \[mo{{l}^{-1}}{{K}^{-1}}\])
A)
\[51022g\text{ }mo{{l}^{-1}}\] done
clear
B)
\[122044g\text{ }mo{{l}^{-1}}\] done
clear
C)
\[31011g\,mo{{l}^{-1}}\] done
clear
D)
\[61038g\,mo{{l}^{-1}}\] done
clear
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question_answer53)
Freezing point of an aqueous solution is\[\left( -0.186 \right){}^\circ C\]. Elevation of boiling point of the same solution is\[{{K}_{b}}=0.512{}^\circ C,K{{ }_{f}}=1.86{}^\circ C\], find the increase in boiling point.
A)
\[0.186{}^\circ C\] done
clear
B)
\[0.0512{}^\circ C\] done
clear
C)
\[0.092{}^\circ C\] done
clear
D)
\[0.2372{}^\circ C\] done
clear
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question_answer54)
The relationship between osmotic pressure at 273 K when 10g glucose \[\left( {{P}_{1}} \right)\], 10g urea \[\left( {{P}_{2}} \right)\], and 10 g sucrose \[\left( {{P}_{3}} \right)\] are dissolved in 250 mL of water is
A)
\[{{P}_{1}}>{{P}_{2}}>{{P}_{3}}\] done
clear
B)
\[{{P}_{3}}>{{P}_{1}}>{{P}_{3}}\] done
clear
C)
\[{{P}_{2}}>{{P}_{1}}>{{P}_{3}}\] done
clear
D)
\[{{P}_{2}}>{{P}_{3}}>{{P}_{1}}\] done
clear
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question_answer55)
Which observation(s) reflect(s) colligative properties?
(i) A 0.5 m \[NaBr\] solution has a higher vapour pressure than a 0.5 m \[BaC{{l}_{2}}\]solution at the same temperature |
(ii) Pure water freezes at the higher temperature than pure methanol |
(iii) A 0.1 m \[NaOH\]solution freezes at a lower temperature than pure water |
Choose the correct answer from the codes given below |
A)
(i), (ii) and (iii) done
clear
B)
(i) and (ii) done
clear
C)
(ii) and (iii) done
clear
D)
(i) and (iiii) done
clear
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question_answer56)
The difference between the boiling point and freezing point of an aqueous solution containing sucrose (molecular \[wt=342g\text{ }mol{{e}^{-1}}\]) in 100 g of water is \[105{}^\circ C\]. If \[{{K}_{f}}\] and \[{{K}_{b}}\] of water are 1.86 and \[0.51K\text{ }kg\text{ }mo{{l}^{-1}}\] respectively, the weight of sucrose in the solution is about
A)
34.2 g done
clear
B)
342 g done
clear
C)
7.2 g done
clear
D)
72 g done
clear
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question_answer57)
A solution containing 1.8 g of a compound (empirical formula \[C{{H}_{2}}O\]) in 40 g of water is observed to freeze at \[-0.465{}^\circ C\]. The molecular formula of the compound is (\[{{K}_{f}}\] of water \[=1.86kg\text{ }K\text{ }mo{{l}^{-1}}\])
A)
\[{{C}_{2}}{{H}_{4}}{{O}_{2}}\] done
clear
B)
\[{{C}_{3}}{{H}_{6}}{{O}_{3}}\] done
clear
C)
\[{{C}_{4}}{{H}_{8}}{{O}_{4}}\] done
clear
D)
\[{{C}_{6}}{{H}_{12}}{{O}_{6}}\] done
clear
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question_answer58)
Freezing point of an aqueous solution is \[-0.186{}^\circ C.\] If the values of \[{{K}_{b}}\] and \[{{K}_{f}}\] of water are respectively \[0.52K\text{ }kg\text{ }mo{{l}^{-1}}\] and \[1.86K\text{ }kg\text{ }mo{{l}^{-1}}\], then the elevation of boiling point of the solution in K is
A)
0.52 done
clear
B)
1.04 done
clear
C)
1.34 done
clear
D)
0.052 done
clear
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question_answer59)
If the elevation in boiling point of a solution of 10 g of solute (mol. wt.= 100) in 100g of water is \[\Delta {{T}_{b}}\] the ebullioscopic constant of water is
A)
10 done
clear
B)
\[10\Delta {{T}_{b}}\] done
clear
C)
\[\Delta {{T}_{b}}\] done
clear
D)
\[\frac{\Delta {{T}_{b}}}{10}\] done
clear
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question_answer60)
Which one of the following statements is incorrect?
A)
The correct order of osmotic pressure for 0.01 M aqueous solution of each compound is \[BaC{{l}_{2}}>KCl>C{{H}_{3}}COOH>Sucrose\] done
clear
B)
The osmotic pressure \[\left( \pi \right)\] of a solution is given by the equation \[\pi =MRT\], where M is the molarity of the solution done
clear
C)
Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction done
clear
D)
Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression done
clear
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question_answer61)
\[{{\pi }_{1}},{{\pi }_{2}},{{\pi }_{3}}\] and \[{{\pi }_{4}}\] atm are the osmotic pressures of 5% (mass/volume) solutions of urea, fructose, sucrose and \[KCl\] respectively at certain temperature. The correct order of their magnitudes is:
A)
\[{{\pi }_{1}}>{{\pi }_{4}}>{{\pi }_{2}}>{{\pi }_{3}}\] done
clear
B)
\[{{\pi }_{1}}>{{\pi }_{4}}>{{\pi }_{2}}>{{\pi }_{3}}\] done
clear
C)
\[{{\pi }_{4}}>{{\pi }_{1}}>{{\pi }_{2}}>{{\pi }_{3}}\] done
clear
D)
\[{{\pi }_{4}}>{{\pi }_{1}}>{{\pi }_{3}}>{{\pi }_{2}}\] done
clear
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question_answer62)
Which of the following has been arranged in the increasing order of freezing point?
A)
\[0.025MKN{{O}_{3}}<0.1MN{{H}_{2}}CSN{{H}_{2}}\] \[<0.05M\,BaC{{l}_{2}}<0.1MNaCl\] done
clear
B)
\[0.1M\,NaCl<0.05M\,BaC{{l}_{2}}\] \[<0.1M\,N{{H}_{2}}CSN{{H}_{2}}<0.025M\,KN{{O}_{3}}\] done
clear
C)
\[0.1M\,N{{H}_{2}}CSN{{H}_{2}}<0.1M\,NaCl\] \[<0.05M\,BaC{{l}_{2}}<0.025M\,KN{{O}_{3}}\] done
clear
D)
\[0.025M\,KN{{O}_{3}}<0.05M\,BaC{{l}_{2}}\] \[<0.1M\,NaCl<0.1M\,N{{H}_{2}}CSN{{H}_{2}}\] done
clear
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question_answer63)
0.010M solution an acid HA freezes at \[-0.0205{}^\circ C\]. If\[~{{K}_{f}}\] for water is \[1.860K\text{ }kg\text{ }mo{{l}^{-1}}\], the ionization constant of the conjugate base of the acid will be (assume \[0.010M=0.010m\])
A)
\[1.1\times {{10}^{-4}}\] done
clear
B)
\[1.1\times {{10}^{-3}}\] done
clear
C)
\[9.0\times {{10}^{-11}}\] done
clear
D)
\[9.0\times {{10}^{-12}}\] done
clear
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question_answer64)
1.0 M aqueous solution of \[CrC{{l}_{3}}.6{{H}_{2}}O\] freezes at \[-5.58{}^\circ C\]. Assuming complete ionization of the hydrated complex, which of the following isomers conforms to the observation (\[{{K}_{f}}\] for water \[=1.86K\,kg\,mo{{l}^{-1}}\])?
A)
\[[Cr{{\left( {{H}_{2}}O \right)}_{3}}C{{l}_{3}}].3{{H}_{2}}O\] done
clear
B)
\[[Cr{{\left( {{H}_{2}}O \right)}_{4}}C{{l}_{4}}]Cl.2{{H}_{2}}O\] done
clear
C)
\[[Cr{{\left( {{H}_{2}}O \right)}_{5}}Cl]C{{l}_{2}}.{{H}_{2}}O\] done
clear
D)
\[[Cr{{\left( {{H}_{2}}O \right)}_{6}}]C{{l}_{3}}\] done
clear
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question_answer65)
Assuming degree of ionization to be unity in each case, which of the following equimolal solutions would freeze at the lowest temperature?
A)
\[[Pt{{(N{{H}_{3}})}_{6}}]C{{l}_{4}}\] done
clear
B)
\[[Pt{{(N{{H}_{3}})}_{5}}Cl]C{{l}_{3}}\] done
clear
C)
\[[Pt{{(N{{H}_{3}})}_{4}}C{{l}_{2}}]C{{l}_{2}}\] done
clear
D)
\[[Pt{{(N{{H}_{3}})}_{3}}C{{l}_{3}}]Cl\] done
clear
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question_answer66)
Which of the following aqueous solutions should have the highest osmotic pressure?
A)
\[0.011\,M\,AlC{{l}_{3}}\,\text{at}\,50{}^\circ C\] done
clear
B)
\[0.03\text{ }M\text{ }NaCl\text{ at}\,\,25{}^\circ C\] done
clear
C)
\[0.012M{{\left( N{{H}_{4}} \right)}_{2}}S{{O}_{4}}\,\,\text{at}\,\,25{}^\circ C\] done
clear
D)
\[0.03\text{ }M\text{ }NaCl\,\text{at }50{}^\circ C\] done
clear
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question_answer67)
At 760 torr pressure and \[20{}^\circ C\]temperature, 1 L of water dissolves 0.04 gm of pure oxygen or 0.02 gm of pure nitrogen. Assuming that dry air is composed of 20% oxygen and 80% nitrogen (by volume), the masses (in g/L) of oxygen and nitrogen dissolved by 1 L of water at \[20{}^\circ C\]exposed to air at a total pressure of 760 torr are respectively:
A)
0.008, 0.016 done
clear
B)
0.016, 0.008 done
clear
C)
0.16, 0.08 done
clear
D)
0.04, 0.02 done
clear
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question_answer68)
If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water \[\left( \Delta {{T}_{f}} \right),\] when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is \[\left( {{K}_{f}}=1.86K\text{ }kg\text{ }mo{{l}^{-1}} \right)\]
A)
0.372 K done
clear
B)
0.0558 K done
clear
C)
0.0744 K done
clear
D)
0.0186 K done
clear
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question_answer69)
The osmotic pressure (at \[27{}^\circ C\]) of an aqueous solution (200mL) containing 6g of a protein is \[2\times {{10}^{-3}}\] atm. If R= 0.080 L atm\[mo{{l}^{-1}}{{K}^{-1}}\], the molecular weight of protein is
A)
\[7.2\times {{10}^{5}}\] done
clear
B)
\[3.6\times {{10}^{5}}\] done
clear
C)
\[1.8\times {{10}^{5}}\] done
clear
D)
\[1.0\times {{10}^{5}}\] done
clear
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question_answer70)
At temperature \[327{}^\circ C\] and concentration C, osmotic pressure of a solution is P, the same solution at concentration C/2 and at temperature \[427{}^\circ C\] shows osmotic pressure of 2 atm, value of P will be
A)
\[\frac{12}{7}\] done
clear
B)
\[\frac{24}{7}\] done
clear
C)
\[\frac{6}{5}\] done
clear
D)
\[\frac{5}{6}\] done
clear
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question_answer71)
In countries nearer to polar region, the roads are sprinkled with\[CaC{{l}_{2}}\]. This is
A)
to minimise the snow present on roads done
clear
B)
to minimise pollution done
clear
C)
to minimise the accumulation of dust on the road done
clear
D)
to minimise the wear and tear of the roads done
clear
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question_answer72)
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
A)
\[1+\alpha \] done
clear
B)
\[1-\alpha \] done
clear
C)
\[1+2\alpha \] done
clear
D)
\[1-2\alpha \] done
clear
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question_answer73)
Which has the minimum freezing point?
A)
One molal NaCl aq. Solution done
clear
B)
One molal \[CaC{{l}_{2}}\]aq. Solution done
clear
C)
One molal KCl aq. Solution done
clear
D)
One molal urea aq. solution done
clear
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question_answer74)
On mixing 3 g of non - volatile solute in 200 mL of water, its boiling point \[\left( 100{}^\circ \right)\] becomes \[100.52{}^\circ C.\] If \[{{K}_{b}}\] for water is 0.6 K/m then molecular wt. of solute is:
A)
\[10.5g\,\,mo{{l}^{-1}}\] done
clear
B)
\[12.6g\,\,mo{{l}^{-1}}\] done
clear
C)
\[15.7\,g\,\,mo{{l}^{-1}}\] done
clear
D)
\[17.3\,g\,\,mo{{l}^{-1}}\] done
clear
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question_answer75)
Benzene freezes at \[5.50{}^\circ C\]. If the freezing point of 2.48 g of phosphorous in 100 g benzene is \[4.48{}^\circ C\], the atomicity of phosphorus in benzene is (\[{{K}_{f}}\](benzene)\[=5.12\,K\,kgmo{{l}^{-1}}\]):
A)
1 done
clear
B)
3 done
clear
C)
4 done
clear
D)
8 done
clear
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question_answer76)
A solute X has a solubility of 10.0 g in 100 g of water at \[25{}^\circ C.\] If a solution containing 4.0 g of solute in 50 g of water is subjected to evaporation at constant temperature of\[25{}^\circ C\], the osmotic pressure of the solution
A)
remains unchanged throughout done
clear
B)
increases continuously done
clear
C)
increases to constant value done
clear
D)
decreases to constant value done
clear
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question_answer77)
At\[17{}^\circ C\], the osmotic pressure of sugar solution is 580 torr. The solution is diluted and the temperature is raised to \[57{}^\circ C,\] when the osmotic pressure is found to be 165 torr. The extent of dilution is:
A)
2 times done
clear
B)
3 times done
clear
C)
4 times done
clear
D)
5 times done
clear
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question_answer78)
Which of the following terms has units of temperature?
\[I:{{K}_{f}}\] \[II:m{{K}_{f}}\] \[III:i{{K}_{f}}\] \[IV:\frac{m{{K}_{f}}}{i}\] |
A)
I, II done
clear
B)
I, III done
clear
C)
II, III done
clear
D)
II, IV done
clear
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question_answer79)
0.5 m solution of a complex of iron and cyanide ions has the depression of f.pt. to be 3.72 K (\[{{K}_{f}}\] For water \[=1.86\text{ }Kmola{{l}^{-1}}\]). The formula of the complex is:
A)
\[{{K}_{4}}[Fe{{(CN)}_{6}}]\] done
clear
B)
\[{{K}_{2}}[Fe{{(CN)}_{4}}]\] done
clear
C)
\[{{K}_{3}}[Fe{{(CN)}_{6}}]\] done
clear
D)
\[Fe{{\left( CN \right)}_{4}}\] done
clear
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question_answer80)
A living cell contains a solution which is isotonic with 0.2 M glucose solution. What osmotic pressure develops when the cell is placed in \[0.05M\text{ }BaC{{l}_{2}}\] solution at 300 K?
A)
1.23 atm done
clear
B)
3.69 atm done
clear
C)
6.15 atm done
clear
D)
None of these done
clear
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