NEET Chemistry Solutions / विलयन Question Bank

done Self Evaluation Test - Solutions Total Questions - 80

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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
  View Solution play_arrow

• 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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