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question_answer1) 1000 gm of 1 m sucrose solution in water is cooled to\[-3.534{}^\circ C\] . What weight of ice would be separated out at this temperature? \[{{K}_{f}}({{H}_{2}}O)=1.86K\,mole\,kg\].
question_answer2) The freezing point of an 0.08 (m) \[NaHS{{O}_{4}}\] is\[-0.345{}^\circ C\]. Calculate the percentage of \[HSO_{4}^{-}ions\] that transfer a proton to water to form\[SO_{4}^{2-}ion\]. \[{{K}_{f}}\left( {{H}_{2}}O \right)=1.86mo{{l}^{-1}}kg\]
question_answer3) At \[10{}^\circ C\], the osmotic pressure of urea solution is 500 mm. The solution is diluted and the temperature is raised to \[25{}^\circ C\] , when the osmotic pressure is found to be 105.3 mm. Determine extent of dilution \[\left( {{V}_{2}}/{{V}_{1}} \right)\]?
question_answer4) Phenol associates in benzene to a certain extent to form a dimer. A solution containing \[20\times {{10}^{-3}}kg\] of phenol in 1.0 kg of benzene has its freezing point depressed by 0.69 K. Calculate the fraction of phenol that has dimerised. (\[{{K}_{f}}\] for benzene \[=5.12K\,kg\,mo{{l}^{-1}}\] )
question_answer5) An organic liquid, A, is immiscible with water. When boiled together with water, the boiling point is \[90{}^\circ C\] at which the partial vapour pressure of water is 526 mm Hg. The atmospheric pressure is 736 mm Hg. The weight ratio of the liquid and water collected is 2.5:1. What is the molecular weight of the liquid?
question_answer6) A current of dry air is passed through a bulb containing 5 g of a solute in 100 g of water and then through water alone. The losses in weight of the solution and pure water were respectively 0.78 g and 0.02 g. Calculate: (a) relative lowering of vapour pressure
question_answer7) If boiling point of an aqueous solution is \[100.1{}^\circ C\]. What is its freezing point? \[{{K}_{f}}\] for\[{{H}_{2}}O=1.86\]\[K\,kg/mol\], \[{{K}_{b}}=0.513K\,kg/mol\] .
question_answer8) 1.5 g of a monobasic acid when dissolved in 150g of water lowers the freezing point by \[0.165{}^\circ C\]. 0.5 g of the same acid when titrated, after dissolution in water, requires 37.5 ml of N/10 alkali. Calculate the degree of dissociation of the acid (\[{{K}_{f}}\] for water\[=1.86{}^\circ Cmo{{l}^{-1}}\] .)
question_answer9) Sea water is found to contain 5.85% \[NaCl\] and 9.50% \[MgC{{l}_{2}}\] be weight of solution. Calculate its normal boiling point assuming 80% ionisation for \[NaCl\] and 50% ionisation of \[MgC{{l}_{2}}\] \[\left[ {{K}_{b}}\left( {{H}_{2}}O \right)=0.51kg\,mol{{e}^{-1}}K \right]\].
question_answer10) Calculate the boiling point of a solution containing 0.61 g of benzoic acid in 50g of carbon disulphide assuming 84% dimerization of the acid. The boiling point and \[{{K}_{b}}\] of \[C{{S}_{2}}\] are \[46.2{}^\circ C\] and \[2.3K\,kg\,mo{{l}^{-1}}\] , respectively.
question_answer11) A decimolar solution of potassium ferrocyanide \[{{K}_{4}}\left[ Fe{{\left( CN \right)}_{6}} \right]\] is 50% dissociated at 300K. Calculate the osmotic pressure of the solution. \[\left( R=8.314J{{K}^{-1}}mo{{l}^{-1}} \right)\] . Give your answer as a multiple of \[{{10}^{-5}}\].
question_answer12) 29.2% (w/w) HCl stock solution has a density of \[1.25\,g\,m{{L}^{-1}}\] . The molecular weight of HCl is \[36.5\,g\,mo{{l}^{-1}}\] . The volume (mL) of stock solution required to prepare a 200 mL solution of 0.4 M HCl is.
question_answer13) \[M{{X}_{2}}\] dissociates into \[{{M}^{2+}}\] and \[{{X}^{-}}ions\] in an aqueous solution, with a degree of dissociation \[\left( \alpha \right)\] of 0.5. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is
question_answer14) A compound \[{{H}_{2}}X\] with molar weight of 80 g is dissolved in a solvent having density of \[0.4\,g\,m{{l}^{-1}}.\] Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution is
question_answer15) The mole fraction of a solute in a solution is 0.1. At 298 K, molarity of this solution is the same as its molality. Density of this solution at 298 K is\[2.0\,g\,c{{m}^{-3}}\]. The ratio of the molecular weights of the solute and solvent \[\left( \frac{M{{W}_{solute}}}{M{{W}_{solvent}}} \right)\], is
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