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MCQ for Full Syllabus Chemistry Solutions
Full Syllabus Chemistry students should refer to the following multiple-choice questions with answers for Solutions in Full Syllabus.
Solutions MCQ Questions Full Syllabus Chemistry with Answers
Question: Osmotic pressure of solution containing 0.6 g urea and 3.42 g sugar in 100 ml at 27°C
- a) 492 atm
- b) 4.92 atm
- c) 49.2 atm
- d) 28.1 atm
Answer: 4.92 atm
Question: Which gas is most soluble in water?
- a) He
- b) H2
- c) NH3
- d) CO2
Answer: NH3
Question:
Which is having highest elevation in boiling point?
- a) H2O
- b) Solution I
- c) Solution II
- d) Solution III
Answer: Solution III
Question:
Freezing point of solution is marked as
- a) A
- b) B
- c) C
- d) D
Answer: B
Question: van't Hoff factor for acetic acid in aqueous medium at infinite dilution is
- a) 2
- b) 1
- c) 1/2
- d) 3
Answer: 2
Question: Correct order of freezing point of given solution
I. 0.1 M glucose II. 0.2 M urea III. 0.1 M NaCl IV. 0.05 M CaCl2
- a) I < II < III < IV
- b) I > II > III > IV
- c) III = II < IV < I
- d) IV > II > III > I
Answer: III = II < IV < I
Question: Boiling point of 0.01 M AB2 which is 10% dissociated in aqueous medium
as A+2 and B–
- a) 273.006 K
- b) 373.006 K
- c) 0.006 K
- d) 272.006 K
Answer: 373.006 K
Question: Vapour pressure diagram of some liquids plotted against temperature are shown below
Most volatile liquid
- a) A
- b) B
- c) C
- d) D
Answer: A
Question: At higher altitude, the boiling point of water is lowered because
- a) Atmosphere pressure is low
- b) Temperature is low
- c) Atmospheric pressure increases
- d) Water solidifies to ice
Answer: Atmosphere pressure is low
Question: During evaporation of liquid
- a) The temperature of liquid rises
- b) The temperature of liquid falls
- c) The temperature of liquid remains uneffected
- d) The liquid molecules becomes inert
Answer: The temperature of liquid falls
Question: What is the concentration of NO3– ions when equal volumes of 0.1 M AgNO3 and 0.1 M NaCl are mixed together?
- a) 0.1 N
- b) 0.25 M
- c) 0.05 M
- d) 0.2 M
Answer: 0.05 M
Question: If any solute ‘A’ dimerises in water at 1 atm pressure and the boiling point of this solution is 100.52°C. If 2 moles of A is added to 1 kg of water and kb for water is 0.52°C/molal, calculate the percentage association of A
- a) 50%
- b) 30%
- c) 25%
- d) 100%
Answer: 100%
Question: Substance A tetramerises in water to the extent of 80%. A solution of 2.5 g of A in 100 g of water lowers the freezing point by 0.3°C. The molar mass of A is
- a) 122
- b) 31
- c) 244
- d) 62
Answer: 62
Question: K4[Fe(CN)6 ] is supposed to be 40% dissociated when 1M solution prepared. Its boiling point is equal to another 20% mass by volume of non-electrolytic solution A. Considering molality = molarity. The molecular weight of A is
- a) 77
- b) 67
- c) 57
- d) 47
Answer: 77
More Questions........................................................
Question: Which one is not equal to zero for an ideal solution?
- a) ΔP = Pobserved– PRaoult
- b) ΔHmix
- c) ΔSmix
- d) ΔVmix
Answer: ΔSmix
Question: What is the mole fraction of the solute in a 1.00 m aqueous solution?
- a) 0.0354
- b) 0.0177
- c) 0.177
- d) 1.770
Answer: 0.0177
Question: The boiling point of 0.2 mol kg–1 solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is true in this case?
- a) Y is undergoing dissociation in water while X undergoes no change
- b) X is undergoing dissociation in water
- c) Molecular mass of X is greater than the molecular mass of Y
- d) Molecular mass of X is less than the molecular mass of Y
Answer: X is undergoing dissociation in water
Question: Which one of the following electrolytes has the same value of van't Hoff's factor (i) as that of Al2(SO4)3 (if all are 100% ionised)?
- a) K4[Fe(CN)6]
- b) K2SO4
- c) K3[Fe(CN)6]
- d) Al(NO3)3
Answer: K4[Fe(CN)6]
Question: Of the following 0.10m aqueous solutions, which one will exhibit the largest freezing point depression ?
- a) KCl
- b) C6H12O6
- c) Al2(SO4)3
- d) K2SO4
Answer: Al2(SO4)3
Question: The van't Hoff factor i for a compound which undergoes dissociation in one solvent and association in other solvent is respectively
- a) Greater than one and greater than one
- b) Less than one and greater than one
- c) Less than one and less than one
- d) Greater than one and less than one
Answer: Greater than one and less than one
Question: pA and pB are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution. If xA represents the mole fraction of component A, the total pressure of the solution will be
- a) pB+ xA(pB–pA)
- b) pB+ xA(pA–pB)
- c) pA+ xA(pB–pA)
- d) pA+ xA(pA–pB)
Answer: pB+ xA(pA–pB)
Question: The freezing point depression constant for water is –1.86° Cm –1. If 5.00 g Na2SO4 is dissolved in 45.0 g H2O,the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for Na2SO4
- a) 0.381
- b) 2.05
- c) 2.63
- d) 3.11
Answer: 2.63
Question: A 0.1 molal aqueous solution of a weak acid is 30% ionized. If Kf for water is 1.86°C/m, the freezing point of the solution will be
- a) –0.36°C
- b) –0.24°C
- c) –0.18°C
- d) –0.54°C
Answer: –0.24°C
Question: 200 mL of an aqueous solution of a protein contains its 1.26g. The osmotic pressure of this solution at 300 K is found to be 2.57 × 10–3 bar. The molar mass of protein will be (R = 0.083 L bar mol–1 K–1)
- a) 31011 g mol–1
- b) 61038 g mol–1
- c) 51022 g mol–1
- d) 122044 g mol–1
Answer: 61038 g mol–1
Question: A solution of sucrose (molar mass = 342 g mol–1) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be (Kf for water = 1.86 K kg mol–1)
- a) –0.372°C
- b) –0.520°C
- c) +0.372°C
- d) –0.570°C
Answer: –0.372°C
Question: 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
- b) Additon of Na2SO4
- c) Addition of 1.00 molal KI
- d) Addition of water
Answer: Addition of water
Question: A 0.0020 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at –0.00732°C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (k1= –.86°C /m)
- a) 3
- b) 4
- c) 1
- d) 2
Answer: 2
Question: 0.5 molal aqueous solution of a weak acid (HX) is 20% ionized. If Kf for water is 1.86 K kg mol sup–1, the lowering in freezing point of the solution is
- a) –0.56 K
- b) –1.12 K
- c) 0.56 K
- d) 1.12K
Answer: 1.12K
Question: A solution containing 10g per dm3 of urea (molecular mass = 60 g mol–1) is isotonic with a 5% solution of a nonvolatile solute. The molecular mass of this non-volatile solute is
- a) 250 g mol–1
- b) 300 g mol–1
- c) 350 g mol–1
- d) 200 g mol–1
Answer: 300 g mol–1
Question: 1.00 g of a non-electrolyte solute (molar mass 250g mol–1) was dissolved in 51.2 g of benzene. If the freezing point depression constant, Kf of benzene is 5.12 K kg mol–1, the freezing point of benzene will be lowered by
- a) 0.4 K
- b) 0.3 K
- c) 0.5 K
- d) 0.2 K
Answer: 0.4 K
Question: A solution of acetone in ethanol
- a) Shows a negative deviation from Raoult's law
- b) Shows a positive deviation from Raoult's law
- c) Behaves like a near ideal solution
- d) Obeys Raoult's law
Answer: Shows a positive deviation from Raoult's law
Question: During osmosis, flow of water through a semi-permeable membrane is
- a) From solution having higher concentration only
- b) From both sides of semi-permeable membrane with equal flow rates
- c) From both sides of semi-permeable membrane with unequal flor rates
- d) From solution having lower concentration only
Answer: From both sides of semi-permeable membrane with unequal flor rates
Question: The vapour pressure of two liquids P and Q are 80 and 60 torr, respectively. The total vapour pressure of solution obtained by mixing 3 moles of P and 2 moles of Q would be
- a) 140 torr
- b) 20 torr
- c) 68 torr
- d) 72 torr
Answer: 72 torr
Question: A solution of urea (mol. mass 60g mol-1) boils at 100.18°C at the atmospheric pressure. If kf and kb for water are 1.86 and 0.512K kg mol–1 respectively, the above solution will freeze at
- a) –6.54°C
- b) 6.54°C
- c) 0.654°C
- d) –0.654°C
Answer: –0.654°C
Question: A solution has a 1 : 4 mole ratio of pentane to hexane. The vapour pressure of the pure hydrocarbons at 20°C are 440 mm of Hg for pentane and 120 mm of Hg for hexane. The mole fraction of pentane in the vapour phase would be
- a) 0.549
- b) 0.200
- c) 0.786
- d) 0.478
Answer: 0.478
Question: The mole fraction of the solute in one molal aqueous solution is
- a) 0.027
- b) 0.036
- c) 0.018
- d) 0.009
Answer: 0.018
Question: Which of the following compounds can be used as antifreeze in automobile radiators?
- a) Methyl alcohol
- b) Glycol
- c) Nitrophenol
- d) Ethyl alcohol
Answer: Glycol
Question: Mole fraction of the solute in a 1.00 molal aqueous solution is
- a) 1.7700
- b) 0.1770
- c) 0.0177
- d) 0.0344
Answer: 0.0177
Question: 1 × 10–3 m solution of Pt(NH3)4Cl4 in H2O shows depression in freezing point by 0.0054°C. The structure of the compound will be (Given Kf = 1.860 km–1)
- a) [Pt(NH3)4]Cl4
- b) [Pt(NH3)3Cl]Cl3
- c) [Pt(NH3)2Cl2]Cl2
- d) Pt(NH3)Cl3]Cl
Answer: [Pt(NH3)2Cl2]Cl2
Question: Which of the following salt has the same value of van’t Hoff’s factor i as that of K3[Fe(CN)6]?
- a) Na2SO4
- b) Al(NO3)3
- c) Al2(SO4)3
- d) NaCl
Answer: Al(NO3)3
Question: At 25°C, the highest osmotic pressure is exhibited by 0.1 M solution of
- a) Glucose
- b) Urea
- c) CaCl2
- d) KCl
Answer: CaCl2
Question: According to Raoult’s law, the relative lowering of vapour pressure for a solution is equal to
- a) Mole fraction of solute
- b) Mole fraction of solvent
- c) Moles of solute
- d) Moles of solvent
Answer: Mole fraction of solute
Question: The concentration units, independent of temperature, would be
- a) Normality
- b) Weight volume percent
- c) Molality
- d) Molarity
Answer: Molality
Question: The vapour pressure of CCI4 at 25ºC is 143 mm Hg. If 0.5 gm of a non-volatile solute (mol. weight = 65) is dissolved in 100 g CCI4 , the vapour pressure of the solution will be
- a) 199.34 mm Hg
- b) 143.99 mm Hg
- c) 141.43 mm Hg
- d) 94.39 mm Hg
Answer: 141.43 mm Hg
Question: In liquid-gas equilibrium, the pressure of vapours above the liquid is constant at
- a) Constant temperature
- b) Low temperature
- c) High temperature
- d) None of these
Answer: Constant temperature
Question: What is the molarity of H2SO4 solution, that has a density 1.84 gm/cc at 35ºC and contains 98% by weight of solute?
- a) 18.4 M
- b) 18 M
- c) 4.18 M
- d) 8.14 M
Answer: 18.4 M
Question: A 5% (w/v) solution of cane sugar (mol. wt. = 342) is isotonic with 1% (w/v) solution of a substance X. The molecular weight of X is
- a) 68.4
- b) 171.2
- c) 34.2
- d) 136.8
Answer: 68.4
Question: The vapour pressure of a solvent decreased by 10 mm of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be 20 mm of mercury?
- a) 0.4
- b) 0.6
- c) 0.8
- d) 0.2
Answer: 0.6
Question: If 0.15 g of a solute, dissolved in 15 g of solvent, is boiled at a temperature higher by 0.216°C, than that of the pure solvent. The molecular weight of the substance, (Molal elevation constant for the solvent is 2.16°C) is
- a) 10.1
- b) 100
- c) 1.01
- d) 1000
Answer: 100
Question: The vapour pressure of benzene at a certain temperature is 640 mm of Hg. A non-volatile and non-electrolyte solid, weighing 2.175 g is added to 39.08 of benzene. The vapour pressure of the solution is 600 mm of Hg. What is the molecular weight of solid substance?
- a) 65.2
- b) 59.6
- c) 49.50
- d) 79.8
Answer: 65.2
Question: From the colligative properties of solution which one is the best method for the determination of molecular weight of proteins and polymers?
- a) Osmotic pressure
- b) Lowering in vapour pressure
- c) Lowering in freezing point
- d) Elevation in boiling point
Answer: Osmotic pressure
Question: Molarity of liquid HCl, if density of solution is 1.17 gm/cc is
- a) 36.5
- b) 18.25
- c) 32.05
- d) 42.10
Answer: 32.05
Question: A solution contains non volatile solute of molecular mass M2. Which of the following can be used to calculate the molecular mass of solute in terms of osmotic pressure? (m2- mass of solute, V - volume of solution,π - osmotic pressure)
- a)
- b)
- c)
- d)
Answer:
Question: A solution containing components A and B follows Raoult’s law
- a) A - B attraction force is greater than A - A and B - B
- b) A - B attraction force is less than A - A and B - B
- c) A - B attraction force remains same as A - A and B - B
- d) Volume of solution is different from sum of volume of solute and solvent
Answer: A - B attraction force remains same as A - A and B - B
Question: From the colligative properties of solution which one is the best method for the determination of molecular weight of proteins and polymers?
- a) Osmotic pressure
- b) Lowering in vapour pressure
- c) Lowering in freezing point
- d) Elevation in boiling point
Answer: Osmotic pressure
Question: Camphor is often used in molecular mass determination because
- a) It is readily available
- b) It has very high cryoscopic constant
- c) It is volatile
- d) It is solvent for organic substances
Answer: It has very high cryoscopic constant
Question: The vapour pressure of a solvent decreased by 10 mm of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be 20 mm of mercury?
- a) 0.4
- b) 0.6
- c) 0.8
- d) 0.2
Answer: 0.6
Question: Formation of a solution from two components can be considered as
Solution so formed will be ideal if
- a)
- b)
- c)
- d)
Answer:
Question: In liquid-gas equilibrium, the pressure of vapours above the liquid is constant at
- a) Constant temperature
- b) Low temperature
- c) High temperature
- d) None of these
Answer: Constant temperature
Question: Which of the following compounds can be used as antifreeze in automobile radiators?
- a) Methyl alcohol
- b) Glycol
- c) Nitrophenol
- d) Ethyl alcohol
Answer: Glycol
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MCQs for Solutions Chemistry Full Syllabus
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