MCQs for NCERT Class 12 Chemistry Chapter 2 Solutions

Please refer to the MCQ Questions for Class 12 Chemistry Chapter 2 Solutions with Answers. The following Solutions Class 12 Chemistry MCQ Questions have been designed based on the latest syllabus and examination pattern for Class 12. Our experts have designed MCQ Questions for Class 12 Chemistry with Answers for all chapters in your NCERT Class 12 Chemistry book.

Solutions Class 12 MCQ Questions with Answers

See below Solutions Class 12 Chemistry MCQ Questions, solve the questions and compare your answers with the solutions provided below.

Question. The system that forms maximum boiling azeotrope is
(a) carbondisulphide – acetone
(b) benzene – toluene
(c) acetone – chloroform
(d) n-hexane – n-heptane

Question. The molarity of the solution containing 7.1 g of Na₂SO₄ in 100 ml of aqueous solution is
(a) 2 M
(b) 0.5 M
(c) 1 M
(d) 0.05 M

Question. Which one of the following aqueous solutions will exihibit highest boiling point ?
(a) 0.015 M urea
(b) 0.01 M KNO₃
(c) 0.01 M Na₂SO₄
(d) 0.015 M glucose

Question. The relative lowering of the vapour pressure is equal to the ratio between the number of
(a) solute molecules to the solvent molecules
(b) solute molecules to the total molecules in the solution
(c) solvent molecules to the total molecules in the solution
(d) solvent molecules to the total number of ions of the solute. 

Question. The liquids at a given temperature vapourise and under equilibrium conditions the pressure exerted by the vapours of the liquid over the liquid phase is called
(a) osmotic pressure
(b) atmospheric pressure
(c) hydrostatic pressure
(d) vapour pressure

Question. The vapour pressure of the solution at a given temperature is found to be …………… than the vapour pressure of the pure solvent at the same temperature.
(a) higher
(b) lower
(c) equal
(d) can’t calculate

Question. The elevation in boiling point of a solution of 13.44 g of CuCl₂ in 1 kg of water using the following information will be (Molecular weight of CuCl₂= 134.4 g and Kb= 0.52 K kg mol^-1)
(a) 0.16
(b) 0.05
(c) 0.1
(d) 0.2

Question. Which one of the following binary mixtures forms an azeotrope with minimum boiling point type?
(a) acetone-ethanol
(b) H₂O-HNO₃
(c) benzene-toluene
(d) n-hexane-n-heptane

Question. A plot of p₁ or p₂ vs the mole fractions x₁ and x₂ is given as.   

In this figure, lines I and II pass through the point for which.
(a) x₁ ≠ 1; x₂ = 1
(b) x₁ = x₂ ≠ 1
(c) x₁ = 1; x₂ ≠ 1
(d) x₁ = x₂ = 1 

Question. Which of the following aqueous solution has minimum freezing point ?
(a) 0.01 m NaCl
(b) 0.005 m C₂H₅OH
(c) 0.005 m Mg_I2
(d) 0.005 m MgSO₄.

Question. Which of the following fluoride is used as rat poison?
(a) CaF₂
(b) KF
(c) NaF
(d) MgF₂

Question. If N/10 50 ml H₂SO₄, N/3 30 ml HNO₃, N/2 10 ml HCl is mixed and solution is made to 1L. Then normality of resultant solution is
(a) N/ 20
(b) N/40
(c) N/50
(d) N

Question. A solution made by dissolving 40 g NaOH in 1000 g of water is
(a) 1 molar
(b) 1 normal
(c) 1 molal
(d) None of these

Question. The value of Henry’s constant KH is _______.
(a) greater for gases with higher solubility.
(b) greater for gases with lower solubility.
(c) constant for all gases.
(d) not related to the solubility of gases

Question.P_A and P_B 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) P_A + X_A (P_B – P_A)
(b) P_A + X_A (P_A – P_B)
(c) P_B + X_A (P_B – P_A)
(d) P_B + X_A (P_A – P_B)

Question. An X molal solution of a compound in benzene has mole fraction of solute equal to 0.2. The value of X is
(a) 14
(b) 3.2
(c) 1.4
(d) 2

Question. A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of 290 mm Hg at 300 K. The vapour pressure of propyl alcohol is 200 mm Hg. If the mole fraction of ethyl alcohol is 0.6, its vapour pressure (in mm Hg) at the same temperature will be
(a) 360
(b) 350
(c) 300
(d) 700

Question. Molarity of H₂SO₄ is 18 M. Its density is 1.8 g/ml. Hence molality is
(a) 36
(b) 200
(c) 500
(d) 18

Question. How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO₃ ? The concentrated acid is 70% HNO₃
(a) 90.0 g conc. HNO₃
(b) 70.0 g conc. HNO₃
(c) 54.0 g conc. HNO₃
(d) 45.0 g conc. HNO₃

Question. Freezing point of an aqueous solution is – 0.186°C. If the values of Kb and Kf of water are respectively 0.52 K kg mol^–1 and 1.86 K kg mol^–1, then the elevation of boiling point of the solution in K is
(a) 0.52
(b) 1.04
(c) 1.34
(d) 0.052

Question. The molecular weight of benzoic acid in benzene as determined by depression in freezing point method corresponds to
(a) ionization of benzoic acid.
(b) dimerization of benzoic acid.
(c) trimerization of benzoic acid.
(d) solvation of benzoic acid. 

Question. The mole fraction of the solute in one molal aqueous solution i
(a) 0.009
(b) 0.018
(c) 0.027
(d) 0.036

Question. A solution containing components A and B follows Raoult’s law when
(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

Question. Scuba divers may experience a condition called ______.
To avoids this, the tanks used by scuba divers are filled with air diluted with _____ .
(a) Migrains, Hydrogen
(b) Cramps, Nitrogen
(c) Nausea, Oxygen
(d) Bends, Helium

Question. An ideal solution is formed when its components
(a) have no volume change on mixing
(b) have no enthalpy change on mixing
(c) Both (a) and (b) are correct
(d) Neither (a) nor (b) is correct 

Question. When a solute is present in trace quantities the following expression is used
(a) Gram per million
(b) Milligram percent
(c) Microgram percent
(d) Parts per million

Question. 18 g of glucose (C₆H₁₂O₆) is added to 178.2 g of water. The vapour pressure of water for this aqueous solution is
(a) 76.00 torr
(b) 752.40 torr
(c) 759.00 torr
(d) 7.60 torr

Question. The molarity of pure water is
(a) 50 M
(b) 18 M
(c) 55.6 M
(d) 100 M

Question.An aqueous solution of glucose is 10% in strength. The volume in which 1 g mole of it is dissolved, will be
(a) 9 litre
(b) 1.8 litre
(c) 8 litre
(d) 0.9 litre

Question. A mixture of components A and B will show –ve deviation when
(a) ΔV_mix > 0
(b) ΔH_mix < 0
(c) A–B interaction is weaker than A–A and B– B interactions
(d) A–B interaction is stronger than A–A and B–B interactions.

Question. A solution of acetone in ethanol
(a) shows a positive deviation from Raoult’s law
(b) behaves like a non ideal solution
(c) obeys Raoult’s law
(d) shows a negative deviation from Raoult’s law 

Question. Which one of the following binary liquid systems shows positive deviation from Raoult’s law?
(a) Benzene-toluene
(b) Carbon disulphide-acetone
(c) Phenol-aniline
(d) Chloroform-acetone

Question. Blood cells retain their normal shape in solution which are
(a) hypotonic to blood
(b) isotonic to blood
(c) hypertonic to blood
(d) equinormal to blood.

Question. Isotonic solutions have same
(a) molar concentration
(b) molality
(c) normality
(d) None of these

Question. 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 negative deviation from Raoult’s Law.
(b) The solution is non-ideal, showing positive deviation from Raoult’s Law.
(c) n-heptane shows positive deviation while ethanol shows negative deviation from Raoult’s Law.
(d) The solution formed is an ideal solution.

Question. Which one is not equal to zero for an ideal solution:
(a) ΔS_mix
(b) ΔV_mix
(c) ΔP = P_observed – P_Raoult
(d) ΔH_mix

Question. A mixture of two completely miscible non-ideal liquids which distill as such without change in its composition at a constant temperature as though it were a pure liquid. This mixture is known as
(a) binary liquid mixture
(b) azeotropic mixture
(c) eutectic mixture
(d) ideal mixture

Question. Molarity of liquid HCl will be, if density of solution is 1.17 gm/cc
(a) 36.5
(b) 32.05
(c) 18.25
(d) 42.10

Question. On the basis of information given below mark the correct option.
Information: On adding acetone to methanol some of the hydrogen bonds between methanol molecules break.
(a) At specific composition methanol-acetone mixture will form boiling azeotrope and will show positive deviation from Raoult’s law.
(b) At specific composition methanol-acetone mixture forms boiling azeotrope and will show positive deviation from Raoult’s law.
(c) At specific composition methanol-acetone mixture will form minimum boiling azeotrope and will show negative deviation from Raoult’s law.
(d) At specific composition methanol-acetone mixture will form boiling azeotrope and will show negative deviation from Raoult’s law.

Question. Relation between partial pressure and mole fraction is stated by
(a) Graham’s law
(b) Raoult’s law
(c) Le-Chatelier
(d) Avogadro law

Question. Which of the following is dependent on temperature?
(a) Molarity
(b) Mole fraction
(c) Weight percentage
(d) Molality 

Question. What is the mole fraction of the solute in a 1.00 m aqueous solution?
(a) 1.770
(b) 0.0354
(c) 0.0177
(d) 0.177 

Question. How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M HNO₃? The concentrated acid is 70% HNO₃.
(a) 70.0 g conc. HNO₃
(b) 54.0 g conc. HNO₃
(c) 45.0 g conc. HNO₃
(d) 90.0 g conc. HNO₃

Question. Which of the following compounds can be used as antifreeze in automobile radiators?
(a) Methyl alcohol
(b) Glycol
(c) Nitrophenol
(d) Ethyl alcohol

Question. Concentrated aqueous sulphuric acid is 98% H₂SO₄ by mass and has a density of 1.80 g mL–1. Volume of acid required to make one litre of 0.1 M H₂SO₄ solution is
(a) 16.65 mL
(b) 22.20 mL
(c) 5.55 mL
(d) 11.10 mL

Question. The mole fraction of the solute in one molal aqueous solution is
(a) 0.009
(b) 0.018
(c) 0.027
(d) 0.036

Question. 2.5 litre of 1 M NaOH solution is mixed with another 3 litre of 0.5 M NaOH solution. Then find out molarity of resultant solution.
(a) 0.80 M
(b) 1.0 M
(c) 0.73 M
(d) 0.50 M

Question. How many g of dibasic acid (mol. weight 200) should be present in 100 mL of the aqueous solution to give strength of 0.1 N?
(a) 10 g
(b) 2 g
(c) 1 g
(d) 20 g 

Question. What is the molarity of H₂SO₄ solution, that has a density 1.84 g/cc at 35°C and contains 98% by weight?
(a) 18.4 M
(b) 18 M
(c) 4.18 M
(d) 8.14 M 

Question. The concentration unit, independent of temperature, would be
(a) normality
(b) weight volume percent
(c) molality
(d) molarity. 

Question. How many grams of CH³OH should be added to water to prepare 150 mL solution of 2 M CH³OH?
(a) 9.6 × 10³
(b) 2.4 × 10³
(c) 9.6
(d) 2.4

Question. In water saturated air, the mole fraction of water vapour is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is
(a) 1.18 atm
(b) 1.76 atm
(c) 1.176 atm
(d) 0.98 atm.

Question. pA and pB are the vapour pressures 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) pA + xA(pB – pA)
(b) pA + xA ( pA – pB)
(c) pB + xA(pB – pA)
(d) pB + xA ( pA – pB)

Question. Vapour pressure of chloroform (CHCl₃) and dichloromethane (CH₂Cl₂) at 25°C are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of CHCl₃ and 40 g of CH₂Cl₂ at the same temperature will be (Molecular mass of CHCl₃ = 119.5 u and molecular mass of CH₂Cl₂ = 85 u)
(a) 173.9 mm Hg
(b) 615.0 mm Hg
(c) 347.9 mm Hg
(d) 285.5 mm Hg

Question. A solution has a 1 : 4 mole ratio of pentane to hexane.
The vapour pressures of the pure hydrocarbons at 20 °C are 440 mm Hg for pentane and 120 mm Hg for hexane. The mole fraction of pentane in the vapour phase would be
(a) 0.200
(b) 0.549
(c) 0.786
(d) 0.478 

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 mole of P and 2 mol of Q would be
(a) 72 torr
(b) 140 torr
(c) 68 torr
(d) 20 torr

Question. The mixture which shows positive deviation from Raoult’s law is
(a) ethanol + acetone
(b) benzene + toluene
(c) acetone + chloroform
(d) chloroethane + bromoethane.

Question. For an ideal solution, the correct option is
(a) DmixG = 0 at constant T and P
(b) DmixS = 0 at constant T and P
(c) Dmix V ≠ 0 at constant T and P
(d) Dmix H = 0 at constant T and P. 

Question. The mixture that forms maximum boiling azeotrope is
(a) heptane + octane
(b) water + nitric acid
(c) ethanol + water
(d) acetone + carbon disulphide. 

Question. Which of the following statements is correct regarding a solution of two components A and B exhibiting positive deviation from ideal behaviour?
(a) Intermolecular attractive forces between A-A and B-B are stronger than those between A-B.
(b) Δmix H = 0 at constant T and P.
(c) Δmix V = 0 at constant T and P.
(d) Intermolecular attractive forces between A-A and B-B are equal to those between A-B.

Question. Which one of the following is incorrect for ideal solution?
(a) DHmix = 0
(b) DUmix = 0
(c) DP = Pobs – Pcalculated by Raoult’s law = 0
(d) DGmix = 0

Question. Which of the following statements about the composition of the vapour over an ideal 1 : 1 molar mixture of benzene and toluene is correct? Assume that the temperature is constant at 25°C.
(Given, vapour pressure data at 25°C, benzene = 12.8 kPa, toluene = 3.85 kPa)
(a) The vapour will contain equal amounts of benzene and toluene.
(b) Not enough information is given to make a prediction.
(c) The vapour will contain a higher percentage of benzene.
(d) The vapour will contain a higher percentage of toluene. 

Question. Which condition is not satisfied by an ideal solution?
(a) DmixV = 0
(b) DmixS = 0
(c) Obeyance to Raoult’s Law
(d) DmixH = 0 

Question. A solution of acetone in ethanol
(a) obeys Raoult’s law
(b) shows a negative deviation from Raoult’s law
(c) shows a positive deviation from Raoult’s law
(d) behaves like a near ideal solution.

Question. What is the amount of urea dissolved per litre if its aqueous solution is isotonic with 10% cane sugar solution ? (mol. wt. of urea = 60)
(a) 200 g/L
(b) 19.2 g/L
(c) 17.54g/L
(d) 16.7 g/L

Question. The mass of glucose that should be dissolved in 50 g of water in order to produce the same lowering of vapour pressure as is produced by dissolving 1 g of urea in the same quantity of water is 
(a) 1 g
(b) 3 g
(c) 6 g
(d) 18 g

Question. A 5.25% solution of a substance is isotonic with a 1.5% solution of urea (molar mass = 60 g mol^-1) in the same solvent. If the densities of both the solutions are assumed to be equal to 1.0 g cm^-3, molar mass of the substance will be 
(a) 90.0 g mol^-1
(b) 115.0 g mol^-1
(c) 105.0 g mol^-1
(d) 210.0 g mol^-1

Question. A solution of sucrose (molar mass= 342g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure
(R = 0.082L atm K^-1 mol^-1) at 273 K ? 
(a) 3.92 atm
(b) 4.48 atm
(c) 5.92 atm
(d) 29.4 atm

Question. At temperature 327°C and concentration C osmotic pressure of a solution is p, the same solutions at concentration C/2 and a temperature 427°C shows osmotic pressure 2 atm, value of p will be 
(a) 12/7
(b) 24/7
(c) 6/5
(d) 5/6

Question. Which one of the following statements is false?
(a) Raoult’s law states that the vapour pressure of a component over a solution is proportional to its mole fraction
(b) The osmotic pressure (n) of a solution is given by the equation n = MRT, where, M is the molarity of the solution
(c) The correct order of osmotic pressure for 0.01 M aqueous solution of each compound is BaCl₂ > KCl > CH₃COOH > sucrose
(d) Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression

Question. A solution containing 4 g of polyvinyl chloride polymer in one litre of dioxane was found to have an osmotic pressure of 4 .1 x 10^-4 atm at 27°C. The approximate molecular weight of the polymer is 
(a) 1.5 X 10³
(b) 2.4 X 10⁵
(c) 1.0 x 10⁴
(d) 2 x 10¹²

Question. The amount of urea to be dissolved in 500 cc of water (K_f = 1.86° C) to produce a depression of 0. 1.86°C in the freezing point is 
(a) 9g
(b) 6g
(c) 3g
(d) 0.3g

Question. Blood cells do not shrink in blood because blood is
(a) hypotonic
(b) isotonic 
(c) equimolar
(d) hypertonic

Question. The empirical formula of a non-electrolyte is CH₂O. A solution containing 6 g of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution at the same temperature. The molecular formula of the compound is 
(a) C₂H₄O₂
(b) C₃H₆O₃
(c) C₅H₁₀O₅
(d) ₄H₈O₄

Question. In a 0.2 molal aqueous solution of a weak acid HX, the degree of ionisation is 0.3. Taking K I for water as 1.85, the freezing point of the solution will be nearest to
(a) -0.481°C
(b) -0.360°C 
(c) -0.260°C
(d) +0.480°C

Question. Which one is a colligative prope1ty?
(a) Boiling point
(b) Vapour pressure
(c) Osmotic pressure
(d) Freezing point

Question. 18 g of glucose (C₆H₁₂O₆ ) is added to 178.2 g of water. The vapour pressure of water for this aqueous solution at 100°C is 
(a) 759.00 Torr
(b) 7.60 Torr
(c) 76.00 Torr
(d) 752.40 Torr

Question. The freezing point of a 0.05 molal solution of a non-electrolyte in water is
(a) – 0. 093° C
(b) 1.86° C
(c) 0. 93° C
(d) 0. 093° C

Question. Relative lowering of vapour pressw·e of a dilute solution is 0.2. What is the mole fraction of the non-volatile solute?
(a) 0.8
(b) 0.5
(c) 0.3
(d) 0.2

Question. Depression in freezing point is 6 K for NaCl solution if k_f for water is 1.86 K/kg/mol, amount of NaCl dissolved in 1 kg water is 
(a) 3.42
(b) 1.62
(c) 3.24
(d) 1.71

Question. If a solution containing 0.072 g atom of sulphur in 100 g of a solvent (k_f = 7.0) gave a freezing point depression of 0.84 °C, the molecular formula of sulphur in the solution is
(a) S6
(b) S7
(c) S8
(d) S9

Question. Equimolar solution in the same solvent have 
(a) different boiling and different freezing points
(b) same boiling and same freezing points
(c) same freezing point but different boiling point
(d) same boiling point but different freezing point

Question. The molar freezing point constant for water is 1.86°C/mol. If 342 g ofcane sugar (C₁₂H₂₂O₁₁ ) is dissolved in 1000 g of water, the solution will freeze at
(a) -1. 86° C
(b) 1.86°C
(c) – 3.92° C
(d) 2.42° C

Question. The movement of solvent molecules through a semipem1eable membrane is called
(a) electrolysis
(b) electrophoresis
(c) osmosis
(d) cataphoresis

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. 

Question. All form ideal solution except
(a) C₆H₆ and C₆H₅CH₃
(b) C₂H₆ and C₂H₅I
(c) C₆H₅Cl and C₆H₅Br
(d) C₂H₅I and C₂H₅OH

Question. An ideal solution is formed when its components
(a) have no volume change on mixing
(b) have no enthalpy change on mixing
(c) have both the above characteristics
(d) have high solubility.

Question. The freezing point depression constant (Kf) of benzene is 5.12 K kg mol–1. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places)
(a) 0.20 K
(b) 0.80 K
(c) 0.40 K
(d) 0.60 K

Question. If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be
(a) halved
(b) tripled
(c) unchanged
(d) doubled. 

Question. At 100°C the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If Kb = 0.52, the boiling point of this solution will be
(a) 102 °C
(b) 103 °C
(c) 101 °C
(d) 100 °C

Question. 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 × 10^–3 bar. The molar mass of protein will be (R = 0.083 L bar mol^–1 K^–1)
(a) 51022 g mol^–1
(b) 122044 g mol^–1
(c) 31011 g mol^–1
(d) 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 

Question. During osmosis, flow of water through a semipermeable membrane is
(a) from solution having lower concentration only
(b) from solution having higher concentration only
(c) from both sides of semipermeable membrane with equal flow rates
(d) from both sides of semipermeable membrane with unequal flow rates. 

Question. 1.00 g of a non-electrolyte solute (molar mass 250 g mol^–1) was dissolved in 51.2 g of benzene. If the freezing point constant, Kf of benzene is 5.12 K kg mol^–1, the freezing point of benzene will be lowered by
(a) 0.2 K
(b) 0.4 K
(c) 0.3 K
(d) 0.5 K 

Question. A solution containing 10 g per dm3 of urea (molecular mass = 60 g mol–1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is
(a) 200 g mol^–1
(b) 250 g mol^–1
(c) 300 g mol^–1
(d) 350 g mol^–1

Question. A solution of urea (mol. mass 56 g mol^–1) boils at 100.18°C at the atmospheric pressure. If Kf and Kb for water are 1.86 and 0.512 K kg mol^–1 respectively, the above solution will freeze at
(a) 0.654°C
(b) – 0.654°C
(c) 6.54°C
(d) – 6.54°C

Question. Pure water can be obtained from sea water by
(a) centrifugation
(b) plasmolysis
(c) reverse osmosis
(d) sedimentation.

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 

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) 69.5
(b) 59.6
(c) 49.50
(d) 79.8 

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 

We hope you liked Solutions Class 12 Chemistry MCQ Questions given above. If you have any queries please put them in the comments box below. Our teachers will provide a response.