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Solution MCQ Set-1

Test your knowledge on Solutions from Chemistry, Class 12.

80

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60

Questions

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Questions in this Quiz

Q1: An aqueous solution of hydrochloric acid
  • Obeys Raoult’s law
  • Shows negative deviation from Raoult’s law
  • Shows positive deviation from Raoult’s law
  • Obeys Henry’s law at all compositions
Q2: Exactly $1\ g$ of urea dissolved in $75\ g$ of water gives a solution that boils at $100.114^\circ C$ at 760 torr. The molecular weight of urea is 60.1. The boiling point elevation constant for water is
  • 1.02
  • 0.51
  • 3.06
  • 1.51
Q3: $12\ g$ 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
  • equal to second
  • greater than second
  • less than second
  • double that of second
Q4: 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)
  • 156
  • 145
  • 150
  • 108
Q5: The freezing point of equimolal aqueous solution will be highest for
  • $C_6H_5NH_3^+Cl^–$
  • $Ca(NO_3)_2$
  • $La(NO_3)_2$
  • $C_6H_{12}O_6$
Q6: Which of the following $0.10\ m$ aqueous solutions will have the lowest freezing point ?
  • $Al_2(SO_4)_3$
  • $C_6H_{12}O_6$
  • $KCl$
  • $C_{12}H_{22}O_{11}$
Q7: A solution containing $10\ g$ per $dm^3$ 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
  • $300\ g\ mol^{–1}$
  • $350\ g\ mol^{–1}$
  • $200\ g\ mol^{–1}$
  • $250\ g\ mol^{–1}$
Q8: The vapour pressure of a solvent decreases by $10\ mm\ of\ Hg$ 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 $20\ mm\ of\ Hg$ ?
  • 0.8
  • 0.6
  • 0.4
  • 0.2
Q9: A solution containing $1.8\ g$ of a compound (empirical formula $CH_2O$) 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 = $1.86\ kg\ K\ mol^{–1}$)
  • $C_2H_4O_2$
  • $C_3H_6O_3$
  • $C_4H_8O_4$
  • $C_6H_{12}O_6$
Q10: Which observation(s) reflect(s) colligative properties?
(i) A $0.5\ m\ NaBr$ solution has a higher vapour pressure than a $0.5\ m\ BaCl_2$ 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
  • (i), (ii) and (iii)
  • (i) and (ii)
  • (ii) and (iii)
  • (i) and (iii)
Q11: The vapour pressure of benzene at $30^\circ C$ is $121.8\ mm$. By adding $15\ g$ of non-volatile solute in $250\ g$ of benzene, its vapour pressure is decreased to $120.2\ mm$. The molecular weight of solute is :
  • $156.6\ g$
  • $267.4\ g$
  • $356.3\ g$
  • $467.4\ g$
Q12: Pure benzene freezes at $5.45^\circ C$. A $0.374\ m$ solution of tetrachloroethane in benzene freezes at $3.55^\circ C$. The $K_f$ for benzene is:
  • 0.508
  • 5.08
  • 50.8
  • 508
Q13: $0.450\ g$ of urea (mol.wt.60) in $22.5\ g$ of water show $0.170^\circ C$ of elevation in boiling point. The molal elevation constant of water is:
  • $0.051^\circ C$
  • $0.51^\circ C$
  • $5.1^\circ C$
  • $0.83^\circ C$
Q14: The colligative property is not represented by :
  • elevation in boiling point
  • osmotic pressure
  • optical activity
  • relative lowering of vapour pressure
Q15: $20\ g$ of a substance were dissolved in $500\ mL$ of water and the osmotic pressure of the solution was found to be $600\ mm$ of mercury at $15^\circ C$. The molecular weight of substance is :
  • 998
  • 1028
  • 1098
  • 1198
Q16: Which one of the statements given below concerning properties of solutions, describes a colligative effect?
  • Boiling point of pure water decreases by the addition of ethanol
  • Vapour pressure of pure water decreases by the addition of nitric acid
  • Vapour pressure of pure benzene decreases by the addition of naphthalene
  • Boiling point of pure benzene increases by the addition of toluene
Q17: The average osmotic pressure of human blood is $7.8\ bar$ at $37^\circ C$. What is the concentration of an aqueous NaCl solution that could be used in the blood stream?
  • $0.16\ mol/L$
  • $0.31\ mol / L$
  • $0.60\ mol / L$
  • $0.45\ mol / L$
Q18: A $5\%$ solution (by mass) of cane sugar in water has freezing point of $271\ K$ and freezing point of pure water is $273.15\ K$. The freezing point of a $5\%$ solution (by mass) of glucose in water is
  • $271\ K$
  • $273.15\ K$
  • $269.07\ K$
  • $277.23\ K$
Q19: The vapour pressure of pure benzene at a certain temperature is $0.850\ bar$. A non-volatile, nonelectrolyte solid weighing $0.5\ g$ is added to $39.0\ g$ of benzene (molar mass $78\ g/mol$). The vapour pressure of the solution then is $0.845\ bar$. What is the molecular mass of the solid substance?
  • 58
  • 180
  • 170
  • 145
Q20: $0.01\ M$ solution of $KCl$ and $BaCl_2$ are prepared in water. The freezing point of $KCl$ is found to be $–2^\circ C$. What is the freezing point of $BaCl_2$ to be completely ionised ?
  • $– 3^\circ C$
  • $+ 3^\circ C$
  • $– 2^\circ C$
  • $– 4^\circ C$
Q21: “The importance of many pure substance in life depends on their composition.” Which of the following statement justify the above fact?
  • $1\ ppm$ of fluoride ions in water prevents tooth decay.
  • $1.5\ ppm$ of fluoride ions causes tooth decay.
  • Concentration above $1.5\ ppm$ can be poisonous.
  • All of the above.
Q22: Which of the following fluoride is used as rat poison?
  • $CaF_2$
  • $KF$
  • $NaF$
  • $MgF_2$
Q23: Most of the processes in our body occur in
  • solid solution
  • liquid solution
  • gaseous solution
  • colloidal solution
Q24: The term homogenous mixtures signifies that
  • its composition is uniform throughout the mixture.
  • its properties are uniform throughout the mixture.
  • both composition and properties are uniform throughout the mixture.
  • neither composition nor properties are uniform throughout the mixture.
Q25: Which of the following mixture is(are) called solution?
(i) water + ammonia
(ii) water + acetone
(iii) acetone + alcohol
(iv) hexane + water
  • (i), (ii) and (iii)
  • (i), (iii) and (iv)
  • (i) and (iv)
  • (ii) and (iii)
Q26: Which of the following is a quantitative description of the solution?
  • Dilute
  • Concentrated
  • Saturated
  • Molar
Q27: When a solute is present in trace quantities the following expression is used
  • Gram per million
  • Milligram percent
  • Microgram percent
  • Parts per million
Q28: Molarity of liquid $HCl$ will be, if density of solution is $1.17\ gm/cc$
  • 36.5
  • 32.05
  • 18.25
  • 42.10
Q29: $1\ M, 2.5\ litre\ NaOH$ solution is mixed with another $0.5\ M, 3\ litre\ NaOH$ solution. Then find out the molarity of resultant solution
  • $0.80\ M$
  • $1.0\ M$
  • $0.73\ M$
  • $0.50\ M$
Q30: An $X$ molal solution of a compound in benzene has mole fraction of solute equal to $0.2$. The value of $X$ is
  • 14
  • 3.2
  • 1.4
  • 2
Q31: The molarity of the solution containing $7.1\ g$ of $Na_2SO_4$ in $100\ ml$ of aqueous solution is
  • $2\ M$
  • $0.5\ M$
  • $1\ M$
  • $0.05\ M$
Q32: The vapour pressure of pure benzene at $25^\circ C$ is $640\ mm\ Hg$ and that of solution of solute A is $630\ mm\ Hg$. The molality of solution is
  • $0.2\ m$
  • $0.4\ m$
  • $0.5\ m$
  • $0.1\ m$
Q33: $4.0\ g$ of $NaOH$ is dissolved in $100\ ml$ solution. The normality of the solution is
  • $0.1\ N$
  • $0.5\ N$
  • $4.0\ N$
  • $1.0\ N$
Q34: The molarity of pure water is
  • $50\ M$
  • $18\ M$
  • $55.6\ M$
  • $100\ M$
Q35: An aqueous solution of glucose is $10\%$ in strength. The volume in which $1\ g$ mole of it is dissolved, will be
  • $9\ litre$
  • $1.8\ litre$
  • $8\ litre$
  • $0.9\ litre$
Q36: $10\ g$ of $NaCl$ is dissolved in $10^6\ g$ of the solution. Its concentration is
  • $100\ ppm$
  • $0.1\ ppm$
  • $1\ ppm$
  • $10\ ppm$
Q37: On adding a solute to a solvent having vapour pressure $0.80\ atm$, vapour pressure reduces to $0.60\ atm$. Mole fraction of solute is
  • 0.25
  • 0.75
  • 0.50
  • 0.33
Q38: $2.5\ litres$ of $NaCl$ solution contain $5\ moles$ of the solute. What is the molarity?
  • 5 molar
  • 2 molar
  • 2.5 molar
  • 12.5 molar
Q39: The mole fraction of the solute in one molal aqueous solution is
  • 0.009
  • 0.018
  • 0.027
  • 0.036
Q40: $5\ ml$ of $N\ HCl$, $20\ ml$ of $N/2\ H_2SO_4$ and $30\ ml$ of $N/3\ HNO_3$ are mixed together and volume made to one litre. The normality of the resulting solution is
  • $N/5$
  • $N/40$
  • $N/20$
  • $N/40$
Q41: $25\ ml$ of a solution of barium hydroxide on titration with a $0.1$ molar solution of hydrochloric acid gave a titre value of $35\ ml$. The molarity of barium hydroxide solution was
  • 0.07
  • 0.14
  • 0.28
  • 0.35
Q42: Mole fraction of the solute in a $1.00\ molal$ aqueous solution is
  • 0.1770
  • 0.0177
  • 0.0344
  • 1.7700
Q43: What is the normality of a $1\ M$ solution of $H_3PO_4$?
  • $0.5\ N$
  • $1.0\ N$
  • $2.0\ N$
  • $3.0\ N$
Q44: The volume of $4\ N\ HCl$ and $10\ N\ HCl$ required to make 1 litre of $6\ N\ HCl$ are
  • $0.75\ litre$ of $10\ N\ HCl$ and $0.25\ litre$ of $4\ N\ HCl$
  • $0.50\ litre$ of $4\ N\ HCl$ and $0.50\ litre$ of $10\ N\ HCl$
  • $0.67\ litre$ of $4\ N\ HCl$ and $0.33\ litre$ of $10\ N\ HCl$
  • $0.80\ litre$ of $4\ N\ HCl$ and $0.20\ litre$ of $10\ N\ HCl$
Q45: Molarity of $H_2SO_4$ is $18\ M$. Its density is $1.8\ g/ml$. Hence molality is
  • 36
  • 200
  • 500
  • 18
Q46: $200\ ml$ of water is added to $500\ ml$ of $0.2\ M$ solution. What is the molarity of this diluted solution ?
  • $0.5010\ M$
  • $0.2897\ M$
  • $0.7093\ M$
  • $0.1428\ M$
Q47: How many grams of concentrated nitric acid solution should be used to prepare $250\ mL$ of $2.0\ M\ HNO_3$? The concentrated acid is $70\%\ HNO_3$
  • $90.0\ g$ conc. $HNO_3$
  • $70.0\ g$ conc. $HNO_3$
  • $54.0\ g$ conc. $HNO_3$
  • $45.0\ g$ conc. $HNO_3$
Q48: For preparing $0.1\ N$ solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be
  • Less than the theoretical weight
  • More than the theoretical weight
  • Same as the theoretical weight
  • None of these
Q49: If $N/10\ 50\ ml\ H_2SO_4$, $N/3\ 30\ ml\ HNO_3$, $N/2\ 10\ ml\ HCl$ is mixed and solution is made to $1\ L$. Then normality of resultant solution is
  • $N/20$
  • $N/40$
  • $50/N$
  • $N$
Q50: A solution made by dissolving $40\ g\ NaOH$ in $1000\ g$ of water is
  • 1 molar
  • 1 normal
  • 1 molal
  • None of these
Q51: Which of the following concentration terms is/are independent of temperature?
  • Molality only
  • Molality and mole fraction
  • Molarity and mole fraction
  • Molality and normality
Q52: A solution is prepared by dissolving $10\ g\ NaOH$ in $1250\ mL$ of a solvent of density $0.8\ mL/g$. The molality of the solution in $mol\ kg^{–1}$ is
  • 0.25
  • 0.2
  • 0.008
  • 0.0064
Q53: Which of the following units is useful in relating concentration of solution with its vapour pressure?
  • mole fraction
  • parts per million
  • mass percentage
  • molality
Q54: Which of the following concentration unit is independent of temperature ?
  • Normality
  • Molarity
  • Formality
  • Molality
Q55: Which of the following factor do not affect solubility of solid solute in liquid ?
  • Temperature
  • Pressure
  • Nature of solute
  • All of these
Q56: When a solid solute is added to the solvent, some solute dissolves and its concentration increases in solution. This process is known as ______. Some solute particles in solution collide with the solid solute particles and get separated out of solution. This process is known as ______.
  • Crystallization, dissolution.
  • Dissolution, saturation.
  • Saturation, crystallization.
  • Dissolution, crystallization.
Q57: At the state of dynamic equilibrium, for solute + solvent $\rightleftharpoons$ solution.
  • Rate of dissolution = Rate of unsaturation.
  • Rate of dissolution = Rate of unsaturation.
  • Rate of dissolution = Rate of saturation
  • Rate of crystallization = Rate of saturation.
Q58: Which of the following statements is incorrect?
  • A solution in which no more solute can be dissolved at the same temperature and pressure is called a saturated solution.
  • An unsaturated solution is one in which more solute can be dissolved at the same temperature.
  • The solution which is in dynamic equilibrium with undissolved solute is the saturated solution.
  • The minimum amount of solute dissolved in a given amount of solvent is its solubility.
Q59: On dissolving sugar in water at room temperature solution feels cool to touch. Under which of the following cases dissolution of sugar will be most rapid ?
  • Sugar crystals in cold water.
  • Sugar crystals in hot water.
  • Powdered sugar in cold water.
  • Powdered sugar in hot water.
Q60: The solubility of a solid in a liquid is significantly affected by temperature changes. Solute + Solvent $\rightleftharpoons$ Solution. The system being in a dynamic equilibrium must follow Le-chatelier’s principle. Considering the Le-chatelier’s principle which of the following is correct?
  • $\triangle H_{sol} > 0$; solubility $\uparrow$ ; temperature $\downarrow$
  • $\triangle H_{sol} < 0$; solubility $\downarrow$ ; temperature $\uparrow$
  • $\triangle H_{sol} > 0$; solubility $\downarrow$ ; temperature $\uparrow$
  • $\triangle H_{sol} < 0$; solubility $\downarrow$ ; temperature $\uparrow$