Question. Most of the processes in our body occur in
(a) solid solution
(b) liquid solution
(c) gaseous solution
(d) colloidal solution
Answer
B
Question. Which of the following is a quantitative description of the solution?
(a) Dilute
(b) Concentrated
(c) Saturated
(d) Molar
Answer
D
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
Answer
D
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
Answer
B
Question. 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
(a) 0.80 M
(b) 1.0 M
(c) 0.73 M
(d) 0.50 M
Answer
C
Question. Value of Henry’s constant KH _______.
(a) increases with increase in temperature.
(b) decreases with increase in temperature.
(c) remains constant.
(d) first increases then decreases.
Answer
A
Question. Maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon __________.
(a) Temperature
(b) Nature of solute
(c) Pressure
(d) Nature of solvent
Answer
C
Question. Low concentration of oxygen in the blood and tissues of people living at high altitude is due to _________.
(a) low temperature
(b) low atmospheric pressure
(c) high atmospheric pressure
(d) both low temperature and high atmospheric pressure
Answer
B
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.
Answer
B
Question. Which of the followingfactor(s) affect the solubility of a gaseous solute in the fixed volume of liquid solvent ?
(i) Nature of solute (ii) Temperature (iii) Pressure
(a) (i) and (iii) at constant T
(b) (i) and (ii) at constant P
(c) (ii) and (iii) only
(d) (iii) only
Answer
A
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
Answer
B
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
Answer
B
Question. The molarity of pure water is
(a) 50 M
(b) 18 M
(c) 55.6 M
(d) 100 M
Answer
C
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
Answer
B
Question. 10 g of NaCl is dissolved in 106g of the solution. Its concentration is
(a) 100 ppm
(b) 0.1 ppm
(c) 1 ppm
(d) 10 ppm
Answer
D
Question. “The importance of many pure substance in life depends on their composition.”
Which of the following statement justify the above fact?
(a) 1 ppm of fluoride ions in water prevents tooth decay.
(b) 1.5 ppm of fluoride ions causes tooth decay.
(c) Concentration above 1.5 ppm can be poisonous.
(d) All of the above.
Answer
D
Question. Which of the following fluoride is used as rat poison?
(a) CaF2
(b) KF
(c) NaF
(d) MgF2
Answer
C
Question. 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
(a) 0.25
(b) 0.75
(c) 0.50
(d) 0.33
Answer
A
Question. 5 ml of N HCl, 20 ml of N/2 H2SO4 and 30 ml of N/3 HNO3 are mixed together and volume made to one litre. The normality of the resulting solution is
(a) N/5
(b) N/10
(c) N/20
(d) N/40
Answer
D
Question. 25ml 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
(a) 0.07
(b) 0.14
(c) 0.28
(d) 0.35
Answer
A
Question. Mole fraction of the solute in a 1.00 molal aqueous solution is
(a) 0.1770
(b) 0.0177
(c) 0.0344
(d) 1.7700
Answer
B
Question. The term homogenous mixtures signifies that
(a) its composition is uniform throughout the mixture.
(b) its properties are uniform throughout the mixture.
(c) both composition and properties are uniform throughout the mixture.
(d) neither composition nor properties are uniform throughout the mixture.
Answer
C
Question. Which of the following mixture is(are) called solution?
(i) water + ammonia (ii) water + acetone
(iii) acetone + alcohol (iv) hexane + water
(a) (i), (ii) and (iii) (b) (i), (iii) and (iv)
(c) (i) and (iv) (d) (ii) and (iii)
Answer
A
Question. What is the normality of a 1 M solution of H3PO4 ?
(a) 0.5 N
(b) 1.0 N
(c) 2.0 N
(d) 3.0 N
Answer
D
Question. The vapour pressure of pure benzene at 25°C is 640 mm Hg and that of solution of solute A is 630 mm Hg. The molality of solution is
(a) 0.2 m
(b) 0.4 m
(c) 0.5 m
(d) 0.1 m
Answer
A
Question. 4.0 g of NaOH is dissolved in 100 ml solution. The normality of the solution is
(a) 0.1 N
(b) 0.5 N
(c) 4.0 N
(d) 1.0 N
Answer
D
Question. The volume of 4 N HCl and 10 N HCl required to make 1 litre of 6 N HCl are
(a) 0.75 litre of 10 N HCl and 0.25 litre of 4 N HCl
(b) 0.50 litre of 4 N HCl and 0.50 litre of 10 N HCl
(c) 0.67 litre of 4 N HCl and 0.33 litre of 10 N HCl
(d) 0.80 litre of 4 N HCl and 0.20 litre of 10 N HCl
Answer
C
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
Answer
C
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
Answer
C
Question. Which of the following concentration terms is/are independent of temperature?
(a) Molality only
(b) Molality and mole fraction
(c) Molarity and mole fraction
(d) Molality and normality
Answer
B
Question. 2.5 litres of NaCl solution contain 5 moles of the solute. What is the molarity?
(a) 5 molar
(b) 2 molar
(c) 2.5 molar
(d) 12.5 molar
Answer
B
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
Answer
B
Question. 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
(a) 0.25
(b) 0.2
(c) 0.008
(d) 0.0064
Answer
A
Question. Which of the following units is useful in relating concentration of solution with its vapour pressure?
(a) mole fraction
(b) parts per million
(c) mass percentage
(d) molality
Answer
A
Question. 200 ml of water is added to 500 ml of 0.2 M solution. What is the molarity of this diluted solution ?
(a) 0.5010 M
(b) 0.2897 M
(c) 0.7093 M
(d) 0.1428 M
Answer
D
Question. If N /10 50 ml H2SO4, N/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
Answer
C
Question. Which of the following concentration unit is independent of temperature ?
(a) Normality
(b) Molarity
(c) Formality
(d) Molality
Answer
D
Question. Which of the following factor do not affect solubility of solid solute in liquid ?
(a) Temperature
(b) Pressure
(c) Nature of solute
(d) All of these
Answer
B
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
Answer
D
Question. 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
(a) Less than the theoretical weight
(b) More than the theoretical weight
(c) Same as the theoretical weight
(d) None of these
Answer
B
Question. At the state of dynamic equilibrium, for solute + solvent ⇌ solution.
(a) Rate of dissolution = Rate of unsaturation.
(b) Rate of dissolution = Rate of unsaturation.
(c) Rate of dissolution = Rate of saturation
(d) Rate of crystallization = Rate of saturation.
Answer
B
Question. The statement “If 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere, 0.006 moles will be dissolved under a pressure of 2 atmospheres”, illustrates
(a) Dalton’s law of partial pressure
(b) Graham’s law
(c) Raoult’s law
(d) Henry’s law
Answer
D
Question. According to Henry’s law, the amount of gas that will dissolve in blood plasma or any other liquid is determined by which of these factor?
(a) Solubility of the gas in the liquid.
(b) The total pressure of the gas mixture .
(c) pH of the liquid.
(d) The osmotic pressure of the gas mixture.
Answer
A
Question. Henry’s law constant of oxygen is 1.4 × 10–3 mol. lit–1. atm–1 at 298 K. How much of oxygen is dissolved in 100 ml at 298 K when the partial pressure of oxygen is 0.5 atm?
(a) 1.4 g
(b) 3.2 g
(c) 22.4 mg
(d) 2.24 mg
Answer
D
Question. At equillibrium the rate of dissolution of a solid solute in a volatile liquid solvent is ______.
(a) less than the rate of crystallisation.
(b) greater than the rate of crystallisation.
(c) equal to the rate of crystallisation.
(d) zero
Answer
C
Question. 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 ______.
(a) Crystallization, dissolution.
(b) Dissolution, saturation.
(c) Saturation, crystallization.
(d) Dissolution, crystallization.
Answer
D
Question. A beaker contains a solution of substance ‘A’. Precipitation of substance ‘A’ takes place when small amount of ‘A’ is added to the solution. The solution is ______.
(a) saturated
(b) supersaturated
(c) unsaturated
(d) concentrated
Answer
B
Question. Which of the following statements is incorrect?
(a) A solution in which no more solute can be dissolved at the same temperature and pressure is called a saturated solution.
(b) An unsaturated solution is one in which more solute can be dissolved at the same temperature.
(c) The solution which is in dynamic equilibrium with undissolved solute is the saturated solution.
(d) The minimum amount of solute dissolved in a given amount of solvent is its solubility.
Answer
D
Question. 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 ?
(a) Sugar crystals in cold water.
(b) Sugar crystals in hot water.
(c) Powdered sugar in cold water.
(d) Powdered sugar in hot water.
Answer
D
