Solution Chemistry
NEET Questions

The mixture which shows positive deviation from Raoult’s law is

Which of the following statements is correct regarding a solution of two components A and B exhibiting positive deviation from ideal behavior?

An ideal solution is formed when its components

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 solution of acetone in ethanol

An aqueous solution is 1.00 molal in KI. Which change will cause the vapor pressure of the solution to increase?

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

The mole fraction of the solute in one molal aqueous solution is

A 5% solution of cane sugar (mol. wt. = 342) is isotonic with 1% solution of a substance X. The The molecular weight of X is

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

All form ideal solutions except

Which one of the following is incorrect for ideal solution?

Blood cells retain their normal shape in solution which are

The van’t Hoff factor I for a compound which undergoes dissociation in one solvent and association in another solvent is respectively

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.

The vapor 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 vapor pressure is to be 20 mm of mercury?

What is the mole fraction of the solute in a 1.00 m aqueous solution?

From the colligative properties of solution, which one is the best method for the determination of molecular weight of proteins and polymers?

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 solution has a 1: 4-mole ratio of pentane to hexane. The vapor 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 vapor phase would be

The concentration unit, independent of temperature, would be

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

In water-saturated air, the mole fraction of water vapor is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is

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.

The vapor pressure of two liquids P and Q are 80 and 60 torr, respectively. The total vapor pressure of the solution obtained by mixing 3 moles of P and 2 mol of Q would be

Which one is a colligative property?

The relationship between osmotic pressure at 273 K when 10 g glucose (p₁), 10 g urea (p₂), and 10 g sucrose (p₃) are dissolved in 250 mL of water is

How many grams of CH₃OH should be added to water to prepare 150 mL solution of 2 M CH₃OH?

If the molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be

The vapour pressure of CCl₄ at 25°C is 143 mm Hg. If 0.5 g of a non-volatile solute (mol. weight = 65) is dissolved in 100 g CCl₄, the vapour pressure of the solution will be

If 0.1 M solution of glucose and 0.1 M solution of urea are placed on two sides of the semipermeable membrane to equal heights, then it will be correct to say that

Concentrated aqueous sulphuric acid is 98% H₂SO₄ by mass and has a density of 1.80 g mL^–1. The volume of acid required to make one liter of 0.1 M H₂SO₄ solution is

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)

The van’t Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is

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 solution containing components A and B follows Raoult’s law

2.5 liters of 1 M NaOH solution is mixed with another 3 liters of 0.5 M NaOH solution. Then find out the molarity of a resultant solution.

Of the following 0.10 m aqueous solutions, which one will exhibit the largest freezing point depression?

How many g of dibasic acid (mol. weight 200) should be present in 100 mL of the aqueous solution to give a strength of 0.1 N?

According to Raoult’s law, the relative lowering of vapour pressure for a solution is equal to

For an ideal solution, the correct option is

The mixture that forms a maximum boiling azeotrope is

Which of the following is dependent on temperature?

The relative lowering of the vapor pressure is equal to the ratio between the number of

Pure water can be obtained from seawater by

Which condition is not satisfied by an ideal solution?

The boiling point of 0.2 mol kg–1 solution of X in water is greater than the equimolal solution of Y in water. Which one of the following statements is true in this case?

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 up to two decimal places)

During osmosis, flow of water through a semipermeable membrane is

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.

The vapor 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?

What is the molarity of H₂SO₄ solution, which has a density of 1.84 g/cc at 35°C and contains 98% by weight?

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.

Which of the following statements about the composition of the vapor over an ideal 1: 1 molar mixture of benzene and toluene is correct? Assume that the temperature is constant at 25°C. (Given, vapor pressure data at 25°C, benzene = 12.8 kPa, toluene = 3.85 kPa)

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_f for water is 1.86°C/m, the freezing point of the solution will be

The vapor 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 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

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