STANDARD Chemistry Solutions Class 12 Questions

Homogeneous mixture of two or more than two components is called

Which of the following is an example of gaseous solution?

What is the mole fraction of glucose in 10% w/W glucose solution?

What will be the mole fraction of ethanol in a sample of spirit containing 85% ethanol by mass?

How many Na⁺ ions are present in 100 mL of 0.25 M of NaCl solution?

The density of a solution prepared by dissolving 120 g of urea (mol. Mass = 60 u) in 1000 g of water is 1.15 g/mL. The molarity of this solution is

What will be the molality of a solution of glucose in water which is 10% w/W?

Concentration terms like mass percentage, ppm, mole fraction and molality do not depend on temperature. However, molarity is a function of temperature because

Solubility of a substance is its maximum amount that can be dissolved in a specified amount of solvent. It depends upon (i) nature of solute (ii) nature of solvent (iii) temperature (iv) pressure

The law which indicates the relationship between solubility of a gas in liquid and pressure is

According to Henry's law 'the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution'. For different gases the correct statement about Henry's constant is

The value of Henry's law constant for some gases at 293 K is given below. Arrange the gases in the increasing order of their solubility. He : 144.97 kbar, H₂ : 69.16 kbar, N₂ : 76.48 kbar, O₂ : 34.86 kbar

Henry's law constant for molality of methane in benzene at 298 K is 4.27 × 10⁵ mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg is

How much oxygen is dissolved in 100 mL water at 298 K if partial pressure of oxygen is 0.5 atm and Kₕ = 1.4 × 10⁻³ mol/L/atm?

3 moles of P and 2 moles of Q are mixed, what will be their total vapour pressure in the solution if their partial vapour pressures are 80 and 60 torr respectively?

For an ideal solution with pₐ > p_b, which of the following is true?

X, Y and Z in the above graph are

What are the conditions for an ideal solution which obeys Raoult's law over the entire range of concentration?

Intermolecular forces between n-hexane and n-heptane are nearly same as between hexane and heptane individually. When these two are mixed, which of the following is not true about the solution formed?

Which of the following solutions shows positive deviation from Raoult's law?

Which of the following solutions is an example of negative deviation from Raoult's law?

Study the figures given below and mark the correct statement.

Match the column I with column II and mark the appropriate choice.

What is the mass per cent of oxygen in ethanol?

The relative lowering in vapour pressure is proportional to the ratio of number of

A solution is prepared by adding 5 g of a solute 'X' to 45 g of solvent 'Y'. What is the mass per cent of the solute 'X'?

Vapour pressure of a pure liquid X is 2 atm at 300 K. It is lowered to 1 atm on dissolving 1 g of Y in 20 g of liquid X. If molar mass of X is 200, what is the molar mass of Y?

2.82 g of glucose is dissolved in 30 g of water. The mole fraction of glucose in the solution is

1 g of solute (molar mass = 50 g mol⁻¹) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molal elevation constant of the solvent is

What volume of water is to be added to 100 cm³ of 0.5 M NaOH solution to make it 0.1 M solution?

2 g of sugar is added to one litre of water to give sugar solution. What is the effect of addition of sugar on the boiling point and freezing point of water?

What weight of glycerol should be added to 600 g of water in order to lower its freezing point by 10°C? (Kf = 1.86°C m⁻¹)

A solution is made by dissolving 49 g of H₂SO₄ in 250 mL of water. The molarity of the solution prepared is

What will be the molarity of the solution in which 0.365 g of HCl gas is dissolved in 100 mL of solution?

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

What will be the molality of the solution made by dissolving 10 g of NaOH in 100 g of water?

10% solution of urea is isotonic with 6% solution of a non-volatile solute X. What is the molecular mass of solute X?

What will be the molarity of a solution, which contains 5.85 g of NaCl₍ₛ₎ per 500 mL?

Which of the following statements is not correct?

If 500 mL of a 5 M solution is diluted to 1500 mL, what will be the molarity of the solution obtained?

Why is the molecular mass determined by measuring colligative property in case of some solutes is abnormal?

If the concentration of glucose (C₆H₁₂O₆) in blood is 0.9 g L⁻¹, what will be the molarity of glucose in blood?

Which of the following will have same value of van't Hoff factor as that of K₄[Fe(CN)₆]?

What will be the molality of the solution containing 18.25 g of HCl gas in 500 g of water?

Arrange the following aqueous solutions in the order of their increasing boiling points. (i) 10⁻⁴ M NaCl (ii) 10⁻⁴ M Urea (iii) 10⁻³ M MgCl₂ (iv) 10⁻² M NaCl

If α is the degree of dissociation of Na₂SO₄, the van't Hoff's factor (i) used for calculating the molecular mass is

What will be the freezing point of a 0.5 m KCl solution? The molal freezing point constant of water is 1.86°C m⁻¹.

The van't Hoff factor of 0.005 M aqueous solution of KCl is 1.95. The degree of ionisation of KCl is

The elevation in boiling point of a solution of 9.43 g of MgCl₂ in 1 kg of water is (K_b = 0.52 K kg mol⁻¹, Molar mass of MgCl₂ = 94.3 g mol⁻¹)

The unit of ebullioscopic constant is