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Which formula from the following is used to determine molar mass of solute from depression freezing point?
The correct formula for determining molar mass from freezing point depression is M₂ = (1000 × ΔTf × W₁) / (Kf × W₂).
What is molar mass of solute if 50 gram of it in 150 gram solvent has boiling point elevation of 5.54 K? (K_b = 2.77 K kg mol⁻¹)
Using the formula ΔTb = Kb × molality, the molar mass is calculated as 166.6 g mol⁻¹.
What is the value of molal elevation constant of a solvent if 50 g solute (molar mass 111) when dissolved in 150 g of it has elevation in boiling point of 8.3 K?
The molal elevation constant is calculated as 1.86 K kg mol⁻¹ using the given data.
The solution containing 6 g urea (molar mass 60) per dm³ of water and another solution containing 9 g of solute A per dm³ water freezes at same temperature. What is molar mass of A?
The molar mass of solute A is calculated as 180 g mol⁻¹ based on freezing point depression.
Calculate osmotic pressure exerted by a solution containing 0.822 g of solute in 300 mL of water at 300 K. (Molar mass of solute = 340 g mol⁻¹, R=0.0821 L atm K⁻¹ mol⁻¹)
The osmotic pressure is calculated as 0.1 atm using the formula Π = nRT/V.
What type of following solution is obtained from amalgam of mercury with sodium?
An amalgam of mercury with sodium is a liquid-in-solid solution.
What is vapour pressure of solution containing 0.1 mole solute dissolved in 1.8 × 10⁻² kg H₂O? (P₁° = 24 mm Hg)
The vapor pressure of the solution is calculated as 18.12 mm Hg using Raoult's law.
In which of the following salts, the solubility increases appreciably with increase in temperature
The solubility of KBr increases appreciably with temperature.
What is the boiling point of 0.5 molal aqueous solution of glucose boils if 0.1 molal aqueous solution of glucose boils at 100.16°C?
The boiling point is calculated as 100.62°C using the boiling point elevation formula.
The vapour pressure of a solvent decreases by 2.5 mm Hg by adding a solute. What is the mole fraction of solute? (Vapour pressure of pure solvent is 250 mm Hg)
The mole fraction of solute is calculated as 0.01 using Raoult's law.
Molal depression constant for a liquid is 2.77°C kg mol⁻¹, in Kelvin scale it’s value is
The value in Kelvin is 2.77 K kg mol⁻¹.
Which of the following formulae is used to calculate molar mass of solute from elevation in boiling point?
The correct formula is M₂ = (1000 × ΔTb × W₂) / (Kb × W₁).
Calculate solubility of a gas in H₂O at 0.75 bar if Henry’s law constant for the gas is 7 × 10⁻⁴ mol L⁻¹ bar⁻¹?
The solubility is calculated as 5.25 × 10⁻⁴ mol L⁻¹ using Henry's law.
What is ΔTf for a solution containing 5 g sucrose in 100 g solvent? (Molar mass of sucrose = 342 g mol⁻¹ and Kf for solvent = 14.7 K kg mol⁻¹)
The freezing point depression ΔTf is calculated as 1.47 K.
Which of the following solutions does not flow in either direction, when separated by semipermeable membrane? (Molar mass: glucose = 180, urea = 60)
The solution with 6 g urea dm⁻³ and 36 g glucose dm⁻³ does not flow in either direction.
Which of the following formulae is used to calculate molar lowering of vapour pressure from relative lowering?
The correct formula is M₂ = (W₁ / W₂) × (M₁) × (ΔP / P₁°).
Calculate solubility of a gas in water at 1 bar, If Henry’s law constant for the gas is 7 × 10⁻⁴ mol L⁻¹ bar⁻¹?
The solubility is calculated as 7.0 × 10⁻⁴ mol L⁻¹ using Henry's law.
A solution of 6 g of solute in 100 g of water boils at 100.52°C. The molal elevation constant of water is 0.52 K kg mol⁻¹. What is molar mass of solute?
The molar mass of the solute is calculated as 120 g mol⁻¹.
If vapour pressure of pure solvent and solution are 240 and 216 mm Hg respectively then mole fraction of solvent in solution is
The mole fraction of solvent is calculated as 0.6 using Raoult's law.
What is cryoscopic constant of water if 5 g of glucose in 100 g of water has depression in freezing point 2.15 K? (Molar mass of glucose = 180)
The cryoscopic constant of water is calculated as 0.52 K kg mol⁻¹.
What is vapour pressure of a solution containing 2.4 g urea in 10.8 g of water? (P₁° = 400 mm Hg, atomic mass of: C=12, H=1, O=16, N=14)
The vapor pressure of the solution is calculated as 210 mm Hg using Raoult's law.
Which of the following solutions shows negative deviation from Raoult’s law?
Ethanol + Acetone shows negative deviation from Raoult’s law.
Which among the following salts have appreciable increase in solubility with increasing temperature?
NaNO₃ has an appreciable increase in solubility with increasing temperature.
What is vapour pressure of a solution containing 18 g glucose in 162 g of water? (P₁° = 32 mm Hg and molar mass glucose = 180)
The vapor pressure of the solution is calculated as 22.2 mm Hg using Raoult's law.
If molal elevation constant of water is 0.51 K kg mol⁻¹, calculate boiling point of decimolar aqueous solution of glucose? (Boiling point of water = 100°C)
The boiling point is calculated as 100.051°C using the boiling point elevation formula.
Hydrogen in palladium is an example of a solution of
Hydrogen in palladium is an example of a gas-in-solid solution.
What is vapour pressure of a solution containing 6 g urea in 16.2 g of water? (P₁° = 24 mm Hg, molar mass of urea = 60 g mol⁻¹)
The vapor pressure of the solution is calculated as 21.6 mm Hg using Raoult's law.
The molar mass of solute is double that of solvent and weight of solute is (1/10)th that of solvent in a solution. If vapour pressure of solvent is 200 mm Hg, what is lowering in vapour pressure of solution?
The lowering in vapor pressure is calculated as 10 mm Hg.
Which of the following statements is correct for boiling point of a liquid?
The correct statement is that the boiling point is the temperature at which vapor pressure equals the applied pressure.
Henry’s law constant for CH₃Br is 0.16 mol L⁻¹ bar⁻¹ at 298 K. What pressure is required to have solubility of 0.08 mol L⁻¹?
The required pressure is calculated as 0.24 bar using Henry's law.
Which of the following solutions shows positive deviation from Raoult’s law?
Ethanol + Acetone shows positive deviation from Raoult’s law.
What is vapour pressure of a solution containing 0.1 mol of non-volatile solute dissolved in 16.2 g of water? (P₁° = 32 mm Hg)
The vapor pressure of the solution is calculated as 18.1 mm Hg using Raoult's law.
What is boiling point of a decimolar aqueous solution of glucose if molal elevation constant for water is 0.52°C kg mol⁻¹?
The boiling point is calculated as 100.52°C using the boiling point elevation formula.
What is vapour pressure of a solution when 2 mol of a non-volatile solute are dissolved in 20 mol of water? (P₁° = 32 mm Hg)
The vapor pressure of the solution is calculated as 6 mm Hg using Raoult's law.
If 6 g of solute dissolved in 100 g of water lowers the freezing point by 0.93 K. What is molar mass of solute? (Kf = 1.86 kg mol⁻¹)
The molar mass of the solute is calculated as 60 g mol⁻¹ using freezing point depression.
5 g sucrose (molar mass = 342) is dissolved in 100 g of solvent, decreases the freezing point by 2.15 K. What is cryoscopic constant of solvent?
The cryoscopic constant of the solvent is calculated as 4.30 K kg mol⁻¹.
What is Henry’s law constant if solubility of a gas in water at 298 K and 1 bar pressure is 7 × 10⁻⁴ mol L⁻¹?
The Henry's law constant is calculated as 7.0 × 10⁻⁴ mol L⁻¹ bar⁻¹.
Which of the following formulae is used to obtain depression in freezing point?
The correct formula for freezing point depression is ΔTf = Tf₀ - Tf.
What is vapour pressure of solution containing 1.8 g glucose in 16.2 g water? (P₁°=24 mm Hg and Molar mass of glucose = 180 g mol⁻¹)
The vapor pressure of the solution is calculated as 15.7 mm Hg using Raoult's law.
What is the freezing point of 1 molal aqueous solution of a non-volatile solute? (Kf = 1.86 K kg mol⁻¹, Tf₀ for water = 0°C)
The freezing point is calculated as -1.86°C using the freezing point depression formula.
Air is an example of a solution of
Air is an example of a gas-in-gas solution.
What is vapour pressure of solution containing 1 mole of a non-volatile solute in 36 g of water? (P₁°=400 mm Hg)
The vapor pressure of the solution is calculated as 240 mm Hg using Raoult's law.
Which of the following solutions behaves nearly as an ideal solution?
Benzene + toluene behaves nearly as an ideal solution.
The solution containing 6 g urea (molar mass 60) per dm³ of water and another containing 18 g of solute A per dm³ of water freezes at same temperature. What is the molar mass of A?
The molar mass of solute A is calculated as 120 g mol⁻¹ based on freezing point depression.
Vapour pressure of pure solvent and solution are 120 and 108 mm Hg respectively. What is mole fraction of solvent?
The mole fraction of solvent is calculated as 0.4 using Raoult's law.
Henry’s law constant for CH₃Br is 0.16 mol L⁻¹ bar⁻¹ at 298 K. What is solubility of CH₃Br in water at 380 mm Hg?
The solubility is calculated as 0.24 mol L⁻¹ using Henry's law.
The solution containing 3 g urea (molar mass 60) per dm³ of water and another solution containing 4.5 g of solute A per dm³ of water boils at same temperature, then what is molar mass of A?
The molar mass of solute A is calculated as 120 g mol⁻¹ based on boiling point elevation.
Vapour pressure of solution and of pure solvent are P₁ and P₁° respectively. If P₁ / P₁° is 0.15, find the mole fraction of solute
The mole fraction of solute is calculated as 0.15 using Raoult's law.
According to Raoult’s law mole fraction of solute in solution is given by formula
The mole fraction of solute is given by ΔP / P₁° according to Raoult's law.
Which of the following conditions is obeyed by an ideal solution?
An ideal solution is characterized by comparable interactions between solute and solvent molecules.
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