Which one of the following is incorrect for ideal solution ?

Which gas when passed through dilute blood will impart a cherry red colour to the solution?

The vapour density of undecomposed N₂O₄ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to NO₂. The percent dissociation of N₂O₄ at the final temperature is: 

At 298 K, 500cm³ H₂O dissolved 15.30 cm³ CH₄(STP) under a partial pressure of methane of one atm. If Henry's law holds, what pressure is required to cause 0.001 mole methane to dissolve in 300cm³ water ?

The molal depression constant for water=1.85 deg/molal and for benzene is 5.12 deg/molal. If the ratio of the latent heats of fusion of benzene to water is 3:8, calculate the freezing point of benzene.

Which of the following colligative properties is associated with the concentration term 'molarity'?

The vapour pressure of a dilute aqueous solution of glucose is 750 mm of mercury at 373 K. The mole fraction of solute in the solution is-

Which one of the folowing pairs of solution can we expect to be isotonic at the same temperature-

The latent heat of vapourisation of water is 540 cal g^-1 at 100$°\mathrm{C}$. K_b for water is

1. 0.56 K.mole^-1

2. 1.86 K.mole^-1

Which of the following aqueous solution has osmotic pressure nearest to that an equimolar solution of K₄[Fe(CN)₆]?

The molar volume of liquid benzene (density= 0.877 g ml^-1) increases by a factor of 2750 as it vapourises at 20$°\mathrm{C}$. At 27$°\mathrm{C}$ when a non-volatile solute (that does not dissociate) is dissolved in 54.6cm3 of benzene, vapour pressure of this solution, is found to be 98.88 mm Hg. calculate the freezing point of the solution.

Given: Enthalpy of vapourisation of benzene(l)=394.57 Jg^-1. Enthalpy of fusion of benzene (l) = 10.06 kJ mol^-1 Molal depression constant for benzene=5.0 K kg mol^-1.

The depression in the freezing point of water when 10 g of CH₃CH₂CHClCOOH is added to 250 g of water is -K_a=1.4 X 10^-3, K_f=1.86K kg mol^-1

The ratio of the vapour pressure of a solution to the vapour pressure of the solvent is

Mole fraction of the component A in vapour phase is X₁ and mole fraction of component A in liquid mixture is X₂ then 

(${\mathrm{P}}_{\mathrm{A}}^0$ = vapour pressure of pure A; ${\mathrm{P}}_{\mathrm{B}}^0$= vapour pressure of pure B),

then total vapour pressure of the liquid mixture is-

pH of a 0.1 (M) monobasic acid is 2. Osmotic pressure at a given temperature T is-

The vapour pressure of pure water at 298K is 23.76mm. The vapour pressure of a solution of sucrose(C₁₂H₂₂O₁₁) in 5.56 moles of water is 23.392mm Hg. The mass of sucrose in the solution is

Among the following options, 0.1 M aqueous solution will have the lowest freezing point is-

The vapour pressure of toluene is 59.1 torr at 313.75 K and 298.7 torr at 353.15 K. Calculate, the molar heat of vaporisation.

The vapour pressure of pure liquid solvent A is 0.80 atm. When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm, mole fraction of the component B in the solution is-

Lowest boiling point among the following 0.1 (M) aqueous solution is -

a.  K₂SO₄

b. NaCl

c. Urea

d. Glucose

The boiling point of acetic acid is 118.1$°\mathrm{C}$ and its latent heat of vaporisation is 121 cal/gm. A solution containing 0.4344 gm anthracene in 44.16 gm acetic acid boils at 118.24$°\mathrm{C}$. What is the molecular wt. of anthracene ?

Which solution will have the highest boiling point ?

A 2.0% solution by weight of urea in water shows a boiling point elevation of 0.18 deg [Molecular weight of urea=60]. Calculate the latent heat of vaporization per gram of water.

A solution of 18 g of glucose in 1000 g of water is cooled to -0.2$°\mathrm{C}$. The amount of ice separating out from this solution is -

(K_fH₂O=1.86 K molal^-1)

The partial pressure of ethane over a saturated solution containing 6.56 X 10^-2 g of ethane is 1 bar. If the solution contains 5.00 X 10^-2 g of ethane, then what shall be the partial pressure of the gas.

In a dilute solution, any colligative property depends on 

An aqueous solution of 2 percent non volatile solute exerts a pressure of 1.004 bar at the boiling point of the solvent. What is the molecular mass of the solute ?

An aqueous solution of hydrochloric acid is-

1000 gm of 1 m sucrose solution in water is cooled to -3.534$°\mathrm{C}$. What weight of ice would be separated out at this temperature ? ${\mathrm{K}}_{\mathrm{f}}^{\text{'}}\left({\mathrm{H}}_2\mathrm{O}\right)=1.86 \mathrm{K} {\mathrm{mol}}^{-1}\mathrm{kg}.$

Osmotic pressure of equimolar solution of BaCl₂, NaCl and glucose will be in the order -