Assertion : When 'a' mL of a 0.1 molal urea solution is mixed with another 'b' mL of 0.1 molal glucose

                   samples prior to mixing but if 'a' mL of 0.1 molal urea is mixed with 'b' mL of 0.1 molal HF

                   solution, the boiling point of the solution is no different from the boiling points of the

                   the boiling point of the mixture is different from the boiling points of the separate

                   samples.

Reason : HF is an electrolyte (weak) whereas glucose is a non electrolyte.

  1. If both the assertion and the reason are true and the reason is a correct explanation of the assertion
  2. If both the assertion and reason are true but the reason is not a correct explanation of the assertion
  3. If the assertion is true but the reason is false
  4. If both the assertion and reason are false
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The equal weight of a solute is dissolved in an equal weight of two solvents A and B and formed a very dilute solution. The relative lowering of vapour pressure for solution B has twice the relative lowering of vapour pressure for solution A. If MA and MB are the molecular weights of solvents A and B respectively, then:

  • MA = MB

  • MB = 2MA

  • MA = 4MB

  • MA = 2MB

Consider the following liquid-vapor equilibrium 
Liquid  ↔  Vapour 
Which of the following relation is correct?
  • \(\frac{dlnp}{dT}=\frac{-\Delta H_v}{RT}\)
  • \(\frac{dlnp}{dT^2}=\frac{-\Delta H_v}{T^2}\)
  • \(\frac{dlnp}{dT}=\frac{\Delta H_v}{RT^2}\)
  • \(\frac{dlnG}{dT^2}=\frac{-\Delta H_v}{RT^2}\)
For an ideal solution, the non zero value will be for-
  •   \(\Delta H_{mix}\)
  •   \(\Delta S_{mix}\)
  •   \(\Delta V_{mix}\)
  •   \(\Delta P=P_{\text{observed}}-P_{\text{Raoult}}\)

The boiling point of 0.2 mol kg-1 solution of X in water is greater than equimolal solution of Y in water.
 
The correct statements in this case is-
 



 

 
  • X is undergoing dissociation in water.
  • Molecular mass of X is greater than the molecular mass of Y.
  • Molecular mass of X is less he molecular mass of y.
  • Y is undergoing dissociation in water while X undergoes no change.

    • Of the following 0.10m aqueous solutions, the one will exhibit the largest freezing point depression is-
    The freezing point depression constant for water is -1.86°C m-1. If 5.00 g Na2SO4 is dissolved in 45.0 g H2O, the freezing point is changed by -3.82°C. The van’t Hoff factor for Na2SO4 is-

    A solution containing 10g per dm3 of urea (molecular mass = 60g mol-1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is -

    During osmosis, the flow of water through a semi-permeable membrane is -

    The mixture that forms maximum boiling azeotrope is-

    C6H6 freezes at 5.5°C. At what temperature will a solution of 10.44 g of C4H10 in 200 g of C6H6 freeze ? Kf (C6H6) = 5.12°C/m

    The Henry's law constant for the solubility of N2 gas in water at 298 K is 1.0 × 105 atm. The mole fraction of N2 in air is 0.8. The number of moles of N2 from air dissolved in 10 moles of water at 298 K and 5 atm pressure is-        

    If the relative decrease in vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol of H2O, then percentage ionisation of NaCl will be -

    Boiling of dil. HCl acid does not increase its concentration beyond 22.2 per cent because hydrochloric acid:

    A 500 g toothpaste sample has 0.4 g fluoride concentration. The fluoride concentration in terms of ppm will be -

     The correct statement regarding a solution of two component A and B exhibiting positive deviation from idea behavior is -

     The correct sequence of order of increasing solubility in the n-octane is-

    17.4% (w/v) K2SO4 solution at 27°C is isotonic to 5.85% (w/V) NaCl solution at 27°C. lf

    NaCl is 100% ionised, the % ionisation of K2SO4 in aqueous solution is-

    [At wt. of K= 39,Na =23] :-

    The vapor pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in the vapor phase in contact with an equimolar solution of benzene and toluene is:

    The mixture shows positive deviation from Raoult's law is-

    The freezing point of 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 upto two decimal places) :

    For a solution, the plot of osmotic pressure (π) versus the concentration (c in mol L-1) gives a straight line with slope 310R where 'R' is the gas constant. The temperature at which osmotic pressure measured is -

    For the dissociation of PCl5 into PCl3 and Cl2 in gaseous phase reaction, if d is the observed vapour density and D the theoretical vapour density with 'a' as degree of dissociation. Variation of D/d with 'a' is given by which graph

    At 100°C the vapour density of nitrogen peroxide (N2O4) is 26.8. The percentage dissociation into NO2 molecules is

    The vapour density of N2O4 at a certain temperature is 30. What is the percentage dissociation of N2O4 at this temperature?

    What is the correct sequence of active masses in increasing order in gaseous mixture, containing one gram per litre of each of the following?

    I. NH3

    II. N2

    III. H2

    IV. O2

    Select the correct answer using the codes given below:

    When a saturated solution of sodium chloride is heated, it 

    The graph among the following that represents Henry's Law is -

     


     

    ln liquid CCl4 which of the following has maximum solubility?

    Which of the following represents a metastable system?
    0:0:1


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