Home
Class 12
CHEMISTRY
If quantities DeltaT(f), DeltaTb ,Deltap...

If quantities `DeltaT_(f), DeltaT_b ,Deltap` and `pi` without subscript refer to the electrolyte solution and these with subscript refer to the non-electrolyte solution then which one is incorrect?

A

`i=(DeltaT_(f))/((DeltaT_(f))0)`

B

`i=(DeltaT_(b))/((DeltaT_(b))0)`

C

`i=(DeltaP)/((P^(@))0)`

D

`i = (pi)/((pi)_(0))`

Text Solution

Verified by Experts

The correct Answer is:
C
`i = (Delta P)/((Delta P)_(0)) = (Delta P//P^(@))/((Delta P)_(0)//P^(@))`
Promotional Banner

Topper's Solved these Questions

  • DILUTE SOLUTION AND COLLIGATIVE PROPERTIES

    P BAHADUR|Exercise Exercise 3B Objectice Problems|1 Videos

  • DILUTE SOLUTION AND COLLIGATIVE PROPERTIES

    P BAHADUR|Exercise Exercise 9 Advanced Numerical|12 Videos

  • CHEMICAL KINETICS

    P BAHADUR|Exercise Exercise 9|13 Videos

  • ELECTROCHEMISTRY

    P BAHADUR|Exercise Exercise (9) ADVANCED NUMERICAL PROBLEMS|36 Videos

Similar Questions

Explore conceptually related problems

How are DeltaT_(b) and DelatT_(f) related to the molar mass of the solute ?

Addition of non-volatile solute to a solvent always inceases the colligative properties such as osmotic pressure, DeltaP, DeltaT_(b) and DeltaT_(f) . All these colligative properties are direactly propertional to molality if solutions are dilute. The increase in colligative properties on addition of non-volatile solute is due to incease in number of solute particles. For different aqueous solutions of 0.1 N NaCl, 0.1 N urea, 0.1 N Na_(2)SO_(4) and 0.1 N Na_(3)PO_(4) solution at 27^(@)C , the correct statement are : (P) The order of osmotic pressure is, NaCl gt Na_(2)SO_(4) gt Na_(3)PO_(4) gt urea (Q) pi = (DeltaT_(b))/(K_(b)) xx ST for urea solution (R) Addition of salt on ice increases its melting point (S) Addition of salt on ice brings in melting earlier

Addition of non-volatile solute to a solvent always inceases the colligative properties such as osmotic pressure, DeltaP, DeltaT_(b) and DeltaT_(f) . All these colligative properties are direactly propertional to molality if solutions are dilute. The increase in colligative properties on addition of non-volatile solute is due to incease in number of solute particles. For different aqueous solutions of 0.1 N NaCl, 0.1 N urea, 0.1 N Na_(2)SO_(4) and 0.1 N Na_(3)PO_(4) solution at 27^(@)C , the correct statement are : 1g mixture of glucose and urea present in 250 mL aqueous solution shows an osmotic pressure of 0.74 atm at 27^(@) C . Assuming solution to be dilture, which are correct ? (P) Percentage of urea in solute mixture is 17.6 (Q) Relative lowering in vapour pressure of this solutions is 5.41 xx 10^(-4) . (R) The solution will boil at 100.015^(@)C , if K_(b) of water is 0.5 K "molality"^(-1) (S) If glucose is replaced by same amount of sucrose, the solution will show higher osmotic pressure at 27^(@)C (T) If glucose is repalced by same amount of NaCl , the solution will show lower osmotic pressure at 27^(@)C .

A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. Dissolution of a non-volatile solute into a liquid leads to

A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. A liquid possessing which of the following characteristics will be most suitable for determining the molecular mass of a compound by cryoscopic measurements?

Ratio of (DeltaT_(b))/(K_(b)) of 10 g AB_(2) and 14g A_(2)B per 100 g of solvent in their respective, solution ( AB_(2) and A_(2)B both are non-electrolytes) is 1 mol/kg in both cases. Hence, atomic wt. of A and B are respectively.