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How muCHM molecular mass of NaCl is obta...

How muCHM molecular mass of `NaCl` is obtained experimentally using colligative properties ?

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As concentration of particles in the solution is doubled, value of colligative property is double than expected value and hence molecular mass is halved, i.e. observed molecular mass = 58.5/2 = 29.25
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The molecular mass of sodium chloride obtained by using a colligative property is

Explain giving examples the term 'colligative molality'. Why do we sometimes get abnormal molecular masses of the substances using colligative properties of the solution? The freezing point depression of 0.1 molal solution of benzoic acid in benzene is 0.526K . For benzene K_(f) is 5.12K kg "mol"^(-1) . Calculate the value of van't Hoff factor for benzoic acid in benzene. What conclusion can you draw about the molecular state of benzoic acid in benzene?

Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . van't Hoff coefficient 'g' for 100% dissociated NaCl solution is:

Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . The maximum elevation in b.pt. is noticed in :

Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . van,t Hoff factor (i) for dimerisation of benzoic acid in water, assuming 30% degree of association is:

Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . The degree of dissociation of electrolyte A_(x)B_(y) is given by the relation:

Colligative properties i.e., the properties of solution which depends upon the number pf aprticles present in solution are osmotic pressure, depression in freezing point, elevation in boiling point and lowering in vapour pressure. Experimental values of colligative properties for electroetically because electrolytes dissociates to furnish more ions in solution. On the other hand experimentally obtained values of colligative properties for associating nature of solute ate lower than those obtained theoretically. The ratio of experimantal colligative properties to theoretical colligative properties is called as van't Hoff factor (i) . The correct order of osmotic pressure for the solutions : (I) 1N urea , (II) 1N NaCl (III) 1N Na_(2)SO_(4) , (IV) 1N Na_(3)PO_(4) is:

Colligative properties of solution depend upon the number of particles present in solution. Experimental values colligative properties for electrolytes are always higher than these obtained theoretically because electrolyte dissociates to furnish more ions in solution. The ration of experimental values to theoretical values is called as van't Hoff factor (i) . The correct order of freezing point for the following, each are 1 molal solutions in water and take alpha = 1 : (i) Urea , (ii) NaCl (iii) Na_(3)PO_(4) , (iv) Na_(2)SO_(4)

A: Observed molecular mass of CaCl_2 determined by any colligative property is less than ideal molecular mass. R: CaCl_2 ionised in water as it is strong electrolyte.

PRADEEP-SOLUTIONS-ADDITIONAL QUESTIONS (VERY SHORT ANSWER QUESTIONS)
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  2. What are isotonic solutions ? Give one example .

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  3. What is van't Hoff equation for dilute solution?

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  7. Define osmotic pressure.

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  9. Define molal elevation constant or ebullioscopic constant?

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  10. Define molal depression constant or cryoscopic constant.

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  12. Between 2 M glucose solution and 1 M glucose, which one has a lower fr...

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  13. What is an antifreeze?

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  14. How muCHM molecular mass of NaCl is obtained experimentally using coll...

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  15. How is the colligative property of solution changed when a solute in a...

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  16. Calculate the value of van't Hoff factor for a dilute solution of K(2)...

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  17. Arrange the following solutions in increasing order of their van't Hof...

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  18. Give an example of a compound in which hydrogen bonding results in the...

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  19. When is the value of van't Hoff factor more than one?

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