Experimental) Ideal) Compound ATr of a mol of cmpd in ATr of a mol of cmpd in St

Question

Experimental) Ideal) Compound ATr of a mol of cmpd in ATr of a mol of cmpd in Strong, Weak or Nonelectrolyte 1 kg of H20 1.86 1.85 1.95 1.98 3.45 3.53 3.84 5.47 1 kg of H20 CoH 120 (NH2)2CO NH3 CH CO2H KI KBr do not respond do not respond H,so,353 K2SO4 a) If each of the solutions is prepared by adding 1 mole of compound to 1 kg of water why does each have a different T? b) Determine the ideal Tr for the compounds in the table above, except NH3 and COOH, why can't we determine an ideal freezing point for NH, and CH, CO H? c) why does the ideal AT, differ from the Tf experimental? 1314 1.1515

Explanation / Answer

Answer – b) Colligative properties depend on the solute exclusively. Various colligative properties for example, freezing point depression, elevation in boiling point, etc, are depending on the number of solute particles present in the solution.

Number of particles of the solute is written in terms of moles of solute. So the calculation of freezing point depression is directly proportional to the molality ( mol solute / mass of solvent in kg )

Mathematical expression of calculation of the depression in freezing point as follow:

Tf = i*m*kf

i is Vant hoff factor which gives number of solute particles formed from 1 one molecule of solute.

Kf is freezing point constant of solvent.

Kf is the change in temperature of solvent per kg of the solvent. As the number of particles of solute increase then there is increase difference in freezing point of the solution and solvent. This happens when we provide the heat to the solution then some of it heat is taken by the solute particles.

But this is does obey for all the solute since solute particles do not behave ideally in solution. For example, NH3 when we have NH3 molecule in the solution then it forms ammonium ion and OH- ion due to its basic nature.

Acetic acid also forms H3O+ and acetate ion in the solution which then is responsible for the deviation from the one which behaves according to the equation given above.

So there is not any response from such compound. And we cannot predict change in T for such compound

The (NH2)2CO is urea and it is nonpolar. The urea is not form the ions, so it is non electrolyte.

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