Two aqueous solutions are prepared: 1.00 m Na2CO3 and 1.00 m LiCl. Which of the following statements is true?
A. The Na2CO3 solution has a higher osmotic pressure and higher vapor pressure than the LiCl solution.
B. The Na2CO3 solution has a higher osmotic pressure and higher boiling point than the LiCl solution.
C. The Na2CO3 solution has a lower osmotic pressure and lower vapor pressure than the LiCI solution.
D. The Na2CO3 solution has a lower osmotic pressure and higher boiling point than the LiCl solution.
E. None of these statements is true.

The solution has a higher osmotic pressure and higher boiling point than LiCl solution.

Explanation:

As concentrations of two aqueous solutions are same therefore we can write:

                                , and

where , and are lowering of vapor pressure, elevation in boiling point and osmotic pressure of solution respectively. is van't hoff factor.

= total number of ions generated from dissolution of one molecule of a substance (for strong electrolyte).

Here both and LiCl are strong electrolytes.

So, and

Hence, lowering of vapor pressure, elevation in boiling point and osmotic pressure will be higher for solution.

Therefore the solution has a higher osmotic pressure and higher boiling point than LiCl solution.

k thx :)

Explanation: