Question

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.

Answer 1

Answer:

The $Na_{2}CO_{3}$ 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:

                                $\Delta P\propto i$ , $\Delta T_{b}\propto i$ and $\pi \propto i$

where $\Delta P$, $\Delta T_{b}$ and $\pi$ are lowering of vapor pressure, elevation in boiling point and osmotic pressure of solution respectively. $i$ is van't hoff factor.

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

Here both $Na_{2}CO_{3}$ and LiCl are strong electrolytes.

So, $i(Na_{2}CO_{3})=3$ and $i(LiCl)=2$

Hence, lowering of vapor pressure, elevation in boiling point and osmotic pressure will be higher for $Na_{2}CO_{3}$ solution.

Therefore the $Na_{2}CO_{3}$ solution has a higher osmotic pressure and higher boiling point than LiCl solution.

Answer 2

Osmotic pressure is defined as the pressure exerted to prevent the backflow of solvent, whereas vapor pressure is defined as the pressure exerted by the vapors on the walls of a container in a closed system.

The $\text{Na}_2\text{CO}_3$ solution has higher osmotic pressure and boiling point than the LiCl solution.

The answer can be explained as:

• The concentrations of the aqueous solutions of the given solutions are equal, such that lowering of vapor pressure, elevation in boiling point, and osmotic pressure is directly proportional to dissociation of ions of one molecule of a strong electrolyte.

• The sodium carbonate and lithium chloride are the strong electrolytes, such that the van't Hoff factor for both the electrolytes are 3 and 2, respectively.

• The lowering of vapor pressure, osmotic, and boiling point will be higher for sodium chloride than the lithium chloride solution.

Thus, the sodium chloride will have higher osmotic pressure than lithium chloride.

To know more about osmotic pressure, refer to the following link:

https://brainly.com/question/12497098