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Sveta_85 [38]
3 years ago
10

Two aqueous solutions are prepared: 1.00 m Na2CO3 and 1.00 m LiCl. Which of the following statements is true?

Chemistry
1 answer:
svlad2 [7]3 years ago
7 0

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.

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