Which of these aqueous solutions would be expected to have the highest boiling point?

a. 0.100 m cacl2

b. 0.200 m naoh

c. 0.050 m k2so4

d. 0.050 m al2(so4)3

e. 0.200 m ch3oh

0.200 m NaOH has the highest boiling point (option B)

Explanation:

Step 1: Data given

The elevation of boiling point is proportional to the number of ions in solution.

The van't Hoff factor, i, is a measure of how many ions are produced from one molecule of the solute. For nonelectrolytes,  i = 1).

We can compute the product of the van't Hoff factor and the molality for each of the solutes in the list:

a. 0.100 m CaCl2

⇒ CaCl ⇒ Ca^2+ + 2Cl-  : van't Hoff factor = 3

0.100 * 3 = 0.300

b. 0.200 m NaOH

⇒ NaOH ⇒ Na+ + OH-   : Van't Hoff factor = 2

0.200 * 2 = 0.400

c. 0.050 m K2SO4

⇒ K2SO4 = 2K+ + SO4^2-   : Van't Hoff factor = 3

0.050 * 3 = 0.150

d. 0.050 m Al2(SO4)3

⇒ Al2(SO4)3  ⇒ 2Al^3+ + 3SO4^2-   : Van't Hoff factor = 5

0.050 * 5 = 0.250

e. 0.200 m CH3OH

methanol is a non-emektrolyte  Van't hoff factor = 1

0.200 * 1 = 0.200

Since the highest result is from 0.200 m NaOH, means this has the highes boiling point. ( Option B) is correct)

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