A 135-mL sample of a 10.0 M ethylene glycol \(\mathrm{(C_2H_6O_2)}\) solution is diluted to 1.50 L. What are the freezing and boiling points of the final solution? (Assume a density of 1.05 g/mL for the final solution.)

Equation Transcription:

Text Transcription:

(C_2H_6O_2)

Solution 124 P:

Here, we are going to calculate the boiling point and freezing point of the final solution .

Step 1: Calculation of the strength of the final solution by using dilution equation.

M1V1= M2V2 ------(1)

Where, M1 and V1 are Molarity and volume of the initial solution whereas M2 and V2 are the Molarity and volume of the solution.

From the Question,

It is given that,

M1 (initial Molarity) =10 M

V1 (initial volume) = 135.0 mL

M2 (final Molarity) =?

V2 (initial volume) = 1.50L =1500 mL

Thus, from equation (1)

M1V1= M2V2 ------(1)

M2 = M1V1/V2

= = 0.9 M

The final strength of the solution is 0.9 M = 0.9 mol/L

1 L solution contains = 0.9 mol

1.50 L solution contains = 0.9 mol x 1.50L/1 L = 1.35 mol ethylene glycol