In an experiment, calcium carbonate reacted with different volumes of hydrochloric acid in water. One of the products formed dur
ing the experiment was carbon dioxide. The time taken for 0.89 mL of carbon dioxide to form was recorded. A partial record of the experiment is shown. Experimental Record Flask Mass of Calcium Carbonate Volume of HCl Volume of Water Time 1 4.0 g 25 mL 0 mL 11.2 seconds 2 4.0 g 20 mL 5 mL 3 4.0 g 15 mL 10 mL 4 4.0 g 10 mL 15 mL
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INFORMATION:
We know that:
- pure water boils at 99.8 degrees celcius
And we must calculate the expected elevated boiling point of a solution of 2.50g of CaCl2, in 50.0mL (i.e., 50.0g) of H2O
STEP BY STEP EXPLANATION:
To calculate it, we need to use that:
Boiling point of solution = boiling point of pure solvent + boiling point elevation (ΔTb)
The elevation in boiling point (ΔTb) is proportional to the concentration of the solute in the solution. It can be calculated via the following equation.
Where,
- i is the Van’t Hoff factor
- Kb is the ebullioscopic constant
- m is the molality of the solute
From given information, we know that:
- i = 3
Now, the ebullioscopic constant (Kb) is often expressed in terms of °C * kg * mol^-1. The value of Kb for water is 0.512.
So, kb = 0.512 °C * kg * mol^-1
Then, we must calculate the molality
So, m = 0.45 mol/kg
Replacing the values in the formula for ΔTb
Finally, the expected elevated boiling point of the solution would be
ANSWER:
The expected elevated boiling point of the solution is 100.49 °C