Question

The molar mass of a nonelectrolyte is 58.0 g/mol. Determine the boiling point of a solution containing 35.0 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.7258C.

Short answer

The boiling point of the solution is $100.24°C$.

Step-by-step solution

Step 1:

The equation for boiling point elevation is $\Delta T=K_b\times m_{solute}$

Molar mass =58.0g/mol

Mass (nonelectrolyte) =35.0g

Mass ( $H_{2}O$)=6000.0g

Step 2:

Calculate the boiling point of the solution.

$\Delta T=0.512°Ckg/mol\times \frac{35.0g}{0.600kg\times 58.0g/mol}=0.515°C$

The boiling point of the solution is $99.725°C+0.515=100.24°C$