Compute the boiling point of this solution:
1.00*10^2g C10H8O6S2 (1,5-naphthalenedisulfonic acid) in 1.00*10^2g H2O (nonionizing solute)
The freezing point of H2O is Lowered 1.86 Celsius per mole of solute.
The boiling point of H2O is Raised 0.512 Celsius per mole of solute.
Do you have a question?
what is the boiling point of this solution.
1.8
To compute the boiling point of the solution, we need to consider the effect of the solute on the boiling point of water.
First, let's determine the number of moles of solute (C10H8O6S2) and water (H2O) in the solution using their respective masses.
Mass of C10H8O6S2 = 1.00 * 10^2 g
Molar mass of C10H8O6S2 = 1 * 12.01 + 8 * 1.01 + 6 * 16.00 + 2 * 32.07 = 254.25 g/mol
Number of moles of C10H8O6S2 = Mass of C10H8O6S2 / Molar mass of C10H8O6S2
= 1.00 * 10^2 g / 254.25 g/mol
= 0.393 mol
Similarly, the number of moles of H2O can be calculated as:
Number of moles of H2O = Mass of H2O / Molar mass of H2O
= 1.00 * 10^2 g / 18.02 g/mol
= 5.548 mol
Now, we can calculate the boiling point elevation caused by the solute, which is given as 0.512°C per mole of solute.
Boiling point elevation = Boiling point constant * Number of moles of solute
Assuming the boiling point constant is constant at 0.512°C/mol, we can calculate the boiling point elevation as:
Boiling point elevation = 0.512°C/mol * 0.393 mol
= 0.201696°C
Therefore, the boiling point of the solution is raised by approximately 0.2017°C compared to the boiling point of pure water.