Answer:
The boiling point of a solution is higher than that of the pure solvent (in this case, water) due to the presence of solute particles in the solution. This phenomenon is known as boiling point elevation.
To calculate the change in boiling point, we can use the formula:
ΔTb = Kb x molality
where ΔTb is the change in boiling point, Kb is the molal boiling point constant for water (0.512 °C/m), and molality is the concentration of the solute in the solution expressed in mol/kg.
To calculate the molality of the solution, we first need to determine the number of moles of solute present. The number of moles of solute can be calculated using the formula:
n = m / M
where n is the number of moles, m is the mass of the solute, and M is the molar mass of the solute.
Using these formulas, we can calculate the change in boiling point as follows:
n = 2.10 g / 208.23 g/mol = 0.01 mol
molality = n / 5.50 kg = 0.002 mol/kg
ΔTb = 0.512 °C/m x 0.002 mol/kg = 0.001 °C
So, the predicted change in boiling point of water when 2.10 g of barium chloride is dissolved in 5.50 kg of water is 0.001 °C.
It's important to note that this is just an estimate, and the actual change in boiling point may be slightly different due to various factors such as the purity of the solute and the presence of other substances in the solution.
Step-by-step explanation: