Here's how to determine the boiling point of a 2.35 m solution of sodium sulfate:

1. Understand the Concept of Boiling Point Elevation

* Boiling point elevation is the phenomenon where the boiling point of a solvent is increased when a non-volatile solute is added.

* The extent of elevation depends on the molality (moles of solute per kilogram of solvent) of the solution and a property called the molal boiling point elevation constant (K_b), which is specific to the solvent.

2. Determine the Relevant Constants

* For water:

* K_b = 0.512 °C/m

* Normal boiling point = 100 °C

3. Calculate the Change in Boiling Point (ΔT_b)

* ΔT_b = i * K_b * m

* i: van't Hoff factor (accounts for the number of particles the solute dissociates into)

* K_b: Molal boiling point elevation constant

* m: Molality of the solution

* Sodium sulfate (Na₂SO₄) dissociates into 3 ions in water:

* Na₂SO₄ → 2 Na⁺ + SO₄^2-

* Therefore, i = 3

* Calculate ΔT_b:

* ΔT_b = (3) * (0.512 °C/m) * (2.35 m) = 3.62 °C

4. Calculate the New Boiling Point

* New boiling point = Normal boiling point + ΔT_b

* New boiling point = 100 °C + 3.62 °C = 103.62 °C

Therefore, the boiling point of a 2.35 m solution of sodium sulfate is approximately 103.62 °C.