If the 3.90 m solution from part a boils at 103.45 ∘c, what is the actual value of the van't hoff factor, i? the boiling point of pure water is 100.00 ∘c and kb is equal to 0.512 ∘c/m.

Some of the solutions exhibit colligative properties. These properties depend on the amount of solute dissolved in a solvent. For boiling point elevation, we calculate the increase in temperature by the equation:

ΔT(boiling point)  = (Kb)mi

where Kb is a constant, m is the molality of the solution, i is the van't Hoff factor. 

From the given data, we can easily calculate for i as follows:

ΔT(boiling point)  = (Kb)mi
103.45 - 100  = (0.512)3.90i
i = 1.73 <van't Hoff factor

Idk the answer sorry