What is the freezing point of an aqueous solution that has 25.00 g of calcium iodide dissolved in 1250 g of water?

- 0.380ºC

Explanation:

The lowering of the freezing point of a solvent is a colligative property ruled by the formula:

Where:

ΔTf is the lowering of the freezing pointKf is the molal freezing constant of the solvent: 1.86 °C/mm is the molality of the solutioni is the van't Hoff factor: the number of particles (ions) per unit of ionic compound.

a) molality, m

m = number of moles of solute/ kg of solventnumber of moles of CaI₂ = mass in grams/ molar massnumber of moles of CaI₂ = 25.00g / 293.887 g/mol = 0.0850667molm = 0.0850667mol/1.25 kg = 0.068053m

b) i

Each unit of CaI₂, ideally, dissociates into 1 Ca⁺ ion and 2 I⁻ ions. Thus, i = 1 + 2 = 3

c) Freezing point lowering

ΔTf =  1.86 °C/m × 0.068053m × 3 = 0.3797ºC ≈ 0.380ºCI have problems to upload the full answer in here, so I attach a pdf file with the whole answer.

They are all decomposition reactions.

Is there an image with it