Question

What is the freezing point (in C) of a 1.56 m aqueous solution of CaCl2? (Amount to three decimal points)

Answer 1

Supposing complete ionization: 
CaCl2 → Ca{2+} + 2 Cl{-} [three ions total] 

(1.56 m CaCl2) x (3 mol ions / 1 mol CaCl2) = 4.68 m ions 

(1.86 °C/m) x (4.68 m) = 8.70 °C change 

0°C - 8.70°C = - 8.70°C

Answer 2

Answer:

-8.705

Explanation:

Just did this problem :) it’s correct