posted by DrFunk on .
How would I go about doing this question, can someone explain it step by step please, my answer I keep getting is 1.17m CaCl2, but the answer is 1.35m CaCl2?
A 1.30M solution of CaCl2 in water has a density of 1.1g/mL/ What is the MOLALITY?
Also, when for questions with relation to finding minimum pressure, or boiling point elevation or freezing point deperession quesitons, how do I know that I have to use the "i" factor or not?
1.30 M means 1.30 moles / liter of solution
1 mole CaCl2 = 111.0 g (How do you get that?)
1.30 mol x 111 g = 144.3 g CaCl2
1.00 L = 1000 mLs
volume x density = mass:
1000 mLs x 1.1 g/mL = 1100 grams solution (total)
1100 g - 144.3g = 955.7 g H2O ---> 0.9553 kg H2O
molality = m = 1.3 mol CaCl2 / 0.9553 kg H2O = ???
The above answer should be multiplied by 3 since 1 mole of CaCl2 produces THREE particles in solution. The new answer is the EFFECTIVE molality you use to get vapor pressure, melting point lowering , and boiling point rise. You got some studying to do on colligative properties and calculations related to that. We do not teach complete units on a bulletin board posting.
1.30 M = 1.30mols of solute/L of solvent
mass of Cacl2 = 1.30 mols CaCl2 x 111g/mol CaCl2(molar mass)= 144.3g of CaCl2 (solute)
Solution = 1.11g/ml
mass of solution = 1.11g/ml x 1000ml/L x1L
= 1110g (solution)
mass of solvent = 1110g (solution) - 144.3g (solute)= 965.7g of solvent x 1kg/1000g = 0.9657kg
molality = 1.30 mols of solute/0.9657kg solvent