A chemist (ahem, I guarantee any non-chemist will not remember having done this equation during college/etc., even if he or she does it 100 times... and, if they do remember it, maybe they are a genius, but will they ever use it, ponder it, find happiness in life from remembering it...) wants to make 5.0
of a 0.270
solution
What mass of (in 
) should the chemist use?
Given Volume of the solution , V = 5.0 L
Molarity of the solution , M = 0.270 M
Molar mass of CaCl2: 40.078 + 2(35.453) = 110.984 g /mol
Mass of CaCl2 = (V) x (Molarity) x (Molar Mass of CaCl2)
5.0 X .270 X 110.984 = 149.8284 = 150 (rounded to two significant numbers)
