Determine the mass of CaCl2 * 6 H2O and the volume of water required to prepare 500 g of a 6% solution

Mass fraction of CaCl2 in solution – the ratio of the mass of anhydrous CaCl2 to the mass of the solution (taking into account the mass of the crystalline hydrate). Find the mass of CaCl2.

m (CaCl2) = 500 * 0.06 = 30 g

Find the number of moles of CaCl2.

n (CaCl2) = 30/111 = 0.27 mol

1 mol of CaCl2 * 6H2O crystalline hydrate contains 1 mol of CaCl2. This means that 0.27 mol of CaCl2 corresponds to 0.27 mol of CaCl2 * 6H2O.

Find the mass of CaCl2 * 6H2O.

m (CaCl2 * 6H2O) = 0.27 * 219 = 59.1 g

m (H2O) = 500 – 59.1 = 440.9 g

V (H2O) = 440.9 ml