The mass percent of water in a hydrate of MnCl2 is 36.41%. What is the emperical formula of the hydrate?
You're going to start with 1 mol H2O and work your way up until you get a % H2O that is 36.41% (or, in my case, very close since I rounded). I will separate my columns with a pipe character - | - but YA isn't very good with tables. [ Remember that the molecular formula has to be in whole numbers, so you're only worried about whole moles of water. 1 mol H2O (first column) 1 mol H2O = 18 g (second column) total weight = 1 mol H2O + 1 mol MnCl2 = 18g + 125g = 143g (third column) % water = (18g / 143g) * 100 = 12.59% 1 mol H2O | 18g | 143g | 12.59% 2 mol H2O | 36g | 161g | 22.36% 3 mol H2O |
54g | 179g | 30.17% 4 mol H2O | 72g | 197g | 36.55% <- - 5 mol H2O | 90g | 215g | 41.86% I'm sure if I had used more precise weights - especially for chlorine - I would have gotten an answer closer to 36.41%, but 36.55% is very close 36.41%. So, the answer is 4 mols of H2O per MnCl2, or, in a formula: MnCl2 * 4H2O ]
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