What is the formula for the hydrate?

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The discussion centers on determining the formula for the hydrate of barium chloride (BaCl2) based on a mass loss during heating. A sample weighing 61 grams lost 9 grams of water upon heating, resulting in a final mass of 52 grams. The correct formula for the hydrate is BaCl2 * 2H2O, as derived from the stoichiometric calculations involving the molar mass of water (18 grams) and the initial mass loss. The confusion arose from an incorrect interpretation of the mole ratio, leading to an erroneous conclusion of BaCl2 * 1/2 H2O.

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Chemistry help please!

I've tried to work out the problem below, but I got weird answer, it's not even in one of the choices. Please help me solve this problem and show me out u got it. Thank you.
A sample of a hydrate of BaCl2 with a mass of 61 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 52 grams. What is the formula for the hydrate?
(A) BaCl2 * 5H2O
(B) BaCl2 * 4H2O
(C) BaCl2 * 3H2O
(D) BaCl2 * 2H2O
(E) BaCl2 * H2O
 
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Ba=137.3gtams Cl2=71 grams
BaCl2=208.3 grams --> but the answer in book says BaCl2 =244 grams.
61 grams - 52 grams = 9 grams
9grams / 18grams (H2O) = 1/2
so my answer is BaCl2 * 1/2 H2O, which doesn't make any sense @ all, and it's not one of the answer choices.
 
ok so you have 1/2 moles of H20, how many moles of BaCl2 do you have? balance them out and you'll get the answer.
 

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