When 8.95g of hydrated magnesium bromide is heated 2.03g of water is driven off What is the empirical Formula?

To find the empirical formula of hydrated magnesium bromide, we first determine the moles of magnesium (Mg), bromine (Br), and water (H₂O) after heating. The mass of anhydrous magnesium bromide is 8.95g - 2.03g = 6.92g. The moles of water lost (2.03g) is calculated as 2.03g / 18.02g/mol = 0.112 moles. Assuming magnesium bromide has the formula MgBr₂, we find the moles of Mg and Br in the remaining mass, leading to an empirical formula of MgBr₂·xH₂O, where x is determined by the ratio of moles of water to moles of MgBr₂.