After 0.6523g of CoCl2*6H2O is heated,the residue has a mass of 0.4323g. Calculate the % H2Oin the hydrate. What is the actual number of moles of water performula unit CoCl2? I don't even know where to start! Any help would be greatlyappreciated thanks!! After 0.6523g of CoCl2*6H2O is heated,the residue has a mass of 0.4323g. Calculate the % H2Oin the hydrate. What is the actual number of moles of water performula unit CoCl2? I don't even know where to start! Any help would be greatlyappreciated thanks!!
Explanation / Answer
Given data Mass of hydrated salt = 0.6523g Mass of anhydrous salt = 0.4323g Mass of water = 0.6523g - 0.4323 g =0.22 g Mass percentage of water in compound =(0.22g/0.6523g)*100 = 33.7 % Moles of anhydrous salt = 0.4323g/ 129.84 g/mol = 0.00333 mol Moles of water = 0.22 g/18.0 g/mol = 0.01222 mol ratio of moles of salt to water = 0.00333 mol : 0.0122mol = 1 : 3.67 The actual number of moles of waterperformula unit CoCl2 = 3.67 moles Moles of anhydrous salt = 0.4323g/ 129.84 g/mol = 0.00333 mol Moles of water = 0.22 g/18.0 g/mol = 0.01222 mol ratio of moles of salt to water = 0.00333 mol : 0.0122mol = 1 : 3.67 The actual number of moles of waterperformula unit CoCl2 = 3.67 moles