Final answer:
To find the formula of a hydrated copper(II) sulfate, one must calculate the molar mass of both CuSO4 and H2O, determine the number of moles of each from the given masses, and then divide the moles of water by the moles of CuSO4 to find the ratio, represented as CuSO4.xH2O.
Step-by-step explanation:
Determining the Formula of a Hydrated Compound
The question involves determining the chemical formula of a hydrated compound, specifically a hydrate of copper(II) sulfate. This kind of hydrate is described as a salt that has water molecules incorporated into its structure. When heated, the water of hydration is removed, and the mass of the anhydrous salt can be measured. From this information, the ratio of water molecules to salt formula units can be deduced.
Steps to Determine the Formula of the Hydrate
Given that the mass of the anhydrous copper(II) sulfate (CuSO4) is 4.8g and the mass of the water driven off is 2.6g, we can calculate the number of moles of both the anhydrous salt and water to find the ratio.
Calculate the molar mass of anhydrous CuSO4 (63.55 for Cu, 32.07 for S, and 16.00 for each O, total 159.62 g/mol).
Calculate the number of moles of CuSO4 (4.8g / 159.62 g/mol).
Calculate the number of moles of water (2.6g / 18.02 g/mol).
Divide the moles of water by the moles of CuSO4 to find the ratio and hence the number of water molecules per formula unit of CuSO4.
By applying these steps to the actual masses given in the question, the formula of the hydrate can be determined, typically denoted as CuSO4.xH2O, where 'x' represents the number of water molecules.