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Complete the following table. For each of the hydrates: (a) write the chemical formula; (b) calculate the formula mass; and (c) calculate the mass percentage of water.
What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 − 7.58 = 8.09 g of water. 2) Determine moles of MgCO 3 and water: MgCO 3 ---> 7.58 g / 84.313 g/mol = 0.0899 mol H 2 O ---> 8.09 g / 18.015 g/mol = 0.449 mol.
From these data, determine the value of x and write the complete formula for hydrated copper(II) chloride. Solution: 1) Determine the mass of the anhydrate and of the water that was lost: CuCl 2---> 17.917 − 16.221 = 1.696 g H 2 O ---> 18.360 − 17.917 = 0.443 g. 2) Determine moles of each: CuCl 2---> 1.696 g / 134.452 g/mol = 0.012614 mol
Lab - Determining the Chemical Formula of a Hydrate. Some ionic compounds form crystalline structures that trap water molecules within the crystalline framework. They are known as “hydrated salts”, or simply, hydrates.
A hydrate is an ionic compound that contains water molecules in its structure. To determine the formula of a hydrate experimentally, we must calculate the mole: mole ratio of the water portion compared to the anhydrate portion. An anhydrate is the substance that remains after the water is removed from a hydrate.
Formula of a Hydrate (\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)) The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid.
What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 minus 7.58 = 8.09 g of water. 2) Determine moles of MgCO3 and water: MgCO3 --> 7.58 g / 84.313 g/mol = 0.0899 mol H2O --> 8.09 g / 18.015 g/mol = 0.449 mol. 3) Find a whole number molar ratio: MgCO3 --> 0.0899 mol / 0.0899 mol =
