As a solution of copper sulfate slowly evaporates, beautiful...

As a solution of copper sulfate slowly evaporates, beautiful blue crystals made of copper(II) and sulfate ions form such that water molecules are trapped inside the crystals. The overall formula of the compound is $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ a. What is the percent water in this compound? b. At high temperatures, the water in the compound is driven off as steam. What mass percentage of the original sample of the blue solid is lost as a result?

As a solution of copper sulfate slowly evaporates, beautiful blue crystals made of copper(II) and sulfate ions form such that water molecules are trapped inside the crystals. The overall formula of the compound is $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$
a. What is the percent water in this compound?
b. At high temperatures, the water in the compound
is driven off as steam. What mass percentage of the original sample of the blue solid is lost as a result?

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Key Concepts

Thermal Decomposition

Thermal decomposition refers to the process by which a compound breaks down upon heating. In the context of hydrates, heating typically causes the water of crystallization to be driven off as steam, leading to a measurable mass loss that corresponds to the water content originally present in the hydrate.

Hydrates

Hydrates are compounds that include water molecules integrated into their crystal structure. The water, known as water of crystallization, is held in a fixed stoichiometric ratio relative to the compound, and these water molecules significantly affect both the properties and the molar mass of the compound.

Percent Composition

Percent composition is a concept used to determine the percentage by mass of a specific component in a compound. In hydrates, this involves calculating the ratio of the mass of water to the total molar mass of the compound, then converting that ratio into a percentage.

Molar Mass Calculations

Molar mass calculations involve summing the atomic masses of all atoms present in a chemical formula. For hydrates, this calculation must include the water molecules attached to the compound, which plays a critical role in determining the overall mass and percent composition.

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