A mixture of CuSO4 ·5 H2 O and MgSO4 ·7 H2 O is heated until...

A mixture of $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ and $\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}$ is heated until all the water is lost. If 5.020 g of the mixture gives 2.988 g of the anhydrous salts, what is the percent by mass of $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ in the mixture?

A mixture of $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ and $\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}$ is heated until
all the water is lost. If 5.020 g of the mixture gives 2.988 g of the anhydrous salts, what is the percent by mass of $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ in the mixture?

Key Concepts

Stoichiometry

Stoichiometry involves using the relationships between the moles and masses of reactants and products in a chemical reaction. In the context of dehydration and mixture analysis, it allows one to set up equations based on the known ratios in hydrated compounds and their dehydration products, enabling the determination of the amount of each component in the original mixture.

Mass Percent Composition

Mass percent composition is the calculation of the percentage by mass of a component in a mixture relative to the total mass. This concept is applied when analyzing mixtures, such as determining the proportion of one hydrate in an alloy of different hydrates by comparing the mass of the anhydrous residue to the initial sample mass.

Hydrates

Hydrates are chemical compounds that include water molecules in their crystalline structure. The water is typically incorporated in a fixed ratio, and these water molecules can be removed through processes such as heating. Understanding hydrates is essential for analyzing how heating causes the water to be lost, thereby converting the compounds into their anhydrous forms.

Dehydration Reaction

Dehydration reactions involve the removal of water from a compound, typically by applying heat. This process is critical in studying hydrated salts, as heating them results in loss of the water of crystallization, leaving behind an anhydrous salt. This concept is key to linking the mass loss observed experimentally with the amount of water originally present in the hydrates.

Molar Mass Calculation

Molar mass calculations involve determining the mass of one mole of a substance based on its chemical formula, which is essential for converting between mass and moles. In the context of dehydration of hydrates, accurate molar mass calculations of both the hydrated and anhydrous forms allow one to relate the measured mass loss to the number of moles of water removed.

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