Question

suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. given the data collected in the table, what is the formula of the hydrate? the molar mass of water is 18.015 g/mol and the molar mass of barium chloride is 208.23 g/mol.

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$$\begin{tabular}{|l|c|} \\hline mass of empty crucible (g) & 72.505 \\\\ \\hline mass of crucible and hydrate (g) & 75.478 \\\\ \\hline mass of crucible and anhydrous salt (g) & 75.039 \\\\ \\hline \\end{tabular}$$

empirical formula of hydrate:

Explanation:

Calculate the mass of anhydrous salt and water

Using the Anhydrous Salts and Hydrate Formulas knowledge points

$$
LATEXBLOCK0
$$

Convert masses to moles

Using the Stoichiometry knowledge point

$$
LATEXBLOCK1
$$

Determine the mole ratio

Using the Hydrate Formulas knowledge point

$$
LATEXBLOCK2
$$

Write the empirical formula

Using the Hydrate Formulas knowledge point

$$ \text{Formula} = \text{BaCl}_2 \cdot 2\text{H}_2\text{O} $$

Answer:

empirical formula of hydrate: <blank>\(\text{BaCl}_2 \cdot 2\text{H}_2\text{O}\)</blank>