Hydrate of Barium Chloride

In this experiment a hydrate of barium chloride, BaCl₂·xH₂O, is sequentially weighed, heated, and then weighed again after the waters of hydration have been removed. The goal is to determine the hydration number, x.

Determine the mass of BaCl₂·xH₂O before heating
Determine the mass of anhydrous BaCl₂ after heating
Determine the mass of H₂O lost
Convert the masses of BaCl₂ and H₂O into moles
The hydration number is given by the fraction: mol H₂O ÷ mol BaCl₂

Because experimental values are not exact, the calculated value of x is usually close to an integer. If so, that integer is accepted as the correct value.

Watch the video below, then use what you observe to fill out the Data Table and Results Table. Click the ? next to any box for a hint.

Item	Value
Mass of crucible	✓ ✗ g
Mass of crucible + BaCl₂·xH₂O before heating	✓ ✗ g
Mass of crucible + BaCl₂ after heating	✓ ✗ g

🔢 Results Table

Item	Value
Mass of BaCl₂·xH₂O	✓ ✗ g
Mass of BaCl₂	✓ ✗ g
Mass of H₂O	✓ ✗ g
Moles of BaCl₂	✓ ✗ mol
Moles of H₂O	✓ ✗ mol
Hydration number (x)	✓ ✗

Experiment: Hydrate of Barium Chloride