Describe the preparation of 2.00 L of 0.108 M BaCl₂·2H₂O (244.3 g/mol).

To prepare 2.00 L of 0.108 M BaCl₂·2H₂O solution, we need to calculate the amount of BaCl₂·2H₂O needed and then dissolve it in water to make the final volume.

1. Calculate the molar mass of BaCl₂·2H₂O:
Ba: 137.3 g/mol
Cl: 35.5 g/mol
H₂O: 18.0 g/mol
2H₂O: 36.0 g/mol
Total molar mass = 137.3 + 2(35.5) + 36.0 = 244.3 g/mol

2. Calculate the moles of BaCl₂·2H₂O needed:
Molarity = moles/volume
0.108 M = moles/2.00 L
moles = 0.108 M * 2.00 L = 0.216 moles

3. Calculate the mass of BaCl₂·2H₂O needed:
mass = moles * molar mass
mass = 0.216 moles * 244.3 g/mol = 52.7 g

4. Dissolve 52.7 g of BaCl₂·2H₂O in enough water to make 2.00 L of solution.

Materials:

- BaCl₂·2H₂O (244.3 g/mol)
- Deionized water

Procedure:

1. Calculate the mass of BaCl₂·2H₂O required:

```
Mass = (Molarity × Volume) × Molecular weight
Mass = (0.108 M × 2.00 L) × 244.3 g/mol
Mass = 5.32 g
```

2. Weigh out 5.32 g of BaCl₂·2H₂O:

Using a balance, accurately weigh out 5.32 g of BaCl₂·2H₂O and transfer it to a clean beaker.

3. Dissolve the BaCl₂·2H₂O in a small volume of water:

Add a small amount of deionized water (e.g., 50-100 mL) to the beaker containing the BaCl₂·2H₂O and stir until it dissolves completely.

4. Transfer the solution to a volumetric flask:

Quantitatively transfer the BaCl₂·2H₂O solution to a 2.00 L volumetric flask.

5. Dilute the solution to the mark:

Using a graduated cylinder, add deionized water to the volumetric flask until the solution reaches the 2.00 L mark.

6. Mix thoroughly:

Stopper the volumetric flask and invert it several times to mix the solution thoroughly.

Notes:

- It is important to use accurate weighing and volume measurements to ensure the desired concentration.
- Deionized water should be used to avoid introducing impurities into the solution.
- Once prepared, the solution should be stored in a sealed container to prevent evaporation.