Barium metal was quantitatively precipitated from a 1.52 g sample of BaCl2∙2H2O. The mass of the barium that was collected was 0.844 g. Calculate the experimental mass percent of barium in the sample.

To calculate the experimental mass percent of barium in the sample, we can use the following steps:

### Step 1: Write down the mass of the sample and the mass of barium obtained.
- Mass of BaCl₂·2H₂O sample = 1.52 g
- Mass of barium collected = 0.844 g

### Step 2: Use the formula for mass percent:
\[
\text{Mass percent of barium} = \left( \frac{\text{Mass of barium}}{\text{Mass of BaCl}_2 \cdot 2H_2O}} \right) \times 100
\]

Substitute the given values:
\[
\text{Mass percent of barium} = \left( \frac{0.844 \, \text{g}}{1.52 \, \text{g}} \right) \times 100
\]

### Step 3: Calculate the mass percent:
\[
\text{Mass percent of barium} = \left( 0.55526 \right) \times 100 = 55.53\%
\]

### Final answer:
The experimental mass percent of barium in the sample is **55.53%**.

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Would you like further details on how this was calculated? Here are some related questions you might explore:

1. How is barium typically precipitated in chemical reactions?
2. What is the molar mass of BaCl₂·2H₂O?
3. How does the theoretical mass percent of barium in BaCl₂·2H₂O compare to this experimental value?
4. What factors could affect the mass of barium collected in an experiment like this?
5. How do impurities in the sample influence the experimental mass percent?

**Tip**: When calculating experimental percentages, always double-check the purity of your reactants and account for any potential losses during the experiment.

Barium metal was quantitatively precipitated from a 1.52 g sample of BaCl2∙2H2O. The mass of the barium that was collected was 0.844 g. Calculate the experimental mass percent of barium in the sample.

Learn how to calculate the experimental mass percent of barium in a 1.52 g sample of BaCl2∙2H2O with a collected barium mass of 0.844 g. This problem involves concepts of stoichiometry and chemical composition, making it ideal for high school chemistry students.

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