Sodium sulfate forms several hydrates. A sample of one of these hydrates is heated until all the water is removed. What is the formula of the original hydrate if it loses 43% of its mass when heated?

Na₂SO₄•(H₂O)₆.

Explanation:

The mass that is lost when the sample is heated is water.

Let's assume we have 100 g of the hydrate:

43 grams would be water (H₂O), while the rest (100-43=57) would be sodium sulfate anhydrous (Na₂SO₄).

We convert both those masses to moles, using their respective molar masses:

We can write those results as (Na₂SO₄)₀.₄₀•(H₂O)₂.₃₉. Now we just need to multiply those numbers so that they become integers.

If we multiply both coefficients by 5 we're left with (Na₂SO₄)₂•(H₂O)₁₂.

Simplify and thus the final answer is Na₂SO₄•(H₂O)₆.

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