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How do you work out the mass of water of crystallisation for 13.5 g of

$$\ce{Al2(SO4)3*6H2O}$$

The correct answer is 3.24 g of water but I'm unable to derive the answer.

What I have tried:

I worked out the mols of aluminium sulfate which is approx 0.038 mol by dividing 13.5 g/353.5.

Since the ratio of aluminium sulfate: water of crystallisation is 1:6, I multiplied the number of mols by 6 to result in 0.228 mol of water.

To work out the mass, I multiplied mols of water by molar mass to result in 4.101 g which is NOT the answer of 3.24 g .

What am I doing wrong and what is the correct method?

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The mass of aluminium sulfate has to be taken along with the water of crystallization.

Now molar masses
$$ \begin{array}{c| c} \text{compound} & \text{ mass (g)} \\ \hline \ce{Al2(SO4)} & 342 \\ \ce{6H2O} & 108 \\ \ce{Al2(SO4)3\cdot 6H2O} & 450\\ \end{array} $$

After that it's simply ratio and proportion find out the moles of hydrated salt then find out the moles of water finally get the mass of water.

$$\frac{13.5}{450} \times 6 \times 18 = 3.42$$

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