[Atome]

Hello everyone,

I am having some trouble with this following problem and I would appreciate any help or hints.

My work is shown below.

Thank you.

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1. A metal, M, was converted to the sulphate, M₂(SO₄)₃. Then a solution of the sulphate was treated with barium chloride to give barium sulphate crystals, which were then filtered.

M₂(SO₄)_{3 (aq)} + 3BaCl_{2 (aq)} -> 2MCl_{3 (aq)} + 3BaSO_{4 (s)}

If 1.200 g of the metal gave 6.026 g of barium sulphate, what is the molar mass of the metal?

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Grams of sulphate ions = (96 g/mol ÷ 233 g/mol) x 6.026 g

                               = 2.483 g

Barium sulphate in mols = 6.026 g ÷ 233.43 g/mol

                                = 0.02581 mol

Therefore, M₂(SO₄)_{3 (aq)} = 0.08603 mol

However, how would this enable me to help me determine M?

[Borek]

You know number of moles, you know mass - you should be able to calculate molar mass now.