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The student used 15.0 cm³ of 2.00 mol/dm³ sulfuric acid to prepare the crystals. Calculate the maximum mass of hydrated copper(II) sulfate crystals that could be made.

a) 320 g

b) 80 g

c) 160 g

d) 40 g

1 Answer

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Final answer:

To calculate the maximum mass of hydrated copper(II) sulfate crystals, we can use stoichiometry. The maximum mass is approximately 4.79 g.

Step-by-step explanation:

To calculate the maximum mass of hydrated copper(II) sulfate crystals, we need to use stoichiometry.

The balanced chemical equation for the reaction between sulfuric acid (H₂SO₄) and hydrated copper(II) sulfate (CuSO₄·xH₂O) is:

H₂SO₄ + CuSO₄·xH₂O → CuSO₄ + xH₂O

From the equation, we can see that the molar ratio between H₂SO₄ and CuSO₄ is 1:1. Therefore, the number of moles of CuSO₄ that can be made is equal to the number of moles of H₂SO₄ used.

Using the given concentration and volume of H₂SO₄, we can calculate the number of moles of H₂SO₄:

Moles of H₂SO₄ = concentration × volume = 2.00 mol/dm³ × 0.0150 dm³ = 0.0300 mol

Since the molar ratio between H₂SO₄ and CuSO₄ is 1:1, the number of moles of CuSO₄ that can be made is also 0.0300 mol. To calculate the maximum mass of hydrated copper(II) sulfate crystals, we need to know the molar mass of CuSO₄·xH₂O.

To find the molar mass of CuSO₄·xH₂O, we must consider the molar mass of each individual element and account for the number of atoms in the compound. The molar mass of CuSO₄ is 159.61 g/mol.

Now we can calculate the maximum mass of CuSO₄·xH₂O crystals:

Maximum mass = number of moles × molar mass = 0.0300 mol × 159.61 g/mol = 4.79 g

Therefore, the maximum mass of hydrated copper(II) sulfate crystals that could be made is approximately 4.79 g.

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