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3 years ago

Can 1750 mL of water dissolve 4.6 moles of Copper Sulfate CuSO4? _________ Why? / Why not?

Chemistry

1 answer:

Wewaii [24]3 years ago

8 0

Answer:

No, you cannot dissolve 4.6 moles of copper sulfate, CuSO₄, in 1750mL of water.

Explanation:

This question is part of a Post-Lab exercise sheet.

Such sheet include the saturation concentrations for several salts.

The saturation concentration of Copper Sulfate, CuSO₄, indicated in the table is 1.380M.

That means that 1.380 moles of copper sulfate is the maximum amount that can be dissolved in one liter of solution.

Find the molar concentration for 4.6 moles of copper sulfate in 1,750 mL of water.

You need to assume that the volume of water (1750mL) is the volume of the solution. This is, that the 4.6 moles of copper sulfate have a negligible volume.

1. Volume in liters:

V = 1,750 mL × 1 liter / 1,000 mL = 1.75 liter

2. Molar concentration, molarity, M:

M = number of moles of solute / volume of solution in liters

M = 4.6 moles / 1.75 liter = 2.6 M

Since the solution is saturated at 1.380M, you cannot reach the 2.6M concentration, meaning that you cannot dissolve 4.6 moles of copper sulfate, CuSO₄ in 1750mL of water.

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3 years ago

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sp2606 [1]

Answer:

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Explanation:

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