An aqueous solution of iron (II) sulfate (FeSO4) is prepared by dissolving 2.00 g in sufficient deionized water to form a 200.00 mL solution. Calculate the molarity of the solution.

Question

Michaela Mccall

Chemistry

23 June, 13:18

An aqueous solution of iron (II) sulfate (FeSO4) is prepared by dissolving 2.00 g in sufficient deionized water to form a 200.00 mL solution. Calculate the molarity of the solution.

+3

Answers (1)

Know the Answer?

Karma Steele · Answer 1

0.066mol/dm^3

Explanation:

The molarity is simply calculating the number of moles in 1L or 1000ml

To get this, we need to know the amount in grammes that would be present in 1L.

Since 2g is sufficient for 200ml, then for 1000ml, the amount sufficient would be 5 * 2 = 10g

Now to get the number of moles needed, we need to know the molar mass of the compound. That is molar mass of FeSO4 = 56 + 32 + 4 (16) = 152g/mol

The number of moles is thus 10/152 = 0.066 mol/dm^3