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How many milliliters of an aqueous solution of 0.202 M iron(II) nitrate is needed to obtain 10.5 grams of the salt?

Question

How many milliliters of an aqueous solution of 0.202 M iron(II) nitrate is needed to obtain 10.5 grams of the salt?

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Step 1

The term molarity refers to the ratio of number of moles (ratio of mass to the molar mass) of a substance to the volume of the give n solution in liters. Its SI units are moles/liter, which can also be denoted as ‘M’.

Step 2

In the given problem, the mass of iron (II) nitrate is given to be 10.5 grams while the molarity of the aqueous solution is given to be 0.202 M.

Firstly, the number of moles of iron (II) nitrate are calculated as follows:

10.5 g
Mass
Number of molesMolar mass 179.845 g/mol
--0.0583 moles
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10.5 g Mass Number of molesMolar mass 179.845 g/mol --0.0583 moles

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Step 3

Now, the volume can be cal...

Molarity Number of moles
Volume (L)
0.202 moles/liter=0.0583 moles
Volume
0.0583 moles
Volume0.202 moles/liter
-0.288613 L
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Molarity Number of moles Volume (L) 0.202 moles/liter=0.0583 moles Volume 0.0583 moles Volume0.202 moles/liter -0.288613 L

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