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What volume of FeSO4.7H2O should be added in 200g of water so that resulting solution contains 10percent FeSO4 by Mass?
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What volume of FeSO4.7H2O should be added in 200g of water so that res...
Calculating the Volume of FeSO4.7H2O to Add


Step 1: Calculate the Mass of FeSO4 Needed


To calculate the mass of FeSO4 needed to make a 10% by mass solution, we first need to know the total mass of the solution. In this case, the problem states that we have 200g of water. Therefore, the total mass of the solution will be 200g.

Next, we need to calculate what 10% of the total mass is. To do this, we multiply the total mass by the decimal equivalent of 10%.

10% = 0.10

0.10 x 200g = 20g

Therefore, we need 20g of FeSO4 in our solution.

Step 2: Calculate the Mass of FeSO4.7H2O Needed


FeSO4.7H2O is a hydrated form of FeSO4, meaning that it contains water molecules within its crystal structure. To calculate the mass of FeSO4.7H2O needed to make our solution, we need to take into account the mass of the water molecules as well.

The molar mass of FeSO4 is 151.91 g/mol, and the molar mass of 7H2O is 126.10 g/mol. Therefore, the molar mass of FeSO4.7H2O is:

(151.91 g/mol) + (7 x 18.02 g/mol) = 278.02 g/mol

To calculate the mass of FeSO4.7H2O needed, we divide the mass of FeSO4 by the molar mass of FeSO4.7H2O and multiply by the molar mass of FeSO4.7H2O.

(20g FeSO4) / (278.02 g/mol FeSO4.7H2O) x (278.02 g/mol FeSO4.7H2O) = 20g FeSO4.7H2O

Therefore, we need 20g of FeSO4.7H2O to make our solution.

Step 3: Calculate the Volume of FeSO4.7H2O Needed


To calculate the volume of FeSO4.7H2O needed, we need to know the density of the compound.
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What volume of FeSO4.7H2O should be added in 200g of water so that resulting solution contains 10percent FeSO4 by Mass?
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