Determine the mass of iron in the following solution. 325mL of 0.050 M FeSO4.
To determine the mass of iron in the given solution, we can use the formula:
mass = molarity x volume x molar mass
First, let's calculate the number of moles of FeSO4 using the formula:
moles = molarity x volume
moles = 0.050 M x 0.325 L
moles = 0.01625 mol FeSO4
Next, we need to find the molar mass of FeSO4. The molar mass of Fe is 55.845 g/mol, S is 32.06 g/mol, and O is 16.00 g/mol.
Molar mass of FeSO4 = (1 x molar mass of Fe) + (1 x molar mass of S) + (4 x molar mass of O)
Molar mass of FeSO4 = (1 x 55.845 g/mol) + (1 x 32.06 g/mol) + (4 x 16.00 g/mol)
Molar mass of FeSO4 = 55.845 g/mol + 32.06 g/mol + 64.00 g/mol
Molar mass of FeSO4 = 151.905 g/mol
Now, we can find the mass of iron by multiplying the moles of FeSO4 by the molar mass:
mass of iron = moles of FeSO4 x molar mass of FeSO4
mass of iron = 0.01625 mol x 151.905 g/mol
mass of iron = 2.472 g
Therefore, the mass of iron in the given solution is 2.472 grams.
To determine the mass of iron in the given solution, we need to use the given concentration of FeSO4 and the volume of the solution.
The concentration of FeSO4 is given as 0.050 M, which means that there are 0.050 moles of FeSO4 in every liter of the solution.
First, let's convert the volume from milliliters to liters:
325 mL = 325/1000 = 0.325 L
Now, we can use the formula:
Mass = Concentration x Volume
Mass of FeSO4 = 0.050 mol/L x 0.325 L
Multiply the concentration and the volume to get the final result:
Mass of FeSO4 = 0.01625 moles
To find the mass of iron, we need to take into account the molar mass of iron (Fe). The molar mass of Fe is 55.845 g/mole.
Now, we can calculate the mass of iron:
Mass of iron = Mass of FeSO4 x (1 mole of Fe / 1 mole of FeSO4) x Molar mass of Fe
Mass of iron = 0.01625 moles x (55.845 g/mole / 1 mole) = 0.9072 grams
Therefore, the mass of iron in the given solution is approximately 0.9072 grams.