Determine the mass of iron in the following solution. 325mL of FeSO4.
To determine the mass of iron in the solution of FeSO4, we need to consider the molarity of FeSO4 and its molecular weight.
First, find the molarity (M) of the solution using the given information. Since the volume is given in milliliters (mL), we need to convert it to liters (L):
325 mL = 325/1000 L = 0.325 L
Next, you need to determine the molar mass of FeSO4. The molar mass of iron (Fe) is approximately 55.85 g/mol, sulfur (S) is 32.07 g/mol, and oxygen (O) is 16.00 g/mol. Since there are four oxygen atoms in FeSO4, we can calculate the molar mass as follows:
Fe: 1 atom x 55.85 g/mol = 55.85 g/mol
S: 1 atom x 32.07 g/mol = 32.07 g/mol
O: 4 atoms x 16.00 g/mol = 64.00 g/mol
Total molar mass of FeSO4: 55.85 + 32.07 + 64.00 = 151.92 g/mol
Now you can calculate the moles of FeSO4 in the solution using the molarity formula:
Molarity (M) = Moles (mol) / Volume (L)
Rearranging the formula, we have:
Moles (mol) = Molarity (M) x Volume (L)
Since we already calculated the molarity and have the volume, we can substitute these values into the formula and solve for moles:
Moles (mol) = 0.325 L x Molarity (M)
The moles of FeSO4 represents the moles of iron (Fe) because there is one mole of iron in one mole of FeSO4.
Finally, to determine the mass of iron (Fe), we use the molar mass of iron (Fe) and the moles of FeSO4:
Mass (g) = Moles (mol) x Molar mass (g/mol)
Substituting the moles of FeSO4 into the formula, we have:
Mass (g) = Moles (mol) x Molar mass of Fe (g/mol)
Now, you can calculate the mass of iron in the FeSO4 solution by using the calculated moles of FeSO4 and the molar mass of iron (Fe).