To find the mass percent of potassium ion in the complex iron salt, we first need to break down the components of the complex, which contains iron (Fe), oxalate ion, and water (H2O).
Given the molar masses:
– Iron (Fe): 55.85 g/mol
– Oxalic acid (H2C2O4): 90.03 g/mol, so oxalate ion (C2O42-): 88.02 g/mol
– Water (H2O): 18.02 g/mol
We also know that the complex is formulated with these components. For example, let’s consider the formula: Fe(C2O4)·nH2O, where n represents the number of water molecules associated with the complex.
1. First, find the molar mass of the entire complex:
Mass of Fe = 55.85 g/mol
Mass of C2O4 = 88.02 g/mol
Mass of H2O = 18.02 g/mol
Total mass of complex (assuming n=6 H2O as a common example) = 55.85 + 88.02 + (6 * 18.02) = 55.85 + 88.02 + 108.12 = 251.99 g/mol
2. Now, if we assume that in a complete dissociation of the complex, potassium ions (K+) are released, we need to know the contribution of K to the overall mass. This is derived from knowing that each potassium ion contributes 39.10 g/mol.
3. To find the mass percent of potassium ion:
– Let’s say our formula also includes 1 mole of K for this example m = no of K ions
Molar mass of K = 39.10 g/mol
Thus, total mass for calculation = 251.99 g/mol + 39.10 g/mol = 291.09 g/mol
Mass percent of K = (mass of K / total mass of the complex) * 100
= (39.10 / 291.09) * 100 ≈ 13.45%
In conclusion, if your complex has potassium as a part of it, the mass percent of potassium ion in this iron oxalate complex can be approximately 13.45%. Adjust the calculation as needed based on the actual proportions of substances in your specific complex.