Understanding the Molar Mass of NaFe(EDTA)·3H2O

When it comes to chemistry, understanding the molar mass of compounds is essential for various applications, including stoichiometry, solution preparation, and chemical reaction calculations. In this article, we will focus on the molar mass of sodium iron(III) ethylenediaminetetraacetate trihydrate, commonly referred to as NaFe(EDTA)·3H2O. This compound is widely used in fields such as agriculture, medicine, and analytical chemistry.

What is NaFe(EDTA)·3H2O?

NaFe(EDTA)·3H2O is a complex formed from the combination of sodium, iron, ethylenediaminetetraacetic acid (EDTA), and three water molecules. EDTA acts as a chelating agent, binding to metal ions like iron to facilitate their solubility and bioavailability. This property makes it particularly useful in various applications, including nutrition and environmental remediation.

Chemical Structure

The chemical formula for sodium iron(III) ethylenediaminetetraacetate is NaFe(C10H12N2O8). When hydrated with three water molecules, the formula becomes NaFe(EDTA)·3H2O.

Calculating the Molar Mass

To calculate the molar mass of NaFe(EDTA)·3H2O, we need to sum the molar masses of all the constituent atoms in the formula. Here’s a breakdown:

1. Sodium (Na): 22.99 g/mol
2. Iron (Fe): 55.85 g/mol
3. Carbon (C): 12.01 g/mol (There are 10 carbon atoms in EDTA)
4. Hydrogen (H): 1.01 g/mol (There are 12 hydrogen atoms in EDTA and 6 from 3H2O = 18 total)
5. Nitrogen (N): 14.01 g/mol (There are 2 nitrogen atoms in EDTA)
6. Oxygen (O): 16.00 g/mol (There are 8 oxygen atoms in EDTA and 3 from 3H2O = 11 total)

Now, let’s do the math:

– Sodium: 1 × 22.99 g/mol = 22.99 g/mol
– Iron: 1 × 55.85 g/mol = 55.85 g/mol
– Carbon: 10 × 12.01 g/mol = 120.10 g/mol
– Hydrogen: 12 × 1.01 g/mol + 6 × 1.01 g/mol = 18.18 g/mol
– Nitrogen: 2 × 14.01 g/mol = 28.02 g/mol
– Oxygen: 8 × 16.00 g/mol + 3 × 16.00 g/mol = 176.00 g/mol

Total Molar Mass Calculation

Now, adding these values together:

\[
22.99 + 55.85 + 120.10 + 18.18 + 28.02 + 176.00 = 401.14 \text{ g/mol}
\]

Thus, the molar mass of NaFe(EDTA)·3H2O is approximately 401.14 g/mol.

Importance of Molar Mass in Applications

Understanding the molar mass of NaFe(EDTA)·3H2O is crucial for various applications:

1. Agriculture: It is used as a micronutrient fertilizer, providing essential iron to plants. Knowing the molar mass helps in formulating correct dosages.

2. Medical Applications: In medicine, NaFe(EDTA) is used for iron supplementation. Accurate dosage calculations require knowledge of its molar mass.

3. Analytical Chemistry: In titrations and other analytical methods, knowing the molar mass allows chemists to calculate concentrations and prepare solutions accurately.

Conclusion

The molar mass of NaFe(EDTA)·3H2O is an important factor in its application across various fields. By understanding how to calculate the molar mass of compounds, scientists and professionals can ensure accurate formulations, whether in agriculture, medicine, or analytical chemistry. With a molar mass of approximately 401.14 g/mol, NaFe(EDTA)·3H2O stands out as a vital compound in both research and practical applications.