how can I prepare 5 micromolar solution of Fe(NO3)3.9H2O? plz guide me as soon as possible

To prepare a 5 micromolar (µM) solution of Fe(NO3)3.9H2O, you will need to follow several steps. Here's a guide on how to do it:

1. Determine the molecular weight of Fe(NO3)3.9H2O.
- The molecular weight of Fe(NO3)3 is 241.86 g/mol.
- The molecular weight of H2O is 18.02 g/mol.
- So, the molecular weight of Fe(NO3)3.9H2O is (241.86) + (9 x 18.02) = 423.18 g/mol.

2. Calculate the molar mass of Fe(NO3)3.9H2O.
- Molar mass is the mass of one mole of a substance, which is the sum of the atomic masses of its constituents.
- Molar mass = (Number of Fe(NO3)3.9H2O molecules per mole) x (Molecular weight of Fe(NO3)3.9H2O).
- In this case, since Fe(NO3)3.9H2O is a single molecule, there is one molecule per mole, so the molar mass is equal to the molecular weight calculated in step 1.

3. Calculate the amount of Fe(NO3)3.9H2O needed.
- To make a 5 µM solution, you need to know how many moles of Fe(NO3)3.9H2O you need per liter of solution.
- Since 1 µM = 1 x 10^-6 M, a 5 µM solution means 5 x 10^-6 moles of Fe(NO3)3.9H2O per liter of solution.
- Therefore, the amount of Fe(NO3)3.9H2O needed is (5 x 10^-6 moles) x (Molar mass of Fe(NO3)3.9H2O).

4. Convert the amount of Fe(NO3)3.9H2O needed to grams.
- Since the molar mass was calculated in grams per mole, you can convert the moles into grams.
- Multiply the amount of Fe(NO3)3.9H2O needed (in moles) by its molar mass (in grams per mole).

5. Dissolve Fe(NO3)3.9H2O in solvent to make the desired volume.
- Dissolve the calculated amount of Fe(NO3)3.9H2O in a suitable solvent, typically deionized water, to make the desired volume of solution.
- For example, if you want to prepare 1 liter of the 5 µM solution, dissolve the calculated mass of Fe(NO3)3.9H2O in enough water to bring the total volume to 1 liter.

Remember to wear appropriate protective gear (gloves, goggles) when handling chemicals, and always follow the recommended safety precautions.