Calculate the mass of Fe(NH4)2(SO4)2.6H2O(s) required to prepare 25ml of 1.0 M Fe(NH4)2(SO4)2.6H20(aq)

25ml of 1.0M contains 0.025 moles of solute.

So, how many grams is that for this compound?

Would you do moles/molar mass to find the grams?

mols = grams/molar mass so

grams = mols x molar mass

No

To calculate the mass of Fe(NH4)2(SO4)2.6H2O required to prepare the given solution, we need to follow a few steps:

Step 1: Find the molar mass of Fe(NH4)2(SO4)2.6H2O
The molar mass can be calculated by adding up the atomic masses of all the atoms in the compound. Here is a breakdown of each component's atomic mass:
- Iron (Fe): Atomic mass = 55.85 g/mol
- Ammonium (NH4): Atomic mass = 18.03 g/mol (14.01 g/mol for Nitrogen plus 4 * 1.01 g/mol for Hydrogen)
- Sulfate (SO4): Atomic mass = 96.06 g/mol (32.07 g/mol for Sulfur plus 4 * 16.00 g/mol for Oxygen)
- Water (H2O): Atomic mass = 18.02 g/mol

Next, we need to account for the number of each component in the compound:
- Fe: 1 atom
- NH4: 2 atoms
- SO4: 2 atoms
- H2O: 6 molecules (6 * 2 = 12 atoms)

Now we can calculate the molar mass:
Molar mass of Fe(NH4)2(SO4)2.6H2O = (1 * 55.85 g/mol) + (2 * 18.03 g/mol) + (2 * 96.06 g/mol) + (6 * 18.02 g/mol) = 392.14 g/mol

Step 2: Convert the volume to moles
To determine the number of moles of Fe(NH4)2(SO4)2.6H2O needed, we need to convert the given volume of the solution to moles using its molarity (M).
1.0 M means that you have 1 mole of the compound dissolved in 1 liter of solution (1000 mL). Therefore, for 25 mL:
Number of moles = (1.0 mol/L) * (25 mL / 1000 mL/L) = 0.025 mol

Step 3: Calculate the mass
Finally, we can calculate the mass of Fe(NH4)2(SO4)2.6H2O required using the molar mass and the number of moles:
Mass = Number of moles * Molar mass = 0.025 mol * 392.14 g/mol = 9.80 g

Therefore, to prepare 25 mL of a 1.0 M Fe(NH4)2(SO4)2.6H2O solution, you would need 9.80 grams of the compound.