The experiment requires 1 mg per ml of iron. what masss of iron (III) nitrate hexahydrate (Fe(NO3) - 6H2O) would you need to dissolve in 1 litre to achieve this value?
I would start by figuring the decimal percentage of Fe in that compound.
Then, to get 1mg fe,you need masscompound*percentage of the compound, or the masscompound to get 1mg is 1mg/percentagecomposition
Then,you need 1000 times that much to make a liter.
so i would find the percent of iron in the compound, and then find the total mass of the compound and multiply it by the percent of iron that i found?
To determine the mass of iron (III) nitrate hexahydrate needed to dissolve in 1 liter of solution, we need to calculate the molar mass of Fe(NO3)3·6H2O and then convert the desired concentration from mg/mL to g/L.
1. Calculate the molar mass of Fe(NO3)3·6H2O:
- The molar mass of Fe(NO3)3: Iron (Fe) has an atomic mass of approximately 55.845 g/mol, and each nitrate group (NO3) has an atomic mass of approximately 62.0049 g/mol (14.0067 g/mol for nitrogen and 3 * 15.9994 g/mol for each oxygen).
Fe: 1 atom * 55.845 g/mol = 55.845 g/mol
NO3: 3 atoms * (14.0067 g/mol + 3 * 15.9994 g/mol) = 187.0053 g/mol
Total molar mass of Fe(NO3)3: 55.845 g/mol + 187.0053 g/mol = 242.8503 g/mol
- The molar mass of 6H2O: Water (H2O) has an atomic mass of approximately 18.015 g/mol, and since there are 6 water molecules in Fe(NO3)3·6H2O: 6 * 18.015 g/mol = 108.09 g/mol
- Molar mass of Fe(NO3)3·6H2O:
242.8503 g/mol + 108.09 g/mol = 350.9403 g/mol
2. Convert the concentration from mg/mL to g/L:
Since 1 mg/ml is the same as 1 g/L, we don't need to convert it further. The desired concentration remains the same: 1 g/L.
3. Calculate the mass of iron (III) nitrate hexahydrate required:
To calculate the mass, we will use the formula: mass = concentration * volume
- Mass = 1 g/L * 1 L = 1 gram
Therefore, you would need 1 gram of iron (III) nitrate hexahydrate (Fe(NO3)3·6H2O) to dissolve in 1 liter of solution to achieve a concentration of 1 mg/mL.