You need to make a .300 M solution of NiSO4 aq. Calculate the mass of NiSO4 6H2O you should put into a .100-L volumetric flasl
_____= mass in g
How many mols do you need? That's mols NiSO4.6H2O = M x L = 0.3M x 0.1 L = ?
Then grams = mols x molar mass = ?
To calculate the mass of NiSO4 · 6H2O, we need to use the molarity (M) of the solution, the desired volume (V), and the molar mass of NiSO4 · 6H2O.
1. Molarity of the Solution:
The molarity (M) of the solution is given as 0.300 M. This means that there are 0.300 moles of NiSO4 in 1 liter of the solution (1 L).
2. Desired Volume:
The desired volume is given as 0.100 L.
3. Molar Mass of NiSO4 · 6H2O:
The molar mass of NiSO4 · 6H2O can be calculated by adding the individual molar masses of each element in the compound:
- Nickel (Ni) has a molar mass of 58.69 g/mol.
- Sulfur (S) has a molar mass of 32.07 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol.
- Hydrogen (H) has a molar mass of 1.01 g/mol.
To calculate the molar mass of NiSO4 · 6H2O, we multiply the molar mass of each element by its respective subscript in the compound and sum them up:
Molar mass of NiSO4 · 6H2O = (58.69 g/mol) + (32.07 g/mol) + (4 x 16.00 g/mol) + (6 x (1.01 g/mol x 2)) = 262.87 g/mol
Now, we can calculate the mass of NiSO4 · 6H2O that should be put into the volumetric flask:
Mass (g) = Molarity (mol/L) x Volume (L) x Molar Mass (g/mol)
Mass (g) = (0.300 mol/L) x (0.100 L) x (262.87 g/mol) = 7.8861 g
Therefore, the mass of NiSO4 · 6H2O that should be put into the 0.100 L volumetric flask is approximately 7.8861 grams.