The mass (in grams) of FeSO4*7H2O required for preparation of 125 mL of 0.90 M
You want how many moles? That's mols = M x L = = 0.90 x 0.125 = ?
Then grams = mols x molar mass. You know mols and molar mass. Solve for grams. Post your work if you get stuck.
Stuck
To determine the mass of FeSO4·7H2O required for the preparation of a 0.90 M solution in 125 mL, we will follow these steps:
Step 1:
Identify the molar mass of FeSO4·7H2O.
Fe atomic mass = 55.85 g/mol
S atomic mass = 32.06 g/mol
O atomic mass = 16.00 g/mol
H atomic mass = 1.01 g/mol
The molar mass of FeSO4·7H2O can be calculated as follows:
55.85 g/mol + 32.06 g/mol + (4 × 16.00 g/mol) + (14.07 g/mol × 7) + (2.02 g/mol × 14) = 278.02 g/mol
Step 2:
Determine the number of moles of FeSO4·7H2O required using the formula:
moles = concentration (M) × volume (L)
The volume needs to be converted from mL to L.
125 mL ÷ 1000 = 0.125 L
moles = 0.90 M × 0.125 L = 0.1125 moles
Step 3:
Calculate the mass of FeSO4·7H2O using the conversion factor:
mass = moles × molar mass
mass = 0.1125 moles × 278.02 g/mol = 31.28 grams
Therefore, the mass of FeSO4·7H2O required is approximately 31.28 grams for the preparation of 125 mL of 0.90 M solution.
To determine the mass of FeSO4*7H2O required for the preparation of 125 mL of 0.90 M solution, we need to follow a few steps:
Step 1: Understand the given information.
We are given the volume of the solution (125 mL) and the molarity (0.90 M).
Step 2: Use the molarity to calculate the number of moles.
Molarity (M) is defined as moles of solute per liter of solution. Therefore, we can use the following formula to calculate the number of moles:
moles = Molarity x Volume (in liters)
To convert the volume from milliliters to liters, divide it by 1000:
Volume (in liters) = Volume (in mL) / 1000
In this case:
Volume (in liters) = 125 mL / 1000 = 0.125 L
So, we have:
moles = 0.90 M x 0.125 L
Step 3: Calculate the number of moles of FeSO4*7H2O.
The compound FeSO4*7H2O indicates that one mole of FeSO4*7H2O consists of one mole of FeSO4 and 7 moles of water. Therefore, we can calculate the number of moles of FeSO4*7H2O using the following conversion factor:
1 mole of FeSO4*7H2O = 1 mole of FeSO4
So, the number of moles of FeSO4*7H2O is the same as the number of moles of FeSO4.
Step 4: Find the molar mass of FeSO4*7H2O.
The molar mass is the mass of one mole of a substance. To calculate the molar mass of FeSO4*7H2O, we need to add up the atomic masses of each element in the compound.
The atomic masses are as follows:
Fe: 55.85 g/mol
S: 32.07 g/mol
O: 16.00 g/mol (there are 4 oxygen atoms)
H: 1.01 g/mol (there are 14 hydrogen atoms)
Molar mass of FeSO4*7H2O = (55.85 g/mol) + (32.07 g/mol) + (4 x 16.00 g/mol) + (14 x 1.01 g/mol)
Step 5: Calculate the mass of FeSO4*7H2O.
Finally, we can calculate the mass of FeSO4*7H2O using the formula:
mass = moles x molar mass
Substitute the values we calculated earlier:
mass = moles of FeSO4*7H2O x molar mass of FeSO4*7H2O
By following these steps, you can determine the mass of FeSO4*7H2O required for the preparation of 125 mL of 0.90 M solution.