how many grams of CuSO4.5H2O is needed to prepare 0.01 M solution?
How much of the solution?
mols needed = M x L = ?
Then grams = mols x molar mass
2.5
To calculate the amount of CuSO4.5H2O needed to prepare a 0.01 M solution, you will need to know the molar mass and the volume of the solution you want to prepare.
The molar mass of CuSO4.5H2O is calculated as follows:
- The molar mass of Cu is 63.55 g/mol
- The molar mass of S is 32.07 g/mol
- The molar mass of O is 16.00 g/mol (there are 4 oxygen atoms in the formula)
- The molar mass of H2O is 18.02 g/mol (there are 5 water molecules in the formula)
Calculating the molar mass for CuSO4.5H2O:
(63.55 g/mol Cu) + (32.07 g/mol S) + (4 * 16.00 g/mol O) + (5 * 18.02 g/mol H2O)
= 63.55 + 32.07 + 64.00 + 90.10
= 249.72 g/mol
Now, to calculate the amount of CuSO4.5H2O needed:
Molarity (M) = moles of solute / volume of solution (in L)
0.01 M = moles of CuSO4.5H2O / volume of solution (in L)
Rearranging the equation to solve for moles of CuSO4.5H2O:
moles of CuSO4.5H2O = Molarity * volume of solution (in L)
moles of CuSO4.5H2O = 0.01 mol/L * volume of solution (in L)
Finally, to calculate the mass of CuSO4.5H2O:
mass of CuSO4.5H2O = moles of CuSO4.5H2O * molar mass of CuSO4.5H2O
For example, if you want to prepare 1 liter (1 L) of the 0.01 M CuSO4.5H2O solution:
moles of CuSO4.5H2O = 0.01 mol/L * 1 L = 0.01 moles
mass of CuSO4.5H2O = 0.01 moles * 249.72 g/mol = 2.50 grams
Therefore, you would need 2.50 grams of CuSO4.5H2O to prepare a 0.01 M solution.
To calculate the number of grams of CuSO4.5H2O needed to prepare a 0.01 M solution, we'll need to know the molar mass of CuSO4.5H2O and the volume of the solution you want to prepare.
First, let's calculate the molar mass of CuSO4.5H2O:
- Atomic mass of Cu = 63.55 g/mol
- Atomic mass of S = 32.07 g/mol
- Atomic mass of O = 16.00 g/mol
- Atomic mass of H = 1.01 g/mol
- Sum of atomic masses: (63.55 + 32.07 + 4 * 16.00 + 10 * 1.01) g/mol = 249.65 g/mol
Now, let's use the formula for molarity (M):
Molarity (M) = moles of solute / volume of solution in liters
To find the grams of CuSO4.5H2O needed, we need to rearrange the equation:
moles of solute = Molarity (M) x volume of solution in liters
Given:
Molarity (M) = 0.01 M
Volume of solution = typically given in liters (e.g., if it is 100 mL, then it would be 0.1L)
Substituting the given values into the equation:
moles of solute = 0.01 M x volume of solution in liters
Finally, to calculate the grams of CuSO4.5H2O needed, we multiply the moles of CuSO4.5H2O by the molar mass:
grams of CuSO4.5H2O = moles of solute x molar mass of CuSO4.5H2O
With this information, you can calculate the gram amount of CuSO4.5H2O needed for a 0.01 M solution.