how much CuSO4.5H2O is required to prepare 100 ml of a .050M aqueous stock solution?
How many moles do you want?
M x L = 0.050 x 0.1 L = ??
That many moles CuSO4.5H2O = grams/molar mass.
u suckk
1.25g?
To determine how much CuSO4·5H2O is required to prepare a 100 ml of a 0.050 M aqueous stock solution, we need to use the equation:
Molarity (M) = moles/volume (L)
First, we need to find the number of moles needed in 100 ml of the solution:
moles = Molarity × volume (in liters)
= 0.050 mol/L × 0.100 L
= 0.005 mol
The molar mass of CuSO4·5H2O can be calculated as follows:
1 Cu: 63.55 g/mol
1 S: 32.07 g/mol
4 O: 16.00 g/mol × 4 = 64.00 g/mol
10 H2O: 18.02 g/mol × 10 = 180.2 g/mol
Summing these masses, we find:
Molar mass of CuSO4·5H2O = 63.55 + 32.07 + 64.00 + 180.2 = 339.82 g/mol
Using the molar mass, we can then calculate the mass needed of CuSO4·5H2O:
mass (g) = moles × molar mass
= 0.005 mol × 339.82 g/mol
≈ 1.70 g
Therefore, approximately 1.70 grams of CuSO4·5H2O is needed to prepare a 100 ml of a 0.050 M aqueous stock solution.