Calculate the mass of solid required to prepare 100 mL of a .50 M aqueous solution copper II sulfate pentahydrate. Help please!!
Molarity=(mass/molmass)/volume
mass= molarity*molmass*volume
To calculate the mass of solid required to prepare the given solution, we need to use the formula:
Moles = Concentration (M) x Volume (L)
First, let's convert the volume from milliliters (mL) to liters (L):
100 mL = 100/1000 L = 0.1 L
Next, we need to determine the moles of copper II sulfate pentahydrate using its molar concentration. The molar concentration (M) is given as 0.50 M.
Moles = 0.50 M x 0.1 L
Moles = 0.05 mol
Now, we need to find the molar mass of copper II sulfate pentahydrate (CuSO4·5H2O). The atomic masses are as follows:
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: 1.008 g/mol
Calculate the molar mass:
Molar mass of CuSO4 = (63.55 g/mol) + (32.07 g/mol) + (4 × 16.00 g/mol)
Molar mass of CuSO4 = 159.61 g/mol
Since there are 5 water molecules (H2O) in the pentahydrate, we need to add the molar mass of water as well:
Molar mass of H2O = (2 × 1.008 g/mol) + (16.00 g/mol)
Molar mass of H2O = 18.02 g/mol
Now, calculate the molar mass of the copper II sulfate pentahydrate:
Molar mass of CuSO4·5H2O = (159.61 g/mol) + (5 × 18.02 g/mol)
Molar mass of CuSO4·5H2O = 249.68 g/mol
Finally, calculate the mass of solid required using the moles and molar mass:
Mass = Moles x Molar mass
Mass = 0.05 mol x 249.68 g/mol
Mass = 12.484 g
To prepare 100 mL of a 0.50 M aqueous solution of copper II sulfate pentahydrate, you will need approximately 12.484 grams of the solid.