How do I prepare 500 ml of a .100 mol/L solution of copper sulphate.
get the molmass of the copper sulfate you are using, I suspect it is not copperIIsulfate (anhydrous), but is copperII sulfate pentahydrate.
At any rate, find the mol mass.
Mass needed: molmass*molarity*volumeinliters.
So take that mass (in grams), add water to make up .5liters, stir, label, and store correctly.
Wash equipment, and your hands.
To prepare a 500 ml solution of 0.100 mol/L copper sulfate, you will need to follow these steps:
Step 1: Calculate the amount of copper sulfate required.
To do this, you need to use the molarity and volume of the solution. The formula you will use is:
Amount (in moles) = Molarity * Volume (in liters)
Given:
Molarity (M) = 0.100 mol/L
Volume (V) = 500 ml = 500/1000 = 0.5 L
Amount (in moles) = 0.100 mol/L * 0.5 L = 0.050 moles
Step 2: Convert the amount of copper sulfate to grams.
You will need the molar mass of copper sulfate, which you can find by summing the atomic masses of its constituent elements. Copper has an atomic mass of 63.55 g/mol, sulfur has a mass of 32.07 g/mol, and oxygen has a mass of 16.00 g/mol.
The formula for copper sulfate is CuSO4, which means there is one copper atom, one sulfur atom, and four oxygen atoms.
Molar mass of CuSO4 = 63.55 g/mol + 32.07 g/mol + (16.00 g/mol * 4) = 159.61 g/mol
Grams = Moles * Molar mass
Grams = 0.050 moles * 159.61 g/mol = 7.98 grams
Step 3: Dissolve the calculated amount of copper sulfate in water.
Weigh out 7.98 grams of copper sulfate using an analytical balance. Place the solid in a clean and dry container, and then add distilled water to make it up to a final volume of 500 ml. Stir the solution well until the copper sulfate completely dissolves.
Note: Always follow safety precautions when handling chemicals, and make sure to wear appropriate protective gear.
Now you have successfully prepared a 500 ml solution of 0.100 mol/L copper sulfate!