Develop a method to prepare 100 ml of 0.500mol/l aqueous CuSO4x5H2O solution. Include the water molecules that are hydrated to the crystals as given in the molecular formula, in your calculation of the molar mass. show all your calculations. Prepare the solution.
I don't know about this being a method; it is a procedure for doing the job.
How many mols do you want? That's M x L = ?
Then mols = grams CuSO4*5H2O/molar mass CuSO4*5H2O = ?.
Place that many grams CuSO4*5H2O in a 100 mL volumetric flask, add some water, swirl until dissolved, then fill to the mark on the volumetric flask with distilled or deionized water. Mix thoroughly. stopper.
To prepare a 0.500 mol/L aqueous CuSO4·5H2O solution, you need to follow these steps:
Step 1: Calculate the molar mass of CuSO4·5H2O:
The molar mass of copper(II) sulfate pentahydrate (CuSO4·5H2O) can be calculated by adding the molar masses of its constituents:
M(CuSO4·5H2O) = M(Cu) + M(S) + 4 * M(O) + 5 * (2 * M(H) + M(O))
From the periodic table:
M(Cu) = 63.55 g/mol, M(S) = 32.07 g/mol, M(O) = 16.00 g/mol, M(H) = 1.01 g/mol
Substituting the values into the formula:
M(CuSO4·5H2O) = 63.55 + 32.07 + 4 * 16.00 + 5 * (2 * 1.01 + 16.00)
M(CuSO4·5H2O) = 63.55 + 32.07 + 64.00 + 5 * (2.02 + 16.00)
M(CuSO4·5H2O) = 63.55 + 32.07 + 64.00 + 5 * 18.02
M(CuSO4·5H2O) = 63.55 + 32.07 + 64.00 + 90.10
M(CuSO4·5H2O) = 249.72 g/mol
Step 2: Calculate the mass of CuSO4·5H2O needed:
For a 100 mL solution of 0.500 mol/L concentration, we need to prepare 0.5 mol/L × 0.100 L = 0.0500 mol of CuSO4·5H2O.
The mass can be calculated using the formula:
Mass = moles × molar mass
Mass(CuSO4·5H2O) = 0.0500 mol × 249.72 g/mol
Mass(CuSO4·5H2O) = 12.49 g
Therefore, 12.49 grams of CuSO4·5H2O is needed to prepare a 100 mL solution of 0.500 mol/L concentration.
Step 3: Prepare the solution:
To prepare the solution, follow these steps:
1. Weigh out 12.49 grams of CuSO4·5H2O using a balance.
2. Transfer the weighed compound into a clean and dry 100 mL volumetric flask.
3. Add distilled water to the flask gradually while stirring until the volume reaches the 100 mL mark on the flask.
4. Continue stirring until the CuSO4·5H2O has completely dissolved in the water.
5. The resulting solution is a 0.500 mol/L CuSO4·5H2O solution.
Remember to exercise caution when handling chemicals and follow appropriate safety protocols.
To prepare a 100 ml solution of 0.500 mol/L copper (II) sulfate pentahydrate (CuSO4⋅5H2O), we need to determine the mass of CuSO4⋅5H2O required.
1. Calculate the molar mass of CuSO4⋅5H2O:
- Molar mass of Cu = 63.55 g/mol
- Molar mass of S = 32.07 g/mol
- Molar mass of O (4 atoms) = 16.00 g/mol * 4 = 64.00 g/mol
- Molar mass of H (10 atoms) = 1.01 g/mol * 10 = 10.10 g/mol
- Total molar mass = (63.55 + 32.07 + 64.00 + 10.10) g/mol = 169.72 g/mol
2. Calculate the mass of CuSO4⋅5H2O required using the molar mass and desired molarity:
- Moles of CuSO4⋅5H2O = 0.500 mol/L * 0.100 L = 0.0500 mol
- Mass of CuSO4⋅5H2O = Moles * Molar mass
= 0.0500 mol * 169.72 g/mol = 8.486 g
Therefore, you will need to measure 8.486 grams of CuSO4⋅5H2O to prepare the solution.
To prepare the solution:
1. Weigh 8.486 grams of CuSO4⋅5H2O using a digital scale.
2. Transfer the weighed CuSO4⋅5H2O crystals into a clean and dry 100 ml volumetric flask.
3. Add distilled water slowly to the flask up to the mark (100 ml) on the neck of the flask.
4. Mix the solution thoroughly by swirling the flask gently until all the CuSO4⋅5H2O crystals dissolve.
You now have a 100 ml solution of 0.500 mol/L aqueous CuSO4⋅5H2O.