1. Calculate the mass needed:
* Molar mass of CuSO₄·4H₂O:
* Cu: 63.55 g/mol
* S: 32.06 g/mol
* O: 16.00 g/mol (x 9 total oxygen atoms)
* H: 1.01 g/mol (x 8 total hydrogen atoms)
* Total molar mass: 249.69 g/mol
* Mass needed:
* 18 mmol * (249.69 g/mol) / (1000 mmol/mol) = 4.49 g
2. Weigh out the copper sulfate tetrahydrate:
* Use a balance to carefully weigh out 4.49 g of copper sulfate tetrahydrate.
3. Dissolve in water:
* Add the weighed copper sulfate tetrahydrate to a suitable container (e.g., a beaker or volumetric flask).
* Add distilled water to dissolve the solid completely.
* The exact volume of water will depend on the desired concentration. If you want a specific concentration, you'll need to calculate the volume of water needed based on the final desired volume.
Important Notes:
* Purity: Always use analytical grade copper sulfate tetrahydrate for accurate results.
* Safety: Copper sulfate is an irritant. Wear appropriate safety goggles and gloves when handling it.
* Solubility: Copper sulfate tetrahydrate is highly soluble in water. Ensure the water volume is sufficient for complete dissolution.
* Concentration: If you need a specific concentration of copper sulfate solution, you'll need to calculate the final volume of water needed.
Example: Making a 0.1 M solution:
* Desired volume: Let's say you want 100 mL of a 0.1 M solution.
* Moles of CuSO₄·4H₂O needed: 0.1 mol/L * 0.1 L = 0.01 mol
* Mass of CuSO₄·4H₂O needed: 0.01 mol * 249.69 g/mol = 2.497 g
* Dissolve the 2.497 g in water and bring the final volume up to 100 mL.
Let me know if you have any more questions about making a specific concentration of copper sulfate solution!
