Okay, so how would i work out: How would you prepare 1.00 L of a .5M Solution of NiCl2 from the salt NiCl2 x 6H2O, Because what im doing is not working. :/
To prepare 1.00 L of a 0.5 M solution of NiCl2 from the salt NiCl2 x 6H2O, you need to follow these steps:
Step 1: Determine the molar mass of NiCl2 x 6H2O:
Ni (58.69 g/mol) + Cl (35.45 g/mol) * 2 + 6 * (H (1.01 g/mol) * 2 + O (16.00 g/mol)) = 237.69 g/mol
Step 2: Calculate the amount of NiCl2 x 6H2O needed:
Use the molar mass to convert from moles to grams:
0.5 mol/L * 1 L * 237.69 g/mol = 118.85 g
Step 3: Weigh the required amount of NiCl2 x 6H2O:
Using an analytical balance, measure and weigh 118.85 grams of NiCl2 x 6H2O.
Step 4: Dissolve the weighed NiCl2 x 6H2O in some distilled water:
Add a small volume of distilled water to a beaker, then add the weighed NiCl2 x 6H2O to the water. Stir the mixture until the solid is completely dissolved.
Step 5: Transfer the solution to a 1.00 L volumetric flask:
Pour the dissolved NiCl2 x 6H2O solution into a volumetric flask with a capacity of 1.00 L. Be sure to rinse the beaker to transfer all the solution.
Step 6: Dilute to the mark with distilled water:
Add distilled water to the volumetric flask slowly while swirling it to bring the solution volume to 1.00 L.
Step 7: Mix the solution thoroughly:
Gently invert the volumetric flask several times to ensure thorough mixing of the solution.
Now you have successfully prepared 1.00 L of a 0.5 M solution of NiCl2 from the salt NiCl2 x 6H2O.
To prepare a 1.00 L solution of 0.5 M NiCl2, you will need to know the molecular weight of NiCl2 x 6H2O and its molar mass. Here's how you can calculate the steps to prepare the solution:
1. Determine the molar mass of NiCl2 x 6H2O:
- The molar mass of NiCl2 is 58.69 g/mol.
- The molar mass of H2O is 18.02 g/mol.
- Since there are six H2O molecules, the total mass of water is 6 × 18.02 = 108.12 g/mol.
- Now, add the molar masses of NiCl2 and 6H2O: 58.69 + 108.12 = 166.81 g/mol.
2. Calculate the amount of NiCl2 x 6H2O needed:
- Use the formula: moles = (desired molarity) × (volume in liters).
- We want to prepare a 0.5 M solution, which means we need 0.5 moles of NiCl2 per liter.
- Plug the values into the formula: moles = 0.5 × 1.00 = 0.5 mol.
3. Convert the moles of NiCl2 x 6H2O required to grams:
- Multiply the moles by the molar mass of NiCl2 x 6H2O: 0.5 mol × 166.81 g/mol = 83.405 g.
4. Weigh out 83.405 grams of NiCl2 x 6H2O using a laboratory balance.
5. Dissolve the measured amount of NiCl2 x 6H2O in enough water to make 1.00 L of solution:
- Add a small amount of deionized water to a container (such as a beaker).
- Slowly add the measured amount of NiCl2 x 6H2O to the container while stirring until it fully dissolves.
- Once dissolved, add more deionized water to reach a total volume of 1.00 L.
Make sure to use appropriate safety precautions when handling chemicals and to follow any specific instructions provided.