How would you prepare 1.00 L of a 0.5 M solution of NiCl2 from the salt NiCl2 x 6H2O
Well, first you'll need to tell the salt NiCl2 x 6H2O to stop hogging all the water! It's okay to share, you know?
To prepare your 0.5 M solution of NiCl2, you'll need to know the molar mass of NiCl2. So, let's see... Ni (nickel) has a molar mass of approximately 58.7 g/mol, and Cl (chlorine) has a molar mass of approximately 35.45 g/mol. Oh, and don't forget to count those pesky water molecules too!
So, NiCl2 x 6H2O has a total molar mass of approximately (58.7 + 2 * 35.45 + 6 * (2 * 1.01 + 16.00)) g/mol. Calculate that and you'll get your answer!
Now, to prepare 1.00 L of a 0.5 M solution, you'll need to dissolve the correct mass of NiCl2 x 6H2O in enough water to make 1.00 L of solution. Just make sure to use a really big spoon, okay? Safety first!
But remember, even though this process involves water, it's not an invitation for a pool party. No diving into the solution, I'm sorry to disappoint you!
To prepare a 0.5 M solution of NiCl2 with a final volume of 1.00 L, you'll need to determine the amount of NiCl2 x 6H2O required and the volume of solvent (water) needed.
1. First, calculate the molar mass of NiCl2 x 6H2O:
- The molar mass of NiCl2 = 58.7 g/mol
- The molar mass of 6H2O = 6 * (2 * 1.01 g/mol + 16.00 g/mol) = 180.2 g/mol
- The molar mass of NiCl2 x 6H2O = 58.7 g/mol + 180.2 g/mol = 238.9 g/mol
2. Calculate the amount of NiCl2 x 6H2O required:
- To prepare a 0.5 M solution, you need 0.5 moles of NiCl2 per liter.
- Moles = Molarity (M) * Volume (L)
- Moles = 0.5 mol/L * 1.00 L = 0.5 mol
Since the molar mass of NiCl2 x 6H2O is 238.9 g/mol, you can calculate the required mass of NiCl2 x 6H2O using the following formula:
- Mass (g) = Moles * Molar mass
- Mass (g) = 0.5 mol * 238.9 g/mol = 119.45 g
3. Now, you have determined that you need 119.45 g of NiCl2 x 6H2O to prepare a 0.5 M solution with a final volume of 1.00 L.
4. We'll now move on to the preparation steps:
- Measure and weigh out 119.45 g of NiCl2 x 6H2O on an analytical balance.
- Transfer the weighed salt into a volumetric flask.
- Add some solvent (water) to the flask until it is about half full.
- Swirl the flask gently to dissolve the salt completely.
- Once dissolved, add more solvent (water) to the flask until it reaches the calibrated mark (1.00 L) on the neck of the flask.
- Continue to swirl the flask gently to ensure homogeneity of the solution.
Congratulations! You have now prepared 1.00 L of a 0.5 M solution of NiCl2 from the salt NiCl2 x 6H2O. Remember to label the flask properly with the concentration, date, and any other relevant information.