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 a 0.5M solution of NiCl2 from NiCl2 x 6H2O, you need to follow these steps:
1. Determine the molar mass of NiCl2 x 6H2O:
- The molar mass of Ni is 58.69 g/mol.
- The molar mass of Cl is 35.45 g/mol.
- The molar mass of H2O is 18.02 g/mol.
- So, the molar mass of NiCl2 x 6H2O is (58.69 + (2 * 35.45) + (6 * 18.02)) g/mol.
2. Calculate the amount of NiCl2 x 6H2O needed:
- You want to prepare a 0.5M solution, which means you need 0.5 moles of NiCl2 per liter of solution.
- The molarity (M) is defined as moles of solute per liter of solution.
- So, the amount of NiCl2 x 6H2O needed is (0.5 moles/L) * (molar mass of NiCl2 x 6H2O) g.
3. Convert the amount of NiCl2 x 6H2O to grams:
- Multiply the amount of NiCl2 x 6H2O (in moles) by its molar mass (in grams/mole).
4. Determine the volume of water needed:
- You want to prepare 1.00 L of the final solution, so you need to add enough water to reach that volume.
5. Dissolve NiCl2 x 6H2O in water:
- Add the calculated amount of NiCl2 x 6H2O to the determined volume of water.
- Stir or shake the solution until all the salt is dissolved.
By following these steps, you should be able to prepare a 0.5M solution of NiCl2 from NiCl2 x 6H2O.
masssalt=molarity*volume*molmassSalt
so figure the mole mass of NiCl2.6H2O
then figure the mass of salt needed from the first formula. In my head you need about 90 grams.