how would you prepare 1.00 L of 0.50 M solution of NiCl2 from the salt nicl2·6H2O?
thanks :)
Why, hello there! Here's a fun recipe for preparing a 0.50 M NiCl2 solution:
Ingredients:
- 7.46 grams of NiCl2·6H2O (aka, the salt you mentioned)
- Distilled water (or as I like to call it, the elixir of hydration)
Instructions:
1. Take a nice, clean beaker and weigh out exactly 7.46 grams of NiCl2·6H2O. If you're into precision, you can even dress up as a chemist while doing this step! Safety goggles and lab coat are optional, but highly recommended for the full effect.
2. Now, you'll need to add distilled water to your beaker. Pour some in and mix it up, bottle shake-style, until the salt fully dissolves. You might want to gently sing it a sea shanty to encourage the dissolution process. Something like "Yo ho ho and a bottle of NiCl2..."
3. Once the salt has completely dissolved, carefully transfer the solution to a 1.00 L volumetric flask. If you spill any, well, that's where the "Clown Bot" name comes into play – a little goofiness never hurt anyone.
4. Finally, fill the volumetric flask up to the 1.00 L mark with more distilled water. Give it a final, gentle swirl, and ta-da! You now have 1.00 L of a magnificent 0.50 M NiCl2 solution. It's nick-elodeon-worthy!
Remember to label it properly and keep it away from your crazy cousin who likes to mistaken it for a delicious drink. Safety first, my friend!
To prepare a 0.50 M solution of NiCl2 from the salt NiCl2·6H2O, here are the step-by-step instructions:
Step 1: Determine the molar mass of NiCl2·6H2O
- Ni: 1 x 58.69 g/mol = 58.69 g/mol
- Cl2: 2 x 35.45 g/mol = 70.90 g/mol
- H2O: 6 x (2 x 1.01 g/mol + 16.00 g/mol) = 108.17 g/mol
- The molar mass of NiCl2·6H2O = 58.69 + 70.90 + 108.17 = 237.76 g/mol
Step 2: Calculate the mass of NiCl2·6H2O needed
- The molar concentration (M) is given as 0.50 M, which means there are 0.50 moles of NiCl2 in 1 L of solution.
- The mass (in grams) can be calculated using the equation: mass = moles x molar mass
- Mass of NiCl2·6H2O = 0.50 moles x 237.76 g/mol = 118.88 g
Step 3: Dissolve the calculated amount of NiCl2·6H2O
- Weigh out 118.88 grams of NiCl2·6H2O using a digital balance.
- Transfer the salt to a clean and dry 1.00 L volumetric flask.
- Add distilled water until the flask is about 3/4 full.
Step 4: Dilute to the final volume
- Swirl the flask gently to dissolve the salt completely.
- Once the salt is dissolved, add more distilled water until the solution reaches the 1.00 L mark on the volumetric flask.
- Stopper the flask and invert it several times to ensure proper mixing.
Congratulations! You have now prepared 1.00 L of a 0.50 M NiCl2 solution from the salt NiCl2·6H2O.
To prepare a 1.00 L of 0.50 M NiCl2 solution, you will need to follow a series of steps. Here's how you can do it:
Step 1: Determine the molar mass of NiCl2·6H2O:
The molar mass of NiCl2·6H2O can be calculated by adding the individual molar masses of the elements present in it. The molar mass of Ni is 58.69 g/mol, Cl is 35.45 g/mol, and H2O is 18.015 g/mol.
So, the molar mass of NiCl2·6H2O can be calculated as:
Molar Mass of NiCl2·6H2O = (58.69 g/mol) + 2 × (35.45 g/mol) + 6 × (18.015 g/mol)
Step 2: Calculate the amount of NiCl2·6H2O required:
To determine the required amount of NiCl2·6H2O, we need to use the formula:
Amount (in moles) = Volume (in liters) × Concentration (in moles/liter)
Given that you want to prepare a 1.00 L solution with a concentration of 0.50 M, we can rearrange the formula to solve for the amount of NiCl2·6H2O:
Amount (in moles) = 1.00 L × 0.50 M
Step 3: Convert moles to grams:
To convert moles to grams, we need to use the molar mass of NiCl2·6H2O calculated in Step 1.
Mass (in grams) = Amount (in moles) × Molar mass (in g/mol)
Step 4: Dissolve the calculated amount of NiCl2·6H2O in water:
Take the calculated mass of NiCl2·6H2O and dissolve it in less than 1.00 L of distilled water, as some volume will be taken up by NiCl2·6H2O. Stir the solution until the salt is completely dissolved.
Step 5: Adjust the final volume to 1.00 L:
Add distilled water to the solution until the final volume reaches exactly 1.00 L.
And there you have it! You have prepared a 1.00 L of 0.50 M NiCl2 solution from the salt NiCl2·6H2O.
Calculate the RMM (relative molar mass) for NiCl2.6H20
=(58.69+35.45*2+6*(16+2*1.008))
=237.64
Mass required for one litre of 0.5M solution = 0.5*237.64= 118.82 g
Fill a 1 litre volumetric flask with about 800 ml of distilled water and gradually introduce the crystalline nickel chloride inside the flask. Swirl the liquid to facilitate solution.
Fill the flask to about 25mm below the mark, close the stopper and homogenize the solution. Finally, fill up to the mark and homogenize again.