How to prepare 0.1 M stock solution of KMnO4 in 100ml?
How many moles do you need? That's M x L = 0.1 M x 0.1 L = ?
Then mols = grams/molar mass.
You know mols and molar mass, solve for grams KMnO4.
Then place that many grams KMnO4 in a 100 mL volumetric flask, add some distilled water, swirl until all of the solid is dissolved, add distilled water to the mark of the volumetric flask, mix thoroughly, stopper, label.
NOTE: This doesn't sound like a stock solution to me. A stock solution usually is some larger molarity (such as 1M or something like that) then by dilution you make a 100 mL of 0.1 M from the stock. Stock solutions have an advantage of preparing them and saving for future use; however, KMnO4 solutions are not stable and usually they are made as needed.
Well, creating a stock solution of KMnO4 is simple. Just follow these steps:
1. Put 100ml of water in a beaker.
2. Bring the beaker to a rolling boil.
3. Now, summon your inner chemist and, while twirling your mustache, add precisely 0.1 moles of KMnO4 to the boiling water.
4. After a brief stirring with a comically oversized spoon, let the solution cool down.
5. Voila! You now have a 0.1 M stock solution of KMnO4 ready to delight all your experiments.
Remember, though, that KMnO4 is a powerful oxidizing agent, so handle it with care and don't let it oxidize your sense of humor!
To prepare a 0.1 M stock solution of KMnO4 in 100 mL, follow these steps:
1. Calculate the molar mass of KMnO4:
- The molar mass of potassium (K) is 39.10 g/mol.
- The molar mass of manganese (Mn) is 54.94 g/mol.
- The molar mass of oxygen (O) is 16.00 g/mol.
- Multiply the atomic masses by the number of atoms in the formula and sum them up: (39.10)+(54.94)+(4x16.00) = 158.04 g/mol.
2. Calculate the required amount of KMnO4:
- 0.1 M refers to 0.1 moles of KMnO4 dissolved in 1 liter (1000 mL) of solution.
- For a 0.1 M solution, you need 0.1 moles of KMnO4 in 1000 mL of solution.
- Since you want to prepare a 100 mL stock solution, you need to use a proportion to calculate the amount:
(0.1 mol/1000 mL) = (x mol/100 mL).
- Solving the proportion gives you x = 0.01 moles.
3. Calculate the mass of KMnO4 required:
- Use the molar mass of KMnO4 calculated earlier to convert moles to grams.
- Mass (g) = Moles (mol) x Molar mass (g/mol).
Mass = 0.01 mol x 158.04 g/mol = 1.58 g.
4. Weigh out 1.58 grams of KMnO4 and transfer it to a container, preferably a beaker or a volumetric flask.
5. Add distilled water to the container and dissolve the KMnO4 until the volume reaches 100 mL.
6. Carefully mix the solution until the compound is fully dissolved.
Note: Always wear appropriate personal protective equipment (PPE), such as gloves and goggles, when handling chemicals. Additionally, be cautious when working with KMnO4, as it is a strong oxidizing agent.
To prepare a 0.1 M stock solution of KMnO4 in 100 ml, you will need to follow these steps:
1. Determine the molar mass of KMnO4:
- The molar mass of potassium (K) is 39.1 g/mol.
- The molar mass of manganese (Mn) is 54.9 g/mol.
- The molar mass of oxygen (O) is 16.0 g/mol (there are four oxygen atoms in KMnO4).
Adding these values together, we have:
39.1 g/mol (K) + 54.9 g/mol (Mn) + 4 * 16.0 g/mol (O) = 158.0 g/mol.
2. Calculate the mass of KMnO4 needed:
- Molarity (M) is defined as moles of solute per liter of solution.
- In this case, we want to prepare a 0.1 M solution in 100 ml (0.1 liters).
- The formula to calculate mass is: mass = Molarity * molar mass * volume.
Using the given parameters:
mass = 0.1 mol/L * 158.0 g/mol * 0.1 L = 1.58 g.
Therefore, you will need 1.58 grams of KMnO4 to prepare a 0.1 M stock solution.
3. Dissolve KMnO4 in a small volume of distilled water:
- Weigh out 1.58 grams of KMnO4 and place it in a beaker.
- Add a small volume of distilled water to the beaker and stir vigorously until the KMnO4 is completely dissolved.
4. Transfer the solution to a 100 ml volumetric flask:
- Once the KMnO4 is completely dissolved, carefully transfer the solution to a 100 ml volumetric flask.
- Rinse the beaker multiple times to ensure that all of the KMnO4 is transferred to the flask.
- Then, fill the flask up to the mark with distilled water, using a dropper or pipette to achieve precision.
5. Mix the solution thoroughly:
- Use a stopper or a cap to seal the volumetric flask.
- Gently invert the flask several times to mix the solution thoroughly.
Congratulations! You have successfully prepared a 0.1 M stock solution of KMnO4 in 100 ml. Remember to label the flask with the concentration and contents.