Describe how you would prepare 0.05 mol.dm-3 sodium carbonate in a total volume 250 mls.
For a 0.05 M (that's 0.05 mol/dm^3) Na2CO3 in 250 mL, how many mols Na2CO3 is that? That's mols = M x L = 0.05 M x 0.250 L = 0.0125 mols.
Then mols = grams/molar mass. You know mols and molar mass, solve for grams. To prepare such a solution, you add the grams Na2CO3 to an empty (and dry) 250 mL volumetric flask. Add about 100 mL distilled (or deionized) water, swirl until Na2CO3 is dissolved, then add water to the mark on the volumetric flask. Stopper, mix thoroughly, label. Done.
Good and helpful
Well, to prepare 0.05 mol.dm-3 sodium carbonate in a total volume of 250 ml, you'll need to put on your lab coat and grab your comedy goggles. It's time to make some science-infused laughter!
First, let's break it down. We have 0.05 mol.dm-3, which is like trying to catch a slippery banana in a chemistry lab. This just means that we have 0.05 moles of sodium carbonate dissolved in every liter of solution.
Since we want to make a total volume of 250 ml, we need to do some math tricks. Remember, math is like juggling rubber chickens – it takes a little practice, but it's entertaining nonetheless!
We'll start by calculating how many moles we need. We have a volume of 250 ml, which is like having a tiny pool party for molecules. So, multiplying our volume by the molarity, we get: 0.05 mol.dm-3 * 0.25 dm3 = 0.0125 moles.
Now it's time to add some water and create our sodium carbonate solution. Just make sure to use distilled water, and not water from the squirting flowers in your clown pocket! Pour enough water into a beaker to reach the 250 ml mark, which is like filling up a fish tank but with less swimming and more chemistry.
Once you've added the water, it's time to add the sodium carbonate. With a smirk on your face, carefully measure out 0.0125 moles worth of sodium carbonate, making sure not to spill it or accidentally turn it into a clown wig.
Add the sodium carbonate to the beaker and give it a good stir. Imagine you're whipping up an invisible batch of clown confetti cake batter, but instead, you're creating a delightful sodium carbonate solution.
Now comes the grand finale! Put on your laboratory clown shoes and mix everything thoroughly, making sure the sodium carbonate is completely dissolved. You should end up with a 0.05 mol.dm-3 sodium carbonate solution in a total volume of 250 ml.
And just like that, you've successfully prepared your sodium carbonate solution! Don't forget to take a bow and throw some chemical humor into the mix. After all, chemistry is just science's way of clowning around!
To prepare a 0.05 mol.dm-3 sodium carbonate solution in a total volume of 250 mL, follow these steps:
1. Determine the required amount of sodium carbonate (Na2CO3) using the equation:
Moles = Molarity × Volume
Moles = 0.05 mol.dm-3 × 0.250 dm3
= 0.0125 mol
Therefore, you will need 0.0125 moles of sodium carbonate.
2. Calculate the molar mass of sodium carbonate (Na2CO3).
The molar mass is calculated by adding up the atomic masses of each element:
Molar mass of Na2CO3 = (2 × atomic mass of Na) + atomic mass of C + (3 × atomic mass of O)
= (2 × 22.99 g/mol) + 12.01 g/mol + (3 × 16.00 g/mol)
= 105.99 g/mol
Therefore, the molar mass of sodium carbonate is 105.99 g/mol.
3. Calculate the mass of sodium carbonate required.
To calculate the mass, use the equation:
Mass = Moles × Molar mass
Mass = 0.0125 mol × 105.99 g/mol
= 1.3249 g
≈ 1.325 g
Therefore, you need approximately 1.325 grams of sodium carbonate.
4. Measure out the required amount of sodium carbonate accurately using a balance and transfer it into a clean and dry container.
5. Add distilled water incrementally to the sodium carbonate while stirring gently until the total volume reaches 250 mL.
6. Stir the solution thoroughly to ensure complete dissolution of sodium carbonate.
Note: Always wear appropriate personal protective equipment (PPE) when working with chemicals, including goggles and gloves.