An experiment in your laboratory requires 500 mL of a .0200 M solution of Na2CO3. You are given solid Na2CO3, distilled water and a 500 mL volumetric flask Describe how to prepare the required solution showing all calculations and describing each step appropriately.
It is important that you know HOW to prepare a solution.
You want how many moles? That is M x L = 0.02 x 0.500 = ? moles. How many grams is that. grams = moles x molar mass.
That's the easy part. Here is the tricky part. Weigh the grams calculated above exactly, transfer quantitatively to the 500 mL volumetric flask, add a LITTLE water, swirl until ALL of the salt is dissolved, then make to the makr with DI or distilled water. Shake and mix thoroughly. Two important points in my description.
1. You do NOT add the salt to 500 mL H2O because then the solution will be more than (some solutes) or less than(some solutes) when the solute goes into solution.
2. You add the salt to the flask, add some water and swirl until all of the salt is dissolved. See #1 for why.
Well, let's put on our lab coats and get started with this experiment!
Step 1: First, we need to calculate the amount of Na2CO3 required to make a 0.0200 M solution in 500 mL.
The formula weight of Na2CO3 is 105.99 g/mol. To calculate the mass required, we can use the formula:
Mass (g) = Molarity (mol/L) x Volume (L) x Formula Weight (g/mol).
Mass (g) = 0.0200 mol/L x 0.500 L x 105.99 g/mol.
Mass (g) = 1.0598 g.
So, we need 1.0598 grams of Na2CO3.
Step 2: Now, using a weighing balance, measure out 1.0598 grams of solid Na2CO3.
Step 3: Transfer the solid Na2CO3 to the 500 mL volumetric flask.
Step 4: Fill the volumetric flask with distilled water, gradually bringing the volume up to the 500 mL mark. Keep swirling gently to ensure complete dissolution.
Step 5: Once the Na2CO3 is fully dissolved, stop adding water and make sure the bottom of the meniscus aligns precisely with the 500 mL mark on the volumetric flask.
Step 6: Give the flask a good mix to ensure homogeneity. You can try some fancy moves like the "volumetric flask shuffle" if you'd like.
Congratulations! You have successfully prepared a 500 mL solution of 0.0200 M Na2CO3. Be sure to label it properly and keep it away from any clowns who might mistake it for their fizzy drink!
To prepare a 0.0200 M solution of Na2CO3 with a volume of 500 mL, you will need to follow these steps:
1. Calculate the mass of Na2CO3 required:
- Determine the molar mass of Na2CO3:
- Na: 2(22.99 g/mol) = 45.98 g/mol
- C: 1(12.01 g/mol) = 12.01 g/mol
- O: 3(16.00 g/mol) = 48.00 g/mol
- Total molar mass = 45.98 + 12.01 + 48.00 = 105.99 g/mol
- Calculate the mass of Na2CO3 needed using the formula:
- Mass = molarity (M) × volume (V) × molar mass (MM)
- Mass = 0.0200 mol/L × 0.500 L × 105.99 g/mol = 1.0598 g
2. Weigh out 1.0598 g of Na2CO3 using an analytical balance.
3. Transfer the weighed Na2CO3 into the 500 mL volumetric flask.
4. Fill the volumetric flask with distilled water until the bottom of the meniscus reaches the mark on the neck of the flask.
5. Mix the solution gently to ensure complete dissolution of Na2CO3.
6. Verify that the total volume of the solution is 500 mL by checking the bottom of the meniscus against the mark on the neck of the flask.
Once you have completed these steps, you will have successfully prepared a 0.0200 M solution of Na2CO3 with a volume of 500 mL in the laboratory.
To prepare the required solution of Na2CO3, you will need the solid Na2CO3, distilled water, and a 500 mL volumetric flask. Here's a step-by-step guide on how to prepare the solution:
Step 1: Calculate the amount of Na2CO3 needed
The concentration of the solution required is 0.0200 M, which means there are 0.0200 moles of Na2CO3 in one liter of solution. Since we want to prepare a 500 mL solution, we need to calculate the amount of Na2CO3 required in moles.
Moles of Na2CO3 = Concentration (Molarity) × Volume (L)
Moles of Na2CO3 = 0.0200 mol/L × 0.500 L
Step 2: Convert moles to grams
To convert moles of Na2CO3 to grams, we need to know the molar mass of Na2CO3. The molar mass of Na2CO3 is the sum of the atomic masses of sodium (Na), carbon (C), and three oxygen (O) atoms.
Molar mass of Na2CO3 = (2 × atomic mass of Na) + atomic mass of C + (3 × atomic mass of O)
Molar mass of Na2CO3 = (2 × 23.0 g/mol) + 12.0 g/mol + (3 × 16.0 g/mol)
Step 3: Weigh the solid Na2CO3
Using a balance or a weighing scale, measure out the required amount of Na2CO3. Since the molar mass of Na2CO3 is known, you can calculate the mass of Na2CO3 needed.
Mass of Na2CO3 = Moles of Na2CO3 × Molar mass of Na2CO3
Step 4: Dissolve the Na2CO3 in a portion of water
Add some distilled water to a beaker, and then slowly add the measured mass of Na2CO3 into the water. Stir the solution until all the solid Na2CO3 is dissolved.
Step 5: Transfer the solution to a volumetric flask
After the Na2CO3 is completely dissolved, transfer the solution into the 500 mL volumetric flask. Be sure to use a funnel to minimize spills. Rinse the beaker with small portions of distilled water to ensure all the Na2CO3 is transferred.
Step 6: Fill the volumetric flask with distilled water
Add distilled water to the volumetric flask until it reaches the 500 mL mark. Be careful not to go over the mark. Use a dropper or a wash bottle to add the water more precisely.
Step 7: Mix the solution
Carefully invert the volumetric flask a few times to ensure thorough mixing of the Na2CO3 solution.
Now, you have successfully prepared a 500 mL solution of Na2CO3 with a concentration of 0.0200 M.