A student must prepare 2.00 L of 0.100 M Na2CO3 (106 g/mol) Which is the besst procedure for preparing this solution ?
Answered elsewhere, I don't know if above or below.
To prepare a 2.00 L solution of 0.100 M Na2CO3, you will need to follow these steps:
1. Determine the amount of Na2CO3 needed:
Start by calculating the number of moles of Na2CO3 required. You can use the formula:
Moles = Molarity (M) x Volume (L)
Moles = 0.100 M x 2.00 L
2. Calculate the mass of Na2CO3 required:
Use the molar mass of Na2CO3 (106 g/mol) to convert moles to grams:
Mass (g) = Moles x Molar mass
Mass (g) = Moles x 106 g/mol
3. Weigh the appropriate amount of Na2CO3:
Use a digital balance or analytical balance to measure the calculated mass of Na2CO3. Make sure to zero the scale before weighing to get an accurate measurement.
4. Dissolve Na2CO3 in water:
Add a small volume of water to a container that will hold at least 2.00 L of solution. Slowly add the measured Na2CO3 to the water and stir gently until it dissolves completely.
5. Transfer the solution to a volumetric flask:
To ensure accurate volume measurement, use a funnel to transfer the solution from the container to a clean and dry 2.00 L volumetric flask. Rinse the container with a small amount of water to ensure you transfer all the solution.
6. Bring the solution to the mark:
Add distilled water to the volumetric flask until the bottom of the meniscus is precisely at the mark on the neck of the flask. Use a dropper or a wash bottle to add water in small increments, allowing the solution to mix thoroughly after each addition.
7. Cap and invert the flask:
Secure the cap tightly and invert the flask multiple times to ensure the solution is homogeneously mixed.
Now you have successfully prepared a 2.00 L solution of 0.100 M Na2CO3.