Answer :
Answer:
The answer to your question is letter C
Explanation:
Data
Volume = 2 L
Molarity = 0.100 M
Molecular weight Na₂CO₃ = (2 x 23) + (1 x 12) + (3 x 16)
= 46 + 12 + 48
= 106 g
Process
1.- Calculate the grams of Na₂CO₃ needed
106 g ---------------- 1 mol
x ---------------- 0.1 moles
x = (0.1 x 106) / 1
x = 10.6 g
2.- Calculate the grams of Na₂CO₃ needed for 2 liters of solution
10.6 g -------------- 1 liter
x -------------- 2 liters
x = (10.6 x 2) / 1
x = 21.2 grams of Na₂CO₃
Final answer:
To prepare a 2.00 L of 0.100 M Na2CO3 solution, you should weigh out 21.2 g of Na2CO3 and then add water until the final solution volume is 2.00 L.
Explanation:
The subject of this question is Chemistry and it involves the preparation of a solution using Sodium Carbonate (Na2CO3). The question is asking you to identify the best procedure for preparing a 2.00L of 0.100M Na2CO3 solution. The molar mass of Na2CO3 is approximately 105.99 g/mol.
To calculate the amount of Na2CO3 needed, we use the formula: moles = Molarity * Volume. Thus, moles = 0.100 mol/L * 2.00L = 0.200 moles. Multiplying by the molar mass gives us the mass of Na2CO3 we need: 0.200 moles * 105.99 g/mol = 21.2g.
Therefore, the correct answer is option C - weigh out 21.2g of Na2CO3 and then add water until the final solution has a volume of 2.00L. It's crucial to add water until the final solution is 2.00L, as the volume of water does not equate to the volume of the solution.
Learn more about Solution Preparation here:
https://brainly.com/question/37304944
#SPJ3
