You need to prepare 2.00 L of 0.100 M Na2CO3 solution. The best procedure is to weigh out…?
To prepare 2.00 L of a 0.100 M Na2CO3 solution, which of the following procedures is correct?
a. Weigh out 10.6 g of Na2CO3 and add 2.00 L of water to it.
b. Weigh out 21.2 g of Na2CO3 and add 2.00 L of water to it.
c. Weigh out 10.6 g of Na2CO3 and add water until the final solution reaches a volume of 2.00 L.
d. Weigh out 21.2 g of Na2CO3 and add water until the final solution reaches a volume of 2.00 L.
2 Answers
Using the Conc and the vol you can find out how many moles you need.
moles = C x V
moles = 0.100 mol/L x 2.00 L = 0.200 mol
Now convert the 0.200 moles back into mass by using mass = moles x molar mass
mass = 0.200 mol x 105.99 g/mol = 21.198 grams.
molar mass of Na2CO3 = 106 g/mol
find out how many moles of Na2CO3 you need:
0.1 mol/L * 2 L = 0.2 mol
multiply by molar mass to get a mass in grams:
0.2 mol * 106 g/mol = 21.2 g
you would dissolve this in enough water so that the final volume is 2 L; you can't just add it to 2 L of water because the solute may occupy some volume such that the final volume would be more than 2 L and the concentration wouldn't be exactly 0.1 M.
so the answer is D
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