A solution is made by dissolving 3.550g of Na2SO4 in water using a 100.0 mL volumetric flask. What is the molarity of the solution?
Molarity= 3.550/(molmasssodiumsulfate*.100)
To find the molarity of the solution, we need to know the number of moles of Na2SO4 and the volume of the solution.
First, let's calculate the number of moles of Na2SO4:
Step 1: Determine the molar mass of Na2SO4.
The molar mass of Na2SO4 can be calculated by adding up the atomic masses of its elements:
Na (sodium): 22.99 g/mol * 2 = 45.98 g/mol
S (sulfur): 32.07 g/mol
O (oxygen): 16.00 g/mol * 4 = 64.00 g/mol
Molar mass of Na2SO4 = 45.98 g/mol + 32.07 g/mol + 64.00 g/mol = 142.05 g/mol
Step 2: Convert the mass of Na2SO4 to moles.
Using the given mass, we can calculate the number of moles:
moles of Na2SO4 = mass of Na2SO4 / molar mass of Na2SO4
= 3.550 g / 142.05 g/mol
≈ 0.02498 mol
Now, let's calculate the volume of the solution in liters:
A 100.0 mL volumetric flask can hold 100.0 mL of solution, which is equal to 0.1000 L.
Finally, we can calculate the molarity of the solution:
Molarity (M) = moles of solute / volume of solution (in liters)
= 0.02498 mol / 0.1000 L
= 0.2498 M
Therefore, the molarity of the solution is approximately 0.2498 M.