A sample of oxalic acid, H2C2O4, weighing 1.294 g is placed in a 100.0 mL volumetric flask, which is then filled to the mark with water. What is the molarity of the solution?
would the moles be .014?
Remember the definition of molarity.
M = # mols/L.
Convert 1.294 g H2C2O4 to mols.
Then #mols/0.1 L = ??M
Close. The # mols = 1.294/90.035 = 0.014406 which rounds to 0.01441. You have 4 significant figures in 1.294; therefore, you may have that many in the answer.
Oxalic acid? That sounds a bit acidic to me. It's like the grumpy aunt of the acid family. Anyway, let's calculate the molarity of this solution!
First, we need to calculate the number of moles of oxalic acid. The molar mass of H2C2O4 is 90.03 g/mol. So, 1.294 g of oxalic acid is equal to 1.294 g / 90.03 g/mol = 0.01437 mol.
Next, we determine the volume of the solution in liters. The 100.0 mL volumetric flask is equal to 0.100 L.
Now, to calculate the molarity, we divide the number of moles by the volume in liters: 0.01437 mol / 0.100 L = 0.1437 M.
So, the molarity of the solution is approximately 0.1437 M. That's one acidic solution, but don't worry, it won't burn your taste buds like a bad joke!
To find the molarity of the solution, we need to know the number of moles of oxalic acid and the volume of the solution.
First, let's calculate the number of moles of oxalic acid:
1. Calculate the molar mass of oxalic acid (H2C2O4):
H: 2 * 1.008 g/mol = 2.016 g/mol
C: 2 * 12.01 g/mol = 24.02 g/mol
O: 4 * 16.00 g/mol = 64.00 g/mol
Total mass = 2.016 + 24.02 + 64.00 = 90.036 g/mol
2. Convert the mass of the oxalic acid sample to moles:
Moles = mass / molar mass
Moles = 1.294 g / 90.036 g/mol ≈ 0.01438 mol
Next, we need to find the volume of the solution. The volume is given as 100.0 mL, which is the same as 0.1000 L.
Finally, we can calculate the molarity using the formula:
Molarity (M) = moles / volume
Molarity = 0.01438 mol / 0.1000 L ≈ 0.1438 M
Therefore, the molarity of the solution is approximately 0.1438 M.