m1v1 = m2v2 technically isn't the one to use but it will work in this case. The REAL problem is that you don't have the concentration of the HCl. Without that you're dead in the water. You work the problem this way IF you had the molarity of the HCl.
mols HCl = M x L = ?M x 0.0100
mols NaOH = mols HCl from line 1.
M NaOH = mols NaOH/L NaOH. YOu know M and mols, solve for L and convert to mL if desired.
The flask shown here contains 10.0 ml of HCl and a few drops of phenolphthalein indicator. The buret contains 30ml of 0.130M NaOH.
What Volume of NaOH is needed to reach the end point of the titration?
I've used
m1v1=m2v2,
(x)(10.0ml HCl) = (0.130 M/L NaOH) (0.03L)
and have gotten 3.9ml. But I know that I am wrong.
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