Posted by Toni on Saturday, March 3, 2007 at 7:37pm.
Trying to find mass percent of acetic acid in 25 drops of .683M NaOH solution are required to neutralize 10 drops of cleaning vinegar. Assume that the density of the cleaning vinegar is the same as the density of regular vinegar which is 1.05 g ml-1
You need to clean up the post some. As it now reads, "Trying to find the mass percent of acetic acid in 25 drops of .683M NaOH solution are required to neutralize 10 drops of cleaning vinegar." I doubt there is ANY acetic acid in .683M NaOH. I assume it should read, "Trying to find the mass percent of acetic acid. 25 drops of 0.683M NaOH are required to neutralize 10 drops of cleaning vinegar.
drops vinegar x M = drops NaOH x M
Solve for M vinegar.
Now, do you know the size of a drop? or the mass of the drop? Or can you find percent from the molarity and the density?
A nationally known company markets a product called "cleaning vinegar" that is not designed for human consumption. What is the mass percent of acetic acid in this product, if 25 drops of .0683M NaOH solution are required to neutralize 10 drops of the cleaning vinegar? Assume that the denisty of the cleaning vinegar is the same as the density of regular vinegar, which is 1.005 g ml^-1.
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