After titration, 25 mL of a vinegar solution was found to contain 0.03 moles of acetic acid. Using a density of 1.00 g/mL, what is the mass percentage of acetic acid

Question

After titration, 25 mL of a vinegar solution was found to contain 0.03 moles of acetic acid. Using a density of 1.00 g/mL, what is the mass percentage of acetic acid in this vinegar sample? Report your answer to three decimal places.

Answer 1

The key to calculating quantities in chemistry is to use factor labeling to obtain extensive (depend on mass) variables like mass, volume, area, length, moles, time, energy. All of them describe "how much stuff" you are dealing with. In order to find mass percent of acetic acid you need the mass of acetic acid and you divide by the mass of solution (getting the mass fraction of acetic acid) and multiply by 100.

m_AA = .03 moles AA *( g/mole of AA) = g of AA where g/mole of Acetic Acid can be calculated or looked up.

m_VS = 25 ml VS * (1.00 grams/ml VS solution) = g of Vinegar Solution (I don't know why the density is like water to 3 places - should be 1.01 g/ml)

Now do the division and multiply be 100 to make it percent.

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