chem-acid-base titrations

posted by natash

Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present.

a.write a balanced equation for this neutralization reaction
b.what is the molarity of the acetic acid in this vinegar?
c.If the density of the vinegar is 1.006 g/mL, what is the mass percent of acetic acid in the vinegar?

  1. DrBob222

    HC2H3O2 + NaOH ==> HOH + NaC2H3O2

    Calculate mols NaOH from L x M = ??
    Convert mols NaOH to mols HC2H3O2 using the coefficients in the balanced equation.
    M acetic acid= mols/L.

    Determine mols acetic acid in the 10 mL sample and from that grams acetic acid, then calculate percent from
    [grams acetic acid/mass sample]*100

    Post your work if you get stuck.

  2. natash

    ok for part 2
    moles of NaOH=L*M
    .01*.5052=.005052 moles of NaOH
    then moles of NaOH =moles of HC2H3O2 since 1-1 ratio from equation that makes .005052 moles of HC2H3O2 correct?
    then M acetic acid=.005052 moles/.01688L which =2.9*10^-1 is that correct?

    and for part 3 is it mols of acetic acid=.01688L*.5052M and then I'm kinda lost

  3. DrBob222

    Pay attention.
    You must have used 0.010 for L NaOH but the problem says volume NaOH is 16.88 mL.

  4. Mo

    Assume that your vinegar contained a small amount of citric acid (a triprotic acid).
    Using the same experimental data, would you expect the molarity of this sample to be
    the same as or different than a sample which contained only pure acetic acid?

  5. Anonymous


  6. Chemistry

    What is the weight per volume percent (i.e. % density) of 0.5522 g acetic acid in the 10.00 mL sample?

  7. Chaw

    Lashio Education College
    Chemistry Department

  8. Little girl

    5: a
    6: b
    11: d
    13: d
    15 b
    The rest you will have to do it yourself!

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