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Vinegar is a dilute solution of acetic acid. In the titration of 5.00 mL of vinegar, 39.75 mL of 0.137 M sodium hydroxide solution was required to neutralize the vinegar to a phenolphthalein end point. Calculate each of the following of the vinegar.

(a) the molarity : I got 1.09 and its correct so im thinking I have to use this for the next part which is

b) the percent by mass (density of solution = 1.007 g/mL)


  • Chemistry -

    You CAN use the answer from part A but it isn't necessary.
    moles NaOH = M x L
    moles vinegar = moles NaOH
    moles = grams vinegar/molar mass vinegar and solve for grams.
    Then % acetic acid = (mass acetic acid/mass sample)*100 = ??
    You will need to use the density information to convert 5 mL to grams to use for mass of the sample. Vinegar is usually about 4-6% acetic acid.

  • Chemistry -


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