Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present?

(A) 1.60 M
(B) 0.800 M
(C) 0.600 M
(D) 0.450 M
(E) 0.200 M

I know the answer is B, but how do you get this? These types of problems completely lose me. Is a rice table necessary?

Vinegar is acetic acid, which I will write as CH3COOH. It's the right end H that reacts with the NaOH.

SO, mols NaOH = L x M = 0.0267 L x 0.600 M = ?? mols NaOH.
The whole idea of titration is that the mols of the titrant will tell us the amount of the unknown material in the sample.
So we have ?? mols NaOH.
You can see we replaced the 1 H on CH3COOH with OH of the NaOH, so we have 1 mol CH3COOH per 1 mol NaOH. That means we must ALSO have ?? mols CH3COOH.
Since mols = M x L, you know mols CH3COOH, you know L CH3COOH from the problem, solve for M, the molarity.
It can't get much simpler than that; you may be making it too hard. # mols = M x L is all you need to know.

Okay. I got it now. Thank you so much! :)

asked by Sarah
  1. 0.800 M

    posted by kelsey

Respond to this Question

First Name

Your Response

Similar Questions

  1. chem-acid-base titrations

    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
  2. chem.

    A 10.0 mL of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with .5062M NaOH, and 16.58mL is required to reach the equivalence point. A. What is the molarity of the acetic acid? B. If the density of the vinegar
  3. chemistry

    10 ml sample of vinegar an aqueous solution 0f acetic acid( HC2H3O2) is titrated with 0.5062 M and 16.58 ml is required to reach equivalence point what is the molarity of the acetic acid b. if the density of vinegar is 1.006 g/cm3
  4. Chemistry

    In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the
  5. Chemistry

    a 30 mL sample of vinegar is titrated with .1098 M NaOH. it takes 43.28 mL naOH solution to reach the endpoint. Determine the acetic acid concentration in the vinegar solution?
  6. Chemistry

    1. Commercial vinegar is a solution of acetic acid in water. How would you determine which brand of vinegar contains more acetic acid in a given volume of vinegar?
  7. Chemistry

    Acetic acid, HC2H3O2, is the sour constituent of vinegar (acetum is Latin for "vinegar" ). In an experiment, 3.76 g of acetic acid was burned. HC2H3O2(l) + 2 O2(g) 2 CO2(g) + 2 H2O(l) If 54.6 kJ of heat evolved, what is ÄH per
  8. Chemistry

    A sample of 25.00 mL of vinegar is titrated with a standard 1.02 M NaOH solution. It was found that a volume of 19.60 mL of the standard NaOH solution is used to completely neutralize the acetic acid in the solution. Calculate the
  9. chemistry

    A 12.6 mL sample of vinegar, containing acetic acid, was titrated using 0.542 M NaOH solution. The titration required 24.1 mL of the base. what is the molar concentration of acid in the vinegar?'
  10. Chemistry

    A 5.00 mL aliquot of vinegar (acetic acid, FW = 63 g/mol) was diluted and titrated with 0.1104 M NaOH requiring 32.88 mL. If the vinegar has a density of 1.055 g/mL, calculate its acidity as % acetic acid

More Similar Questions