I have done a acid & base titration lab, with 0.1M vinegar (with unknown %tage acid) and 0.1 NaOH...I think the result came out ok, in avg, 25.21mL of NaOH have titrated w/ 30.0mL unknown %tage acid of vinegar.

all I am given is Density of vinegar= 1.00g/mL and Percentage composition = [(mass solute)/ (mass solution)] x100...yet I still cannot understand how to join these two questions to get a clear answer.

please help... this lab is due tomorrow and i have to go away tonight for school varsity matters..

  1. 👍 0
  2. 👎 0
  3. 👁 403
  1. So what's the question? If you know the density of vinegar and its percent composition, why do you need to titrate it? And you need the molarity of the NaOH for the titration to mean anything? Perhaps its 0.1 M NaOH and you just omitted the M.

    1. 👍 0
    2. 👎 0
  2. yes, it is 0.1M NaOH,,, I am really stuck on this lab because I still cannot understand much of it..

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    If 3.15 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.40 qt sample of this vinegar?

  2. Chemistry

    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


    a) How will the concentration of NaOH be affected if during the titration some of the solid potassium hydrogen phthalate was spilled during the transfer? Will the concentration of the standardized NaOH increase, decrease, or have

  4. chemistry

    3.30 mL of vinegar needs 43.0 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.70 qt sample of this vinegar?

  1. Chemistry Titration Lab HELP!

    Hi everyone! I just got a new lab that I MUST complete today, and it's about titration- I have absolutely no clue how to do it, it just doesn't make sense to me! I hope that someone can help explain to me how to do it so I can


    i have a tritation lab due tomorrow and i am stumped on a couple things. its a titration lab using sodium hydroxide (NaOH)- 250 mL 0.300 M concentration, 10 mL of an unknown substance of vinegar, the avg. of titrated NaOH in the

  3. Chemistry

    The end point of the acid base/ titration between vinegar and NaOH occurred when: Question options: The acid and base neutralized each other. The phenolphthalein indicator turned faint pink. The moles of H+ were equal to the moles

  4. Chemistry

    40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid

  1. Chemistry

    Calculate amount (in grams) of unknown acid used for titration. You want 30 mL of titrant to get the equivalence point. Assume that the base is 0.05 M and the unknown acid molar mass is around 400 g/mol.

  2. Chemistry

    I wanted to calculate the average equivalent weight of an unknown acid for an acid-base titration experiment. The mass of the unknown that I had to obtain is 0.2 g and the equivalents of the acid is .001046 L x N. But is this

  3. chemistry

    If 3.30 mL of vinegar needs 42.5 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.50 qt sample of this vinegar?

  4. Chemistry

    An unknown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with NaOH. The appropriate reactions are as follows: Citric acid: H3C6H5O7 (aq) + 3NaOH (aq) -> 3H2O

You can view more similar questions or ask a new question.