Chemistry 12

Hi, I did the acid-base titration lab with HCl and 0.5M NaOH.

I need to calculate the moles of NaOH from molarity of NaOH and the average volume used.

My English isn't good but is it asking me to find the moles of NaOH using the molarity of NaOH and the average volume used correct?

This is my table.
Molarity of NaOH used: Trial 1
Initial volume of NaOH (mL): 27.10
Final volume of NaOH (mL): 38.90
Volume of NaOH used (mL): 11.80

Trial 2

Trial 3

My average volume of NaOH:

Then for some reason I am really confused even though I know it should be very simple... Please help me, thank you kindly.

  1. 👍
  2. 👎
  3. 👁
  1. The average volume is not right because you threw away one of the 11.8 volumes.
    Volumes are 11.80, 11.80 abd 14.10
    Sum those and divide by 3.

    Then mols NaOH = M NaOH x L NaOH = ?

    1. 👍
    2. 👎
  2. I thought we only add the first two because the first one was purposely overshot?

    0.5M NaOH × 12.56666667= 6.283333333
    =6.3 moles

    Thank you for replying!

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. organic chemistry

    1)Why benzoic acid is soluble in NaOH? 2)Why HCl is insoluble in titration of benzoic acid and NaOH? Benzoic is soluble in a solution of NaOH because the base forms the sodium salt with the acid to form sodium benzoate. The sodium

  2. Phenolphtalein vs Methyl Orange (check my reasonin

    Why can either phenolphthalein or methyl orange be used for an HCl-NaOH titration, but only phnolphthalein is suitable for an acetic acid-NaOH titration? Sol: for a while,I misunderstood the question and suggested that Phenol. has

  3. Chemistry

    1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding

  4. chemistry

    The following data were collected at the endpoint of a titration performed to find the molarity of an HCl solution: Volume of acid (HCl) used = 14.4 mL; Volume of base (NaOH) used = 22.4 mL; Molarity of standard base (NaOH) =

  1. Analytical chemistry

    A dilute perchloric acid solution was standardized by dissolving 0.2445 g of primary standard sodium carbonate in 50 mL of the acid, boiling to eliminate CO2, and back-titrating with 4.13mL of dilute NaOH. In a separate titration

  2. Chemistry

    1) You are given solutions of HCl and NaOH and must determine their concentrations. You use 37.0mL of NaOH to titrate 100mL of HCl and 13.6 mL of NaOH to titrate 50.0mL of 0.0782 M H2SO4. Find the unknown concentrations. Molarity

  3. 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

  4. Chemistry

    During an acid-base titration, 25 mL of NaOH 0.2 M were required to neutralize 20 mL of HCl. Calculate the pH of the solution for each: a) Before titration b) After adding 24.9 mL of NaOH c) At equivalence pt d) After adding 25. 1

  1. Chemistry

    I did a lab on vinegar and titration. The question asks.. In the titration of acetic acid and NaOH the use of the color indicator mandates that excess base be present to detect the reading endpoint. Will this cause the calculated

  2. Chemistry

    Hi, I posted yesterday with this lab question. "Calculate the molar amounts of NaOH used in the reaction with the HCl solution and with the HC2H3O2. I think I got the answer to that with the help that I received. I had 5 mL of

  3. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH

  4. chemistry

    PLEASE NOTE: Titration requires several steps in order to obtain exact results. The procedures described in this lab assume that you have already done the TITRATION TUTORIAL and are familiar with the technique. 1. Prepare the NaOH

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