Post a New Question

Chemistry

posted by .

Suppose you have two solutions to titrate with NaOH: (a) 10 ml of.1M HCL (b) 10 ml of .1M CH3COOH
would you expect either of the solutions to require different volumes of NaOH in order to reach an end point? Explain

  • Chemistry -

    Do I need to first figure out the PH?
    I believe that a= 3
    and b=2.87
    therefore it will require more naoh to titrate the acetic acid.

    I am not sure i figured the ph of acetic acid correctly, or if i am on the correct path here...

  • Chemistry -

    No, you don't need to calculate pH. What is the concept of titrating an acid with a base; i.e., when does the indicator show you have reached the end point? The answer to that is that when moles of acid = moles base the indicator tells you to quit adding base. So how many moles are in the 10 mL of 0.1M HCl? That is 0.01 x 0.1 = 0.001 moles HCl.
    How many moles are in the 10 mL of 0.1M CH3COOH? That is 0.01 x 0.1 = 0.001. So the end point will be the same no matter which acid is used. What counts is how many moles of the acid you have.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Hello, I need help with calculations for lab. I prepared excess NaOH and HCL solutions (unknown conc., ~0.1M). Then I standardized my NaOH solution by titrating known amounts of KHP (Potassium hydrogen phthalate)with it in the presence …
  2. Honors Chemistry

    I don't exactly understand this question -- can someone maybe explain it to me please?
  3. Chemistry

    Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution?
  4. college chemistry

    You are given solutions of HCl and NaOH and must determine their concentrations. You use 38 mL of NaOH to titrate 100 mL of HCl and 23.2 mL of NaOH to titrate 50 mL of 0.0782 M H2SO4. Find the unknown concentrations.
  5. Chemistry Help Please!!

    We did an experiment and I don't really know how to calculate this question. If you could show me how to do one, then I could do the rest. INFORMATION: HCl = 0.1404 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask …
  6. Chemistry HELPP!!!!!!

    We did an experiment and I don't really know how to calculate this question. If you could show me how to do one, then I could do the rest. INFORMATION: HCl = 0.1404 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask …
  7. Chemistry 12

    15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is: a. 2 x 10-14 M b. 5 x 10-14 M c. 5 x 10-7 M d. 2 x 10-1 M 16. Aqueous solutions of strong acids and strong bases: a. are good electricity conductors b. …
  8. Chemistry Solubility help!!!!!!!!!

    INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 NaOH (12.1 mL of HCl needed to titrate) Flask C: 0.025 NaOH (10.8 …
  9. Chemistry - Solubility

    INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 M NaOH (7.5 mL of HCl needed to titrate) Flask C: 0.025 M NaOH (10.8 …
  10. Chemistry - Solubility

    INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: A 25 ml aliquot was used Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 M NaOH (7.5 mL of HCl needed to titrate) …

More Similar Questions

Post a New Question