chem

posted by .

calculate the pH during the titration of 100 mL of .200 M HCl with .400 M NaOH after 0,25, 50, and 75 mL NaOH have been added

  • chem -

    This is too long and too detailed to post; in general what you do is start with mols HCl, add x mols NaOH, subtract mols to see mols HCl unreacted, then M = mols/L (remember this is total volume which is mL HCl to start plus mL NaOH added). Then pH = -log(H^+)
    I can expand on individual questions if you get stuck one of them. Post your work.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    HCl is titrated with NaOH. When doing the titration, some of the NaOH splashed onto the inside surface of the Erlenmyer flask, and you forgot to rinse it into your sample. Would the systematic error be falsely high, low, or unaffected …
  2. chem

    HCl is a strong acid and ionizes 100%. NaOH is a strong base and ionizes 100%. We have no way of knowing the pH of HCl + H2O because the problem doesn't state the amount of HCl added or the concentration of HCl. For the NaOH + HCl …
  3. GChem

    1. 25mL of 0.1M HCl is titrated with 0.1M NaOH. What is the pH when 30mL of NaOH have been added?
  4. chem lab

    Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Indicate if the volume of NaOH is before or after the equivalence point. i don't know where to start.
  5. Chemistry

    Consider the titration of 50 mL of 0.250 M HCl with 0.1250 M NaOH. Calculate the pH of the resulting solution after the following volumes of Na OH have been added. a) 0.00 mL b) 50.00 mL c) 99.90 mL d) 100.00 mL e) 100.1 mL The question …
  6. chemistry

    11.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 of the following: 12.Before the titration. 13.After adding 24.9 mL of NaOH. 14.At the equivalence …
  7. 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 …
  8. Chem.

    How can I determine the concentration of HCl remaining in the flask after back titration?
  9. chemistry

    How can I determine the concentration of HCl remaining in the flask after back titration?
  10. 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 acid-base …

More Similar Questions