Chemistry

posted by .

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine the pH after adding 5.0 mL of base beyond the equivalence point.

  • Chemistry -

    Determine where the equivalence point is. Note the volume.
    mmoles OH^- added in excess is 5.0 mL x M = ??
    total volume = mL to arrive at the equivalence point + 5.0 from the base
    mmoles/total mL = M of OH^-
    pOH = -log(OH^-)
    and pH + pOH = pKw = 14. Solve for pH.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chem

    Consider the titration of 20 mL of .105M Butric Acid HBut, with .125M sodium Hydroxide?
  2. chemistry

    Consider the titration of 21.0 mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. what is the initial pH?
  3. Chemistry

    A titration is performed by adding .600 M KOH to 40.0 mL of .800 M HCl. Calculate the pH before addition of any KOH. Calculate the pH after the addition of 5.0 mL of the base. Calculate the volume of base needed to reach the equivalence …
  4. Chemistry 2

    A titration is performed by adding 0.124 M KOH to 40 mL of 0.159 M HNO3. a) Calculate the pH before addition of any KOH. b) Calculate the pH after the addition of 10.26, 25.65 and 50.29 mL of the base.(Show your work in detail for …
  5. 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 …
  6. chemistry

    A 30 mL sample of .165 M propanoic acid is titrated with .300M KOH. Calculate the pH at each volume of added base: 0 mL, 5 mL, 10, equivalence point, one-half equivalence point, 20 mL, 25 mL. Use calculations to make a sketch of the …
  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. Chemistry

    A 40.0 mL sample of 0.100 M HNO2 is titrated with 0.200 M KOH. Calculate the pH at the equivalence point for the titration of HNO2 and KOH. I got pH= 11.74.
  9. chemistry

    Consider the titration of 40.0 mL 0.250 M ethylamine, C2H5NH2, with 0.350 M HCl. Determine each of the following and sketch the titration curve. Kb of ethylamine = 5.6x 10-4 a. The volume of added acid required to reach the equivalence …
  10. Chemistry

    Consider the titration of 20.00 mL of 0.1728 M Ascorbic acid (Ka = 7.9 x 10-5) with 0.4329 M NaOH. Match the following regions in the titration curve with the appropriate pH range. 1.Initial pH 2.Before equivalence point 3.At equivalence …

More Similar Questions