chemistry

posted by .

the following titration data were collected: a 10 mL portion of a unknown monoprotic acid solution was titrated with 1.12340 M NaOH and required 23.95 mL of the base solution for neutralization.


calculate the molarity of the acid solution
calculate the molarity of the acid soluton were it the cas that the acid was diprotic

  • chemistry -

    monoprotic:
    HA + OH^- ==> H2O + A^-
    moles NaOH = M x L = ?
    moles HA = same since 1 mole HA = 1 mol OH^-.
    M HA = moles/L = ?moles/0.01L = ?

    diprotic:
    H2A + 2OH^- ==> 2H2O + A^2-
    moles NaOH = M x L = ?
    moles H2A = 1/2 moles NaOH (since 1 mole H2A = 2 moles NaOH

    M H2A = moles/L = (1/2 ?)/0.01 L = xx

  • chemistry -

    M = 2.691

    if diprotic, =134.6

    Is this correct?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. College Chemistry

    1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample …
  2. 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) = 0.200 …
  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?
  4. Chemistry

    Suppose 50.0 mL of an aqueous solution containing an unknown monoprotic weak acid is titrated with 0.250 M KOH. The titration requires 31.52 mL of the potassium hydroxide solution to reach the equivalence point. What is the concentration …
  5. Chemistry, pH, Buffers

    Please help!! Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show me how do I calculate …
  6. College Chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original …
  7. chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original …
  8. chemistry

    You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original …
  9. chemistry

    A 125.0 mg sample of an unknown, monoprotic acid was dissolved in 100.0 mL of distilled water and titrated with a 0.050 M solution of NaOH. The pH of the solution was monitored throughout the titration, and the following data were …
  10. Chemistry

    15.00mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30mL of the base. What was the normality of the acid solution?

More Similar Questions