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.

  1. 👍
  2. 👎
  3. 👁
  1. I estimated the pH and didn't come close to 11 or 12 but I may not have used the same Ka value you did. Most tables in text books don't agree. Post your work and I'll look at it.

    1. 👍
    2. 👎
  2. Actually, when I did the problem again, I got 8.08.

    Is this correct?

    1. 👍
    2. 👎
  3. Yes, 8. something is right (I think I obtained 8.11 and I used 4E-4 for Ka for HNO2.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    An impure sample of barium hydroxide of mass 1.6524 g was allowed to react with 100 cm3 of 0.200 mol dm-3hydrochloric acid. When the excess acid was titrated against sodium hydroxide, 10.9 cm3 of sodium hydroxide solution was

  2. A.P. Chemistry

    You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00  10-4). A buffer of pH 3.000 is needed. What volumes of HNO2 and KNO2 are required to make 1 liter of buffered solution?

  3. chem class

    A 25.00-mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is ???? M.

  4. chemistry

    A 35.0 ml sample of 0.225 M HBr was titrated with 42.3 ml of KOH. What is the concentration of the KOH?

  1. 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

  2. chemistry

    pls help. A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0,

  3. Chemistry

    What mass of solid aluminum hydroxide can be produced when 50.0mL of .200 M Al(NO3)3 is added to 200.0 mL of .100 M KOH

  4. Chemistry

    A 30.00mL sample of 0.150M KOH is titrated with 0.125M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30.0 mL, 35.0 mL, 36.0 mL, 37.0 mL, 40.0 mL

  1. Chemistry

    Calculate the molarity of the following solutions: 5.0g of KOH in 4.0L of KOH solution I went from grams of KOH to moles of KOH to molarity but still got the wrong answer... 5.0g KOH X 1 mol KOH/56.108g KOH = 5.0 mol

  2. Chemistry

    Exactly 100 mL of 0.14 M nitrous acid (HNO2) are titrated with a 0.14 M NaOH solution. Calculate the pH for the following. (a) the initial solution (b) the point at which 80 mL of the base has been added (c) the equivalence point

  3. Chemistry

    Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq). pKa1 = 1.3 and pKa2 = 6.7 a) before addition of any KOH b) after addition of 25.0 mL of KOH c) after addition

  4. Chemistry

    A 10.0 mL sample of hydrochloric acid solution with an unknown concentration is titrated with a 0.10 mol/L solution of potassium hydroxide. The results of the titration are shown in the table below: Trial Initial volume of KOH

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