Post a New Question

A.P. Chemistry

posted by .

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?

How does the henderson hasslebache equation help find the volume?

  • A.P. Chemistry -

    pH = pKa + log [(base)/(acid)]
    You know Ka. Calculate pKa.
    NO2^- is the base.
    HNO2 is the acid.

    First, plug in pH = 3.00, the pH of the solution you want, and calculate the (base)/(acid) ratio.
    That gives you (base) = factor x (acid).

    Then you know mLbase*Mbase = mLacid*Macid AND you know mLacid + mL bse = 1000.

    You solve for mLacid and mL base. If I didn't goof, it is something like 700 mL acid and 300 mL base.

  • A.P. Chemistry -

    Those volumes I quoted are not the exact volumes but they are close to the correct values.

Answer This Question

First Name
School Subject
Your Answer

Related Questions

More Related Questions

Post a New Question