chem

posted by .

How many mL 0.1 M NaOH could you add to a buffer
formed from 0.1 moles NaHCOO and 0.1 moles HCOOH
without the pH going above 4.74?
Ka (formic acid = 1.8 x 10-4)

  • chem -

    0.1 mol = 100 millimoles.

    ........HCOOH + OH^- ==> HCOO^- + H2O
    I........100....0.........100
    add.............x..............
    C.....100-x....-x.........100+x
    4.74 = 3.74 + log (100+x)/(100-x)
    Solve for x = millimols OH to be added. I get approximately 82 millimols and
    M = millimols/mL, You know M and mmoles, solve for mL.
    Quite a large number when you think about it.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. CHEM

    Calculate the pH of solution made by combining 75.0 mL of 0.10 M formic acid with 30.0 mL of 0.25 M KOH. (Ka for formic acid, HCOOH, is 1.8 X 10^-4)
  2. college

    0.10 moles HCOOH (formic acid) and 0.02 moles HCOONa (sodium formate) are dissolved in a liter of water. what is the resulting pH solution?
  3. AP Chemistry

    A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with …
  4. Chemistry

    A 50.0 mL sample of 0.12 M formic acid, HCOOH, a weak monoprotic acid, is titrated with 0.12 M NaOH. Calculate the pH at the following points in the titration. Ka of HCOOH = 1.8 multiplied by 10-4. What is the pH when 50.0 mL NaOH …
  5. chem ll

    How many grams of formic acid, HCOOH, must be added to 0.270L of 0.180M sodium formate, HCOONa, to yield a buffer solution with a pH of 4.20?
  6. Chemistry

    You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 5.00 using only pure acetic acid, 3.00 M NaOH, and water. Calculate the quantities needed for each of the following steps in the buffer preparation. 1. Add acetic acid …
  7. bio chem

    Explain how to prepare 1L of a buffer at pH 7.4 using 1M hypochlorous acid (Ka = 3.5 x 10-8) and a 1 M NaOH solution. Indicate the volume of hypochlorous acid and sodium hydroxide to use. pH = pKa + log ([A-]/[HA]) Ka= [H+][A-]/[HA] …
  8. Chemistry

    Sodium methanoate, NaHCOO, and methanoic acid, HCOOH, can be used to make a buffer solution. Explain how this combination resists changes in pH when small amounts of acid or base are added. Buffers kind of confuse me and I'm not sure …
  9. Chemistry

    I was given a solution of HCOOH with hand approximate concentration of 0.20 moles and I need to titrate this with a 0.110 V mol of NaOH. If I add 20 milliliters of hcooh to the beaker before I titrate approximately what volume of NaOH …
  10. Chemistry

    Calculate the pH of a 1 L buffer solution that contains 0.050 moles of acetic acid and 0.040 moles of sodium acetate to which 0.020 moles of NaOH has been added.

More Similar Questions