Chemistry

posted by .

Calculate the KA of formic acid if 2.3 g of it is dissolved in 1 litre of water to give [H+] of 0.003 M.

  • Chemistry -

    mols HCOOH = grams/molar mass, then
    M = mols/L soln. I get about 0.05M but you should confirm that.
    .........HCOOH + H2O ==> H3O^+ + HCOO^-
    I .......0.05..............0.......0
    C.......-0.003.........0.003..0.003
    E...0.05-0.003.........0.003...0.003

    Substitute from the ICE chart above into the IKa expression and solve for Ka.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem

    81. Formic acid HCHO2, is a convenient source of small quantities of carbon monoxide. When warmed with sulfuric acid, formic acid decomposes to give CO gas. HCHO2(l) -> H2O(l) + CO(g) If 3.85 L of carbon monoxide was collected over …
  2. Chemistry help needed

    How do I prepare 90% formic acid from conc. formic acid (98%-100% of density 1.22g/ml)?
  3. Chemistry

    calculate the pH at 0ml at the quivalence point and at 40ml in a titration of 25 ml of .120M formic acid with .105M NaOH (kA of formic acid= 1.8x10^-4)
  4. Chemistry

    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)
  5. 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 …
  6. Chemistry

    A buffer is prepared by mixing 0.30 mole of formic acid (HCNO2) and 0.20 mole of sodium formate (NaCHO2) in enough water to make 0.50 liter of solution. Ka of formic acid is 1.7 x 10-4. Calculate the pH of the resulting buffer solution.
  7. Chemistry

    20.0 ml of 1.00 M formic acid are combined with 10.0 ml of 1.00 M sodium formate. Calculate the expected pH. Ka for formic acid is 1.77 x 10^-4
  8. chemistry

    Describe the laboratory preparation of z1Litre of 1.3M formic acid buffer of pH 3.9 from solid sodium formats (molecular weight =68) and formic acid liquid 30% pure (Density of formic acid = 1.029g/ml, pKa = 3.75)
  9. Chemistry

    Explain the laboratory preparation of one Litre of 1.3M formic acid buffer of pH 3.9 from solid sodium formate (molecular weight =68) and formic acid liquid 30% pure (Density of formic acid = 1.029g/ml, pKa = 3.75)
  10. chemistry

    Given a PH of buffer solution is 4.23 made from 0.35 formic acid. Calculate the concentration of formate.The constant dissociation for formic acid is 3.75

More Similar Questions