Chemistry

1.0L of aqueous solution in which [H2CO3]=[HCO3^-]=0.10M and has [H^+]=4.2E-7. What is the concentration of [H^+] ofter 0.005 mole of NaOH has been added?

H2CO3 ==> H^+ + HCO3^-

k1 = (H^+)(HCO3^-)/(H2CO3)
I don't know if you are supposed to calculate or to look up k1. However, you can calculate it as follows.
Since (HCO3^-) = (H2CO3) [both are 0.1 M), then plugging in 0.l M for each gives k1 = (H^+).
If we start with 0.1 mol H2CO3 and add 0.005 mol NaOH, we have 0.1 - 0.005 mols H2CO3 remaining and an extra 0.005 mol HCO3^- formed to make the final (HCO3^-)= 0.1 + 0.005 = ??
Plug k1, H2CO3, and HCO3^- into the k1 expression above and solve for (H^+). I found 3.97 x 10^-7. Post your work if you have trouble. By the way, it is a longwe way but you can also use the Henderson-Hasselbalch equation. Note also that this is a buffer solution and the H^+ didn't change much even though an amount of NaOH equivalent to 5% was added. That's what it is supposed to do. 0.005 mol NaOH added to an unbuffered solution would change the H^+ to 2 x 10^-12.

asked by Vic

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Complete the following equilibrium reactions that are pertinent to an aqueous solution of Ag2CO3. Physical states, s, l, g, and aq, are optional. So far I worked it out to be: Ag2CO3(s) <--> 2Ag^+ + CO3^(2-) H2CO3(aq) +
  2. chemistry

    When a base is introduced into this buffer, which of H2CO3 and HCO3− reacts with the base to maintain the pH of the solution? HCO3− H2CO3
  3. Chemistry

    Complete the charge balance equation for an aqueous solution of H2CO3 that ionizes to HCO3^- and CO3^2- ______ = ______ + _______ + _______ Given choices: [HCO3^-],[CO3^2-], [OH^-], 2[H^+], [H2CO3], 2[CO3^2-], 3[H^+], {H^+] I
  4. chemistry

    It's hydrogen carbonate, which is HCO3- Should the reactant be H2CO3? How do you balance this reaction?: HCO3 ---> H2O + CO2
  5. Chemistry

    4) Which of the following is the most effective buffer system for a pH value of 4.45? a. H2CO3/HCO3- (K1 = 4.4 * 10-7) b. HCO3-/CO32- (K2 = 4.7 * 10-11) c. H2S/HS- (K1 = 1.0 * 10-7) d. HC2O4-/C2O42- (K2 = 5.0 * 10-5) e.
  6. science( chem)

    The total Carbon dioxide content (HCO3- + CO2) in a blood sample is determined by acidifiying the sample and measuring the volume of CO2 evolved with a van slyke manometric apparatuses. The total concent was determined to be 28.5
  7. chemistry

    If 0.1200g of sodium carbonate is dissolved in 50 mL of water and titrated with 0.1000 M HCl, how many mL of HCl will be required to reach the second endpoint? CO3^-2 + H^+1 --> HCO3^-1 HCO3^-1,+ H^+1 --> H2CO3
  8. Chemistry

    1. An aqueous solution contains 0.154 M ascorbic acid (H2C6H6O6) and 0.196 M hydrobromic acid. Calculate the ascorbate (C6H6O62-) ion concentration in this solution. Can you explain how to do this please? thank you. Also if you
  9. chemistry

    In titration of a 0.10M soln of Na2Co3 with HCL which of the following will be present in the largest concentration at the first equivalence point? a. Co3^2- b. HCO3- c. H+ d. H2CO3 e. OH-
  10. Chemistry

    Calculate [CO32- ] in a 0.019 M solution of CO2 in water (H2CO3). If all the CO32- in this solution comes from the reaction shown below, what percentage of the H+ ions in the solution is a result of the dissociation of

More Similar Questions