HomeworkLib
Question

In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-,...

In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-, CO32-) are determined by concentration of the strong acid deposited by acid rain, as well as the concentration of H2CO3 which is controlled by the solubility of carbon dioxide . Under these conditions (constant H2CO3 and relatively low pH) the only carbonic acid equilbrium of importance is the conjugate base reaction of HCO3-, which is related to, but not identical to - and not the reverse of, Equation 1 in Table 10-3. If the concentration of H2CO3 is 1.3 x 10-5 M and the pH =6.27 what is the concentration of the bicarbonate ion, HCO3-?

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-,...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2–...

    Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2– , H3O + , and OH– ) in a 0.0037 M M carbonic acid solution. Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11

  • You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic...

    You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...

  • One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate...

    One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate ion (HCO3- ) system that maintains the pH of blood plasma to a relatively constant value. In blood at 37°C, the Ka of carbonic acid is 8x10-8. Suppose that the concentrations of the buffer components in the blood plasma are: [HCO3-] = 0.24 M and [H2CO3] = .12 M. Calculate the pH of blood.

  • Carbonic acid H2CO3 is a weak acid that fully dissociates in two steps in the presence of increased concentration o...

    Carbonic acid H2CO3 is a weak acid that fully dissociates in two steps in the presence of increased concentration of base. Step 1: H2CO3 =HCO3+H* Step 2: HCO3 =20,2- + H+ What is the composition of species in solution at pH = 10.25 when the halfway point to the first equivalence point has been reached? 50 % H2CO3 and 50 % CO2- 50 % CO2- and 50 % HCO3 50 % H2CO3 and 50 % HCO3 100 % H2CO3

  • a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid...

    a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.

  • 11. which of the following pairs of species is a conjugate acid-base pair? a. NaF, F b. NHs, NH c. H30+, ОН- d. H2CO3,...

    11. which of the following pairs of species is a conjugate acid-base pair? a. NaF, F b. NHs, NH c. H30+, ОН- d. H2CO3, CO32 8. which of the following salts is most likely to form an aqueous solution having the pH <7? a. NaBr b. LiNO3 c. NH4CI d. RbCN 2. which of the following pairs of species is not a conjugate acid-base pair? a. OH, H b. HOCI, OCh c. HSO4,SO42 d. H2CO3, HCO3 11. which of the...

  • Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H2CO3(aq) solution. What...

    Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H2CO3(aq) solution. What is the percent ionization of the acid and resulting pH? [H2CO3] =    [HCO3-] =    [CO32-] =    [H3O+] =    % ionization =    pH =    Acid Acetic Ammonium Formula CH:COOH NH4+ H2BO: Boric Carbonic H2CO3 HC1O2 HCOOH Chlorous Formic Hydrocyanic Perchloric 1.8 x 105 5.6 x 10-10 5.4 x 10-10 4.5 x 10-7 4.7 x 10-11 1.1 x 10-2 1.8 x 10-4 5.2 x 10-10 Very...

  • 21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a...

    21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...

  • Carbonic acid present in the blood comes mainly from dissolved carbon dioxide (CO2). Dissolved carbon dioxide,...

    Carbonic acid present in the blood comes mainly from dissolved carbon dioxide (CO2). Dissolved carbon dioxide, CO2(aq), reacts with water to produce H2CO3. a) Write the equilibrium expression for this process. b) The equilibrium constant for this reaction is the hydration constant for CO2, Kh = [H2CO3]/[CO2(aq)] = 3.0 x 10−3 . Combine this equation with the expression you derived in 1.a) for the equilibrium expressions for the first ionization (controlled by Ka1) and rearrange to obtain the apparent equilibrium...

  • HELP PLEASE 5 – Calculate the concentrations of H+, HCO3- and CO32- in a 0.025 M...

    HELP PLEASE 5 – Calculate the concentrations of H+, HCO3- and CO32- in a 0.025 M H2CO3 solution. 6 – Classify the following as a Lewis acid, Lewis base, both or neither:CO2, H2O, I-, SO2, NH3, OH-, H+, BCl37 – 7-Calculate the pH of a solution that is 0.20 M NH3 and 0.30 M NH4Cl.8 – 8-The pH of blood plasma is 7.40. Assuming the principal buffer system is HCO3-/H2CO3, calculate the ratio [HCO3-]/[H2CO3] . 9 – A 0.2688 g...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT