Question

Calculate the pH and concentrations of the following species in a 0.025M carbonic acid solution. (Given...

Calculate the pH and concentrations of the following species in a 0.025M carbonic acid solution. (Given Ka1=4.3x10^-7 and Ka2=5.6x10^-11

a) H2CO3 b)HCO3- c)CO32- d)H+ e)OH-

Homework Answers

Answer #1

Answer: Here the first thing is to be noted that the concentration of H+ ion is second dissociation is neglected as it is a very low value , Means H+ concentration is majorly depends upon the first dissociation

  H2CO3 ↔ H+ + HCO3-

here , [H+] = [HCO3-]

Ka1 = 4.3 * 10-7 = [H+] 2 / [H2CO3] = [H+] 2 / 0.025

[H+]2  = 1.075 * 10-8

H+ = 1.0368 * 10-4 M

Hence the concentration of [H+] = [HCO3-] = 1.0368 * 10-4 M

And Ph = - log [ 1.0368 * 10-4 ]   

Ph = 3.98

Hence POH = 14-3.98 = 10.02

[OH-] = 9.5499 * 10-11 M

Hence , It is all about the given question . Thank you :)

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the percent ionization of carbonic in 0.1441 M carbonic acid solution, H2CO3? H2CO3(aq) +...
What is the percent ionization of carbonic in 0.1441 M carbonic acid solution, H2CO3? H2CO3(aq) + H2O(l) « HCO3−(aq) + H3O+(aq) Ka1 = 4.3000e-7 HCO3−(aq) + H2O(l) « CO32−(aq) + H3O+(aq) Ka2 = 5.6000e-11
Rainwater is acidic because CO2(g) dissolves in the water, creating carbonic acid, H2CO3 (Ka1=4.3×10−7,Ka2=5.6×10−11). If the...
Rainwater is acidic because CO2(g) dissolves in the water, creating carbonic acid, H2CO3 (Ka1=4.3×10−7,Ka2=5.6×10−11). If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Part A Calculate the concentrations of carbonic acid, bicarbonate ion (HCO3−) and carbonate ion (CO32−) that are in a raindrop that has a pH of 5.80, assuming that the sum of all three species in the raindrop is 1.0×10−5M. Express your answers using two significant...
Consider the determination of the concentration of CO32- in a solution of H2CO3. (Ka1=4.3x10-7, Ka2=5.6x10-11) What...
Consider the determination of the concentration of CO32- in a solution of H2CO3. (Ka1=4.3x10-7, Ka2=5.6x10-11) What appropriate approximation(s) can be made in the second step of determining this concentration?
1. What is the pH of a 1.05M solution of carbonic acid? Ka1 = 4.3 x...
1. What is the pH of a 1.05M solution of carbonic acid? Ka1 = 4.3 x 10-7 Ka2 = 5.6 x 10-11 2. A diprotic acid, H2A has the following Kas: Ka1 = 3.94 x 10-7 and Ka2 = 8.78 x 10-11. What is the Kb of HA-? 3.A diprotic acid, H2A has the following Kas: Ka1 = 3.94 x 10-7 and Ka2 = 8.78 x 10-11. What is the Kb of HA-?
Calculate the concentrations of all species in a 1.12 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 1.12 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4� 10�2 and Ka2 = 6.3� 10�8. NA+ = SO32- = HSO3- = H2SO3 = OH- = H+ =
Calculate the concentrations of all species in a 0.470 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 0.470 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. NA+ SO32- HSO3- H2SO3 OH- H+
The pH of blood serum is maintained by a proper balance of H2CO3 and NaHCO3 concentrations....
The pH of blood serum is maintained by a proper balance of H2CO3 and NaHCO3 concentrations. Calculate the volume of 5M NaHCO3 solution that should be mixed with a 10 mL of sample of blood which is 2M in H2CO3 in order to maintain a pH of 7.4 . Given Ka1 and Ka2 for H2CO3 in blood are 4.3 x 10-7 and 5.6 x 10-11 .
The interaction between carbon dioxide and water results in formation of carbonic acid, H2CO3, which lowers...
The interaction between carbon dioxide and water results in formation of carbonic acid, H2CO3, which lowers the pH of water through the reactions H2CO3(aq)+H2O(l) <---> HCO3-(aq) + H3O+(aq) Ka1= 4.3*10^-7 HCO3-(aq) +H2O(l) <---> CO3 2- (aq) + H3O+ (aq) Ka2=5.6*10^-11 This dissocociation causes "normal" rainwater to have a pH of approximately 5.7. However, H3O+(aq) can also come from other sources, particularly from acids resulting from interactions of water with industrial pollutants. Scientists studying a particular lake found that its pH...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.210 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.210 M oxalic acid solution (Ka1 = 6.5 × 10−2, Ka2 = 6.1 × 10−5). Be sure to report your answers to the correct number of significant figures.
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.370 M oxalic acid...
Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ species in a 0.370 M oxalic acid solution (Ka1 = 6.5 ×10−2, Ka2 = 6.1 ×10−5). Be sure to report your answers to the correct number of significant figures.