Question

How does pH control the forms of carbonic acid, bicarbonate, and carbonate in water and the...

How does pH control the forms of carbonic acid, bicarbonate, and carbonate in water and the chemical conditions when they are equal?

Homework Answers

Answer #1

The pKa1 value for carbonic acid is 6.35. The variatio of carbonic acid, bicarbonate and carbonate with pH is as given below.

When pH<<<pKa1, then [H2CO3] approximately equal to1.

When pH=pKa1, then H2CO3 and HCO3- co exist.

When 7<pH<10, HCO3- is present.

When pH>10 CO3- is present.

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
Give a recipe for preparing a carbonate/bicarbonate buffer solution having a pH of 7.5. For carbonic...
Give a recipe for preparing a carbonate/bicarbonate buffer solution having a pH of 7.5. For carbonic acid,  H2CO3,  pKa1 = 6.37 and pKa2 = 10.25.
1. What are the two pKa values for carbonic acid? What is the pH of a...
1. What are the two pKa values for carbonic acid? What is the pH of a 0.100M solution of sodium bicarbonate? What is the pH of a 0.100M solution of sodium carbonate?
How does the carbonic acid/bicarbonate buffer system respond to a. excersise casuing b. lung impairment causing...
How does the carbonic acid/bicarbonate buffer system respond to a. excersise casuing b. lung impairment causing acidosis c. loss of bicarbonate due to diahrrea
Carbonic acid, H2CO3, is a weak diprotic acid with pKa values of 4.0 and 10.0. Its...
Carbonic acid, H2CO3, is a weak diprotic acid with pKa values of 4.0 and 10.0. Its conjugate base forms are bicarbonate and carbonate. Use this information to answer the questions. d) What is the pH of a buffer made by mixing 100 mL of 0.1 M NaHCO3 and 10 mL of 0.1 M Na2CO3? Answer= pH=9 What is the minimum volume of 1.0 M HCl that you would need to add to 100 mL of the solution in Part (d)...
Assume that the normal blood buffer contains 0.00080 M carbonic acid and 0.0085 M hydrogen carbonate;...
Assume that the normal blood buffer contains 0.00080 M carbonic acid and 0.0085 M hydrogen carbonate; the pKa = 6.35 for carbonic acid and the volume of blood in the body is 7.00 L. The blood pH, due to disruption, is now 7.20. What is the ratio of [HCO3 − ]/[H2CO3] now that the blood has been challenged? How many moles of hydrogen carbonate must be added to the blood to bring the carbonic acid/hydrogen carbonate ratio back to a...
Explain why the bicarbonate/carbonic acid buffer system works well in blood in spite of the fact...
Explain why the bicarbonate/carbonic acid buffer system works well in blood in spite of the fact that the blood pH is at the very edge of the effective buffer range of that base/acid pair. How would hyperventilation raise the blood pH? How would hypoventilation (or respiratory failure) lower the blood pH?
how can you explain how the carbonic acid-bicarbonate buffer system of the blood operates in 2...
how can you explain how the carbonic acid-bicarbonate buffer system of the blood operates in 2 sentences?
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...
What is the alkalinity, in terms of calcium carbonate, of a water with 80 mg/L bicarbonate...
What is the alkalinity, in terms of calcium carbonate, of a water with 80 mg/L bicarbonate and 5 mg/L of carbonate at a pH of 9?
Blood contains a buffer of carbonic acid (H2CO3) and hydrogen carbonate ion (HCO3-) that keeps the...
Blood contains a buffer of carbonic acid (H2CO3) and hydrogen carbonate ion (HCO3-) that keeps the pH at a relatively stable 7.40. What is the ratio of [HCO3-] / [H2CO3] in blood? Ka1 = 4.30x10-7 for H2CO3.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT