Question

You have been supplied with 2M solution of carbonic acid (H2CO3) and a 6M solution of...

You have been supplied with 2M solution of carbonic acid (H2CO3) and a 6M solution of NaOH. What volumes, of these materials are required to prepare 1 L of a 50 mM buffer solution at pH 7 (pKa for carbonic acid is 6.35)

Homework Answers

Answer #1

The volume of H2CO3 solution necessary to prepare said buffer concentration is calculated:

V1 = C2 * V2 / C1 = 0.05 M * 1000 mL / 2 M = 25 mL

The molar ratio of acid and salt is calculated, by means of the equation of henderson hasselbach cleared:

1) n Salt / n Acid = 10 ^ (pH - pKa) = 10 ^ (7 - 6.35) = 4.47

You have:

2) n Salt + n Acid = M * V = 0.05 M * 1 L = 0.05 mol

System of equations between 1 and 2 is applied:

n Salt = 0.041 mol

n Acid = 0.009 mol

The volume of NaOH necessary to produce said amount of salt from the initial acid is calculated:

V NaOH = n Salt * 1000 / M = 0.041 * 1000/6 = 6.83 mL

They are required:

V acid = 25 mL

V NaOH = 6.83 mL

V Water = 68.17 mL

If you liked the answer, please rate it in a positive way, you would help me a lot, 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
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...
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)...
Given that carbonic acid, H2CO3, has a pKa1 = 6.37 and a pKa2 = 10.33, answer...
Given that carbonic acid, H2CO3, has a pKa1 = 6.37 and a pKa2 = 10.33, answer the following. (a) If you wanted to make a pH 7 buffer solution starting with NaHCO3(aq), would you add 0.10 M HCl or 0.10 M NaOH? answer: 0.10 M HCl (b) If you began with 6.5 mL of 0.45 M NaHCO3, how many mL of your choice from (a) would you need to add to get a pH 7 buffer? mL
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.
Consider a the titration of 0.629 L of 0.879 M carbonic acid (H2CO3) with 1.61 M...
Consider a the titration of 0.629 L of 0.879 M carbonic acid (H2CO3) with 1.61 M NaOH. What is the pH at the second equivalence point of the titration?
Consider a the titration of 0.907 L of 0.909 M carbonic acid (H2CO3) with 1.63 M...
Consider a the titration of 0.907 L of 0.909 M carbonic acid (H2CO3) with 1.63 M NaOH. What is the pH at the second equivalence point of the titration?
A solution is made by combining 50 mL 1.0 M carbonic acid, 2.0 mL 5.0 M...
A solution is made by combining 50 mL 1.0 M carbonic acid, 2.0 mL 5.0 M KOH and 448 mL pure water (assume the total volume is 500 mL). The pKa of carbonic acid is 6.35. Calculate the pH of the resulting solution.
The next three (3) problems deal with the titration of 371 mL of 0.501 M carbonic...
The next three (3) problems deal with the titration of 371 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.9 M NaOH. 1)What is the pH of the solution at the 2nd equivalence point? 2)What will the pH of the solution be when 0.1282 L of 1.9 M NaOH are added to the 371 mL of 0.501 M carbonic acid? 3) How many mL of the 1.9 M NaOH are...
Describe how much of a 5M solution of NaOH you would need to prepare approximately 1...
Describe how much of a 5M solution of NaOH you would need to prepare approximately 1 L of sodium actetate buffer, pH= 4.8, from 1 L of acetic acid (10 mM). Acetic acid pKa is 4.8.