Question

How would you prepare a buffer with pH 7.4 using species from the ionizations of carbonic acid? The Ka values are 4.3 x 10 and 5.6 x 101 Would this bufer be more effective against added acid or added base? Explain.
0 0
Add a comment Improve this question Transcribed image text
Know the answer?
Add Answer to:
How would you prepare a buffer with pH 7.4 using species from the ionizations of carbonic...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Describe how would you prepare 500.0 mL of buffer with pH = 9.08 and [HA] +...

    Describe how would you prepare 500.0 mL of buffer with pH = 9.08 and [HA] + [A−] = 0.10 M using the following reagents available to you in the stock room and any appropriate glassware. Available: NH4Cl (F.W. = 53.5)   Ka = 5.5×10−10 pKa = 9.26 6.00M HC2H3O2       Ka = 1.8×10−5    pKa = 4.74 NaH2PO4•H2O (F.W. = 137.99)       Ka = 7.4×10−8    pKa = 7.13 3.00M NaOH             Deionized H2O 1) Pick the correct weak acid. 2) Solve the Henderson-Hasselbalch equation for...

  • What is the pH after 0.28 moles of HCl is added to a buffer containing 1.00...

    What is the pH after 0.28 moles of HCl is added to a buffer containing 1.00 moles of HOBr and 1.00 moles NaOBr ? Ka HOBr = 2.5 x 10-9 What is the pH of a 1.14M solution of carbonic acid? Ka1 = 4.3 x 10-7  Ka2 = 5.6 x 10-11

  • Consider how to prepare a buffer solution with pH = 3.40 (using one of the weak...

    Consider how to prepare a buffer solution with pH = 3.40 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.443-M solution of weak acid with 0.365 M potassium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the potassium hydroxide solution would have to be added to the acid solution of your...

  • c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml...

    c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml of this buffer. For full creds, show your work in detail. (4) aj Calculate the pH if 9.5 mL of 10.0 M NaOH (ag) is added to 200.0 mL ofa freshly prepared solution of this buffer. For full credit, show your work in detail (4) e) You should see from the calculations that this buffer is better able to buffer against added acid than...

  • Prepare a buffer by acid-base reactions. Consider how to prepare a buffer solution with pH =...

    Prepare a buffer by acid-base reactions. Consider how to prepare a buffer solution with pH = 7.35 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.362-M solution of weak acid with 0.325 M potassium hydroxide. pk Weak Acid HNO2 HCIO HCN Conjugate Base NO2 CIO CN K 4.5 x 10-4 3.5 x 10-8 4.0 x 10-10 3.35 7.46 9.40 How many L of the potassium hydroxide solution would have to be added...

  • 1. How would you prepare a liter of "carbonate buffer" at a pH of 10.07? You...

    1. How would you prepare a liter of "carbonate buffer" at a pH of 10.07? You are provided with carbonic acid (H2CO3), sodium hydrogen carbonate (NaHCO3), and sodium carbonate (Na2CO3). Please give an explanation. 2. Provide the mole ratio to support your answer. (Give your answer in the form base : acid.)

  • 8. Human blood contains two buffer systems, one based on phosphate species and one on carbonate...

    8. Human blood contains two buffer systems, one based on phosphate species and one on carbonate species. At the temperature of human blood, the K, values for phosphoric acid are 1.3x10,2.3x10 and 6x10-12, respectively. The Ka values for carbonic acid are 8x10-7 and 1.6x10-10 a. If blood has a normal pH of 7.4, draw the principle phosphate and carbonate species present? b. What is the ratio between the two phosphate species?

  • (17.2.c.7) Consider how to prepare a buffer solution with pH = 7.53 (using one of the weak acid/conjugate base systems s...

    (17.2.c.7) Consider how to prepare a buffer solution with pH = 7.53 (using one of the weak acid/conjugate base systems shown here) by combining1.00 L of a 0.357-M solution of weak acid with 0.300 M sodium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the sodium hydroxide solution would have to be added to the acid solution of your...

  • You must prepare a solution to use as an environment that involves a particular strain of...

    You must prepare a solution to use as an environment that involves a particular strain of bacteria that has a very limited pH range in which it can survive. This bacteria needs a medium with a pH = 6.10. You are tasked with making 500 mL buffer for this bacterium given the following reagents available to you in the lab, these are in the table b. State which reagent(s) and exactly how much you used of each to create the...

  • Consider how best to prepare one liter of a buffer solution with pH = 3.36 using...

    Consider how best to prepare one liter of a buffer solution with pH = 3.36 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of...

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
ADVERTISEMENT