Question

1. What is the concentration of OAc- in a 0.1M Acetate buffer, pH 11? (pKa for...

1. What is the concentration of OAc- in a 0.1M Acetate buffer, pH 11?

(pKa for Acetic acid is 4.77)

2. As the pKa of an acid increases, the acid will be:

Converted to basic solution

Weaker

Stronger

Converted to neutral solution

0 0
Add a comment Improve this question Transcribed image text
Know the answer?
Add Answer to:
1. What is the concentration of OAc- in a 0.1M Acetate buffer, pH 11? (pKa for...
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
  • 1. What is the concentration of HOAc in a 0.1M Acetate buffer, pH 11.00? (pKa for...

    1. What is the concentration of HOAc in a 0.1M Acetate buffer, pH 11.00? (pKa for Acetic acid is 4.77). Please show full workings.

  • Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M...

    Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.

  • what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M...

    what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M buffer solution at pH 5.0? What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....

  • You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate....

    You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate

  • Do the calculations to make 200ml of 0.1M sodium acetate buffer with a pH of 5.1...

    Do the calculations to make 200ml of 0.1M sodium acetate buffer with a pH of 5.1 starting with 5.0M acetic acid and 1.0M NaOH ****show calculations***** 1.How much acetic acid is needed? 2.What is the ratio of Ac- to HAc at pH of 5.1? 3. What fraction of total acetate is Ac-at pH 5.1 4. How much OH- is needed to obtain 68.7% Ac-?

  • What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10...

    What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10 M buffer solution at pH 4.6pH 4.6? Note that the concentration, pH value, or both may differ from that in the first question. Strategy Rearrange the Henderson–Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A−]/[HA][A−]/[HA] . Use the mole fraction of acetate to calculate the concentration of acetate. Calculate the concentration of acetic acid. Step 1: The ratio...

  • What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...

    What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...

  • A. Calculate the pH of a solution that has a concentration of H+ of 8.9 x...

    A. Calculate the pH of a solution that has a concentration of H+ of 8.9 x 10-5 M and indicate whether the solution is acidic, basic, or neutral. B. An acetic acid buffer solution is required to have a pH of 5.27.  You have a solution that contains 0.010 moles of acetic acid.  How many moles of sodium acetate will you need to add to the solution?  The pKa of acetic acid is 4.74.  Show all calculations.

  • What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...

    What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...

  • What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...

    What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that m the first question. STRATEGY 1. Rearrange the Hendereon-Hasselbalch equation to solve for thfe rabo of base (acetate) to aad (acetic add).[A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration ot acetic acid.

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