HomeworkLib
Question

What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00  L of solu...

What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00  L of solution? The dissociation constant Ka of HA is 5.66*10^-7.

pH = __________
What is the \rm pH after 0.150 mol of \rm HCl is added to the buffer from Part A? Assume no volumechange on the addition of the acid.
pH = _____________
What is the \rm pH after 0.195 mol of \rm NaOH is added to the buffer from Part A? Assume novolume change on the addition of the base.
pH = ______________

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1
pH = pKa + log ([salt]/[acid])

pKa = -log(5.66*10^-7)
=7-log(5.66) = 6.247

[salt] = 0.305/2 = 0.152
[acid] = .506/2=.253

1. pH = 6.247 + log(.152/.253)
=6.247-0.221 =6.026

2.
if strong acid added it will nutrilize salt(conjugate base) and make HA
so new [HA] = 0.506+0.150/2 = 0.328
[NaA] = 0.305-0.150 /2 = 0.0775

so pH =
=6.247 - log(0.0775/0.328)
= 6.247-0.626
=5.621

3. stong base added it will make NaA from HA
so new
[HA] = 0.506-0.195 /2 = 0.155
[NaA] = 0.305+0.195/2=0.250

so pH = 6.247 + log (0.250/0.155)
=6.246+0.207 = 6.454

ANSWER
1 0
Add a comment
Know the answer?
Add Answer to:
What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00  L of solu...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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

  • Part A What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of so...

    Part A What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Express the pH numerically to three decimal places. pH = SubmitHintsMy AnswersGive UpReview Part Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid....

  • Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.406 mol of NaA in 2.00 Lof sol...

    Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.406 mol of NaA in 2.00 Lof solution? The dissociation constant Ka of HA is 5.66×10−7. Express the pH numerically to three decimal places. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal...

  • Part A: What is the pH of a buffer prepared by adding 0.708 mol of the...

    Part A: What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.406 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Part B:What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Part C: What is the pH after 0.195 mol of NaOH is added to the...

  • PART A: What is the pH of a buffer prepared by adding 0.809 mol of the...

    PART A: What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. PART B: What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. PART C:What is the pH after 0.195 mol of NaOH is added to the...

  • ± pH Changes in Buffers Part A What is the pH of a buffer prepared by...

    ± pH Changes in Buffers Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Express the pH numerically to three decimal places. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express...

  • Part A - 7 What is the pH of a buffer prepared by adding 0.809 mol...

    Part A - 7 What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K, of HA is 5.66 x 10 Express the pH numerically to three decimal places. View Available Hint(s) Ivo AED ? pH = Submit Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume...

  • II, 8 part A: What is the pH of a buffer prepared by adding 0. 809...

    II, 8 part A: What is the pH of a buffer prepared by adding 0. 809 mol of the veak acid HA to 0.607 mol of Na A in 2.00 LOT Solution? The dissociation constant of HA is 5.66 x 10? Dart B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. What is the pH after 0.195 mol of NaOH is...

  • change in Ph in buffers part A What is the pH of a buffer prepared by adding 0.607mol of the weak acid HA to 0.608mol...

    change in Ph in buffers part A What is the pH of a buffer prepared by adding 0.607mol of the weak acid HA to 0.608mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66

  • What is the pH after 0.150 mol of HCl is added to the buffer from Part...

    What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid Express the pH numerically to three decimal places. ► View Available Hint(s) ROO? V AE pH= 5.81 Submit Previous Answers X Incorrect; Try Again You used the final concentration of HA (after the addition of HCI), but you used the initial concentration of A You may want to review Hint 3. Determine the...

  • The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH=pKa +log[Base]/[Acid] Part A: What...

    The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH=pKa +log[Base]/[Acid] Part A: What is the pH of a buffer prepared by adding 0.809mol of the weak acid HA to 0.406mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66

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