HomeworkLib
Question

A weak base has an initial concentration of 0.287 M. After undergoing dissociation the pH is...

A weak base has an initial concentration of 0.287 M. After undergoing dissociation the pH is 12.23.

A- + H2O ⇌ OH- + HA

What is the percent ionization of the base?

Options:

A

5.92%

B

12.3%

C

1.68%

D

0.0123%

E

0.995%
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
A weak base has an initial concentration of 0.287 M. After undergoing dissociation the pH is...
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

  • A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is...

    A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H2O ⇌ H3O+ + A- What is the percent ionization of the acid?

  • Question 6 (1 point) A weak base has an initial concentration of 0.588 M. After undergoing...

    Question 6 (1 point) A weak base has an initial concentration of 0.588 M. After undergoing dissociation the pH is 12.14. A+ H2O = HA + OH- What is the percent ionization pf the base? 0.569% O 1.41% 4.84% 0.0992% 2.35%

  • A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is...

    A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H20 = H30* + A What is the percent ionization of the acid? 0.155% 2.34% 0.0993% 0.782% O 0.0118%

  • A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with...

    A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with a concentration of 0.1200 M is titrated with 0.1500 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.1200 M sample of HA? c. What is the percent ionization of the 0.1200 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 8.00 ml NaOH have been added?

  • percent ionization of a weak base pH and Percent lonization of a Weak Base Ammonia, NH,...

    percent ionization of a weak base pH and Percent lonization of a Weak Base Ammonia, NH, is a weak base with a Ky, value of 1.8 x 105 The degree to which a weak base dissociates is given by the base ionization content K) For the generic weak base, B B(aq) + H2O(1) BH(aq) + OH (!) this constant is given by Pan A KDO What is the pH of a 0.165 Mammonia solution? Express your answer numerically to two...

  • 1.Determine the percent ionization of a solution having a pH of 4.03 and an initial weak...

    1.Determine the percent ionization of a solution having a pH of 4.03 and an initial weak acid concentration ([HA]init) of 0.00017. 2. Determine the percent ionization of a solution having a pH of 4.57 and an initial weak acid concentration ([HA]init) of 0.00016. 3. A 0.100 M solution of a weak acid has a pH of 1.96. Calculate the [H3O+] in the solution. 4. Suppose you have a 0.100 M solution of a weak acid that has a pH of...

  • 14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00...

    14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00 ml sample with a concentration of 0.250 M is titrated with 0.150 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.250 M sample of HA? c. What is the percent ionization of the 0.250 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 12.00 ml 0.150M...

  • The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For...

    The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....

  • A weak acid, HF, is prepared with an initial concentration of 1.20 M. After reaching equilibrium,...

    A weak acid, HF, is prepared with an initial concentration of 1.20 M. After reaching equilibrium, it has a pH of 1.551. What is the percent ionization of this acid? Select one: 4.2% 0.84% 2.4% None of these 0.082%

  • A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What...

    A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+ (aq) + A (aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, K ? Answer in scientific...

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