HomeworkLib
Question

Calculate the pH of a solution containing 0.0334 M potassium hydrogen fumarate and 0.021 M dipotassium...

Calculate the pH of a solution containing 0.0334 M potassium hydrogen fumarate and 0.021 M dipotassium fumarate. The Ka values for fumaric acid are 9.50 × 10-4 (Ka1) and 3.30 × 10-5 (Ka2).

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

Homework Answers

Answer #1

To do the calculations we have to consider the second ionization reaction as Potassium Hydrogen fumerate is formed due to the ionization of the 1st proton.

pKa2 = -logKa2 = -log (3.30 *10^-5) = 4.48

pH = pKa2 + log [dipotassium fumarate/Potassium hydrogen fumerate]

    = 4.48 + log [0.021/0.0334]

    =4.28

1 2
Add a comment
Know the answer?
Add Answer to:
Calculate the pH of a solution containing 0.0334 M potassium hydrogen fumarate and 0.021 M dipotassium...
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

  • Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M...

    Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M disodium maleate. The Ka values for maleic acid are 1.20 x 10 (Ka1) and 5.37 x 10-7 (Ka2) 1.8 pH A solution containing 0.0306 M succinic acid and 0.019 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 105 (Kal) and 2.31 x 10 (Ka2) pH

  • Calculate the pH of each solution. A solution containing 0.0345 M0.0345 M maleic acid and 0.047...

    Calculate the pH of each solution. A solution containing 0.0345 M0.0345 M maleic acid and 0.047 M0.047 M disodium maleate. The ?aKa values for maleic acid are 1.20×10−2 (?a1)1.20×10−2 (Ka1) and 5.37×10−7 (?a2).5.37×10−7 (Ka2). pH= A solution containing 0.0320 M0.0320 M succinic acid and 0.018 M0.018 M potassium hydrogen succinate. The ?aKa values for succinic acid are 6.21×10−5 (?a1)6.21×10−5 (Ka1) and 2.31×10−6 (?a2).2.31×10−6 (Ka2). pH=

  • O Attempt 7 Calculate the pH of each solution. A solution containing 0.0243 M maleic acid...

    O Attempt 7 Calculate the pH of each solution. A solution containing 0.0243 M maleic acid and 0.034 M disodium maleate. The K, values for maleic acid are 1.20 x 10 (Kal) and 5.37 x 10 (Ka2) pH| 1.93 A solution containing 0.0360M succinic acid and 0.023 M potassium hydrogen succinate. The K, values for succinic acid are 6.21 x 10 (Kal) and 2.31 x 10 (K2) 9- = Hd 10

  • 2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic...

    2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic acid is 1.8x10-5 . 3. Calculate the pH of a 0.225 M solution of H2CO3. Ka1 = 4.3x10^-7 ; Ka2 = 5.6x10^-11 4. Calculate the pH of a 0.0080 M solution of sulfuric acid. Ka2 = 1.2x10^-2

  • part 1 is wrong Calculate the pH of each solution. A solution containing 0.0243 M maleic...

    part 1 is wrong Calculate the pH of each solution. A solution containing 0.0243 M maleic acid and 0.034 M disodium maleate. The K, values for maleic acid are 1.20 x 10-?(K) and 5.37 x 10 (K2). pH = 2.00 A solution containing 0.0360 M succinic acid and 0.023 M potassium hydrogen succinate. The K, values for succinic acid are 6.21 x 10" (K1) and 2.31 x 10 "(K), pH = 4.01

  • calculate the ph of a buffer system containing 1.00 M propionic acid and 1.00 M potassium...

    calculate the ph of a buffer system containing 1.00 M propionic acid and 1.00 M potassium propionate after you add 0.200 mole of gaseous HCl to 1.00 L of solution. Ka for propionic acid = 1.35x10^-5

  • Calculate the pH of 1.00 x 10^-2 M oxalic acid solution. Calculate the pH of 1...

    Calculate the pH of 1.00 x 10^-2 M oxalic acid solution. Calculate the pH of 1 x 10^-2 M solution of sodium oxalate. Ka1 = 5.62 x 10^-2, Ka2 = 5.42 x 10^-5

  • 8. If the pH of a 0.20 M potassium oxalate solution is 8.82, calculate the experimental...

    8. If the pH of a 0.20 M potassium oxalate solution is 8.82, calculate the experimental value for Ka2 for oxalic acid. (Don't use any K values from the table)

  • 9.  What is the pH of a 25 mL solution of 1.0 M potassium fluoride (KF)?  The Ka...

    9.  What is the pH of a 25 mL solution of 1.0 M potassium fluoride (KF)?  The Ka of hydrofluoric acid (HF) is 7.2 x 10-4.                   A.  6.5                   B.  7.4                   C.  8.6                   D.  9.9 10. What is the concentration of arsenate ions in 3.5 M solution of arsenic acid (H3AsO4)?                                                       Ka1= 5.0 x 10-3                                                       Ka2= 9.3 x 10-8                                                       Ka3= 3.0 x 10-12 A.  2.1 x 10-18M B.  9.3 x 10-8M C.  1.2 x 10-6M D.  3.0 x 10-12M *Please answer both* Thank you!

  • What is the pH of a 1.00 M solution of disodium sulfate (Na2SO4)? You can calculate...

    What is the pH of a 1.00 M solution of disodium sulfate (Na2SO4)? You can calculate the Kb from the Ka values given in the question 1. (Ka1 = large Ka2 = 1.2 x 10-2) 7.94 8.02 6.01 7.96

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