QUESTION 2Calculate the ratio [CH3COOH]/[NaCH3COO] that gives a solution with pH = 5.00?Hint: Rearrange the Hendersen-Hasselbach equation to solvepH = pka + log [base]/[acid]The Ka of CH3COOH is 1.8x10-50.280.360.440.55O 0.63

The Henderson Hasselbalch equation for acidic buffer is given as :

Answered: QUESTION 2 Calculate the ratio…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.45QE

See similar textbooks

Similar questions

Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
For H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by systematic method
The pH of a 0.24 M solution of dimethylamine is 12.51. Calculate the Kb value for dimethylamine (4.4 × 10−4) Calculate Kb for F- if Ka for HF is 7.1 x 10–4. Polyprotic Acids and Mixture of Acids please help me with this problem
Hello, i am provided the pH levels and volumes for Bromocresol Green weak acid by strong base and strong base by weak acid. I am also provided the pH levels and volumes for Phenolphthalein weak acid by strong base and strong base by weak acid. How can we set up a table with all these information to make a graph for each. Heres the data Bromocresol Green: - weak acid by strong base: 12.80 pH; 20.3 mL - strong base by weak acid: 1.49 pH; 20.1 mL Phenolphthalein: - weak acid by strong base: 12.83 pH; 20.1 mL - strong base by weak acid:1.49 pH; 20.1 mL
Calculate the pH of a 0.40 M CH3COOna solution. Kb for CH3COO- = 5.6*10^-10. (Show the dissociation equation for salt, and show the reaction of CH3COO- ion with H2O)
pH calculation after the second equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 69.4 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5
2,What is the pH of the solution with hydronium ion concentration of 6.3 x 10-12 M? Group of answer choices 10.80 12.60 11.20 11.80 10.20 3,Calculate the pH of 0.50 L of the solution containing 5.61.0g KOH dissolved at 25oC. Group of answer choices 13.30 13.00 0.33 13.70 1.33 4. Calculate the [H3O+]of the solution with pH=9.2. Group of answer choices 2.0 x 10-10 3.6 x 10-9 6.3 x 10-10 9.2 x 10-9 2.0 x 10-9
The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKb of this weak base (3 significant figures).
pH calculation when the second equivalence pointis reached: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 50.0 ml of 0.500 MNaOH. Round your calculated value for pH to twofigures to the right of the decimal point. Significantconstants: Ka1 of oxalic acid = 5.60 x 10^-2 and Ka2of oxalic acid = 5.42 x 10^-5
pH calculation before the first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 23 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka of oxalic acid = 5.60 x 10^-2 and Ka of hydrogenoxalate anion = 5.42 x 10^-5
Please solve question #2 1. A 1.00 L Tris buffer solution is made by mixing 121.14 g of Tris base (MW = 121.14 g/mol), 84 mL of 10 M HCl and 916 mL of water. What is the pH of the prepared Tris buffer? 2. A lab mate accidentally spilled 10 mL of 10 M HCl onto the petri dish culturing Azotobacter. How much do you expect the pH of the solution to change (little, a lot or not at all)? Calculate the resulting pH after the HCl spill.
to make a basic solution byadding an acid to water. She says allyou need to do is make a 2.0×10−9 Maqueous solution of HI, giving [H+] =2.0×10–9 M. Taking the negative log ofthis concentration yields a pH of 8.7.This is within the range of bases on thepH scale. What is going on here? Canyour lab partner really defy the laws ofchemistry?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

QUESTION 2 Calculate the ratio [CH3COOH]/[NaCH3COO] that gives a solution with pH = 5.00? Hint: Rearrange the Hendersen-Hasselbach equation to solve pH = pka + log [base]/[acid] The Ka of CH3COOH is 1.8x10-5 0.28 0.36 0.44 0.55 O 0.63