A 117.6 mL sample of 0.100 M methylamine (CH3NH₂; Kb = 3.7 x 104) is titrated with 0.285 M HNO₂. Calculatethe pH after the addition of each of the following volumes of acid.Part A0.0 mLExpress the pH to two decimal places.pH =SubmitPart BpH =22.2 mLExpress the pH to two decimal places.Part CSubmitfor Panze for Part do for Part redo foart A reor Part A keyboard shortcuts for Part A help for Part ApH =Part Dfor Part 2 for Part Ndo for Part redo foart 8 resor Part B keyboard shortcuts for Part B help for Part B44.4 mLExpress the pH to two decimal places.Request AnswerSubmitpH =Request Answerfor PartSubmit66.6 mLExpress the pH to two decimal places.for Part Cdo for Part redo forart Crestor Part C keyboard shortcuts for Part C help for Part CRequest Answerfor Partor Partio for Part redo for DrRequest Answeror Part D keyboard shortcuts for Part D help for Part DReview | Constants | Periodic Table

The objective of the question is to calculate the

A 117.0 mL sample of 0.100 A methylamine (CH₂NH₂; K-3.7 x 10-) is strated with 0.205 M HNOS. Calculate the pit ater the addition of each of the following volumes of acid Part A Express the pH to two decimal places. pil. Submit Be Part B 22.2 ml Express the pH to two decimal places. pl Part C var Pans 22 V for Partre Submit pl 44.4 ml. Express the pH to two decimal places. Part D fog Pag 12 2018 Voo for Part redo tot refor Pan 8 keyboard shortcuts for Part help for Pan Submit pl. for Party Parto for Part redo forer Part C keyboard shortcuts for Part C help & Part 000 ml. Express the pH to two decimal places. A PA Part keyboard shortcuts for Part A her Part Submit Para o for Part&redotorer Part D keyboard shortcuts for Part D help & Part D

A 117.0 mL sample of 0.100 A methylamine (CH₂NH₂; K-3.7 x 10-) is strated with 0.205 M HNOS. Calculate the pit ater the addition of each of the following volumes of acid Part A Express the pH to two decimal places. pil. Submit Be Part B 22.2 ml Express the pH to two decimal places. pl Part C var Pans 22 V for Partre Submit pl 44.4 ml. Express the pH to two decimal places. Part D fog Pag 12 2018 Voo for Part redo tot refor Pan 8 keyboard shortcuts for Part help for Pan Submit pl. for Party Parto for Part redo forer Part C keyboard shortcuts for Part C help & Part 000 ml. Express the pH to two decimal places. A PA Part keyboard shortcuts for Part A her Part Submit Para o for Part&redotorer Part D keyboard shortcuts for Part D help & Part D

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 113CP: When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally...

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A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?
The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If die pH at 50.0 mL NaOH added is 4.0 and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka and Ka. for the diprotic acid. d.
Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.

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