Look at the titration curve below and determine what acid from the list could be the acid beingtitrated with NaOH. The black colored circle represents the equivalence point.O(A) HCNO Ka = 3.5 × 10-4 (B) H2C2O4 Ka = 5.9 × 10-2(C) HCHO₂ Ka = 1.8 × 10-4 (D) HC (E) HN3 Ka = 1.9 × 10-5pH7.03.4602550Submitvolume NaOH added

Step 1: Determine the volume at the equivalence point. From the given titration curve the volume at…

Answered: Look at the titration curve below and…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 52SSC

See similar textbooks

Similar questions

8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Assume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl. (a) What is the pH of the NH3 solution before the titration begins? (b) What is the pH of the equivalence point? (c) What is the pH at the midpoint of the titration? (d) Which indicator would you suggest to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 11.0, 15.0, 20.0, 22.0, and 25.0 mL of the acid. Combine this information with that from (a) through (c) and plot the titration curve.
a) What will be the H+ concentration in a 1.0 M HCN solution? (HCN is a weak acid: Ka = 4.0x10-1) b) Methylamine is a weak base. Calculate the pH of a 0.2 M aqueous solution of methylamine. The Kb = 3.6 x 10-4 c) In a titration, 15.0 mL of 0.100 M phosphoric acid H3PO4 neutralises 30.0 mL of a solution of calcium hydroxide Ca(OH)2. What is the M of the solution of calcium hydroxide?
The titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH. The reaction can be represented as: CH3 CO2 H + OH− ⟶ CH3 CO2− + H2 O(a) What is the initial pH before any amount of the NaOH solution has been added? Ka = 1.8 × 10−5 for CH3CO2H. (b) Find the pH after 25.00 mL of the NaOH solution have been added.(c) Find the pH after 12.50 mL of the NaOH solution has been added.(d) Find the pH after 37.50 mL of the NaOH solution has been added.
In the titration of 60.0 mL of 1.0 M methylamine, CH3NH₂ (K₁ = 4.4 x 10-4), with 0.50 M HCI, calculate the pH under the following conditions. (a) after 0.00 mL of 0.50 M HCI has been added 4.0 (b) after 20.0 mL of 0.50 M HCI has been added 4.0✔ (c) after 60.0 mL of 0.50 M HCI has been added 4.0✔ (d) at the stoichiometric point 4.0✔ (e) after 200.00 mL of 0.50 M HCI has been added 4.0
Calculate the pH of a buffer system containing 3.0 M NH3 and 2.0 M NH4Cl. (K, of NH4, the acid in this system, is 5.6 x 10-10.) Enter your answer in the provided box. PH
Calculate the pH of a buffer system containing 1.5 M NH3 and 1.5 M NHẠCI. (K, of NH, the acid in this system, is 5.6 x 1010.) Enter your answer in the provided box. pH =
Answer: Get the answers by The samples of nitric and acetic acids shown here are both titrated with a 0.100 M solution of NAOH(aq). Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3. (b) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration. (c) Phenolphthalein would be a suitable indicator for both titrations. (d) The pH at the beginning of the two titrations will be the same. (e) The titration curves will both be essentially the same after passing the equivalence point. (f) Methyl red would be a suitable indicator for both titrations. 25.0 mL of 1.0 M HNOz(ng) 25.0 mL of 1.0 M CH;COOH(aq)
Use Figure to find an indicator for these titrations:(a) 0.10 M HCl with 0.10 M NaOH(b) 0.10 M HCOOH with 0.10 M NaOH
Which of the following is the most effective buffer system for a pH value of 5.50? (a) HC3H5O2/C3H5O2− Ka = 1.34x10−5 (b) HC2O4−/C2O42− Ka = 5.42x10−5(c) HNO2/NO2− Ka = 7.10x10−4(d) HOCl/OCl− Ka = 3.00x10−8
What is the pH of a buffer solution consistig of 0.035 M NH3 and 0.050 M NH4 + ? (Ka for HN4+ = 5.6 x 10-10)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS