Be sure to answer all parts.Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N(K₁ = 5.2 × 10-4), with 0.1000 M HCl solution after the following additions of titrant.(a) 11.00 mL:pH =(b) 20.10 mL:pH==(c) 29.00 mL:pH =XXX

Answered: Image /qna-images/answer/f77d9c52-07f2-47a9-a6ca-7b86b0dc6f19.jpg

Answered: Be sure to answer all parts. Find the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Give typed full explanation of all subparts not a single word hand written otherwise leave it
The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K, for the weak acid? 14.0 12.0 10.0 공 8.0 6.0 4.0 2.0 0.0 0.0 10.0 1444444444444ÄÄÄÄÄÄÄÄÄÄÄÄÄ 20.0 30.0 Volume of titrant (mL) 40.0 50.0
Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, Kp = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4
Really having trouble with this table for HC4H7O2 and C4H7O2, appreciate any help.
Consider the titration of 40.0 mL of 0.0600 M C6H5NH2 (a weak base; Kb = 4.30e-10) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH = (b) 6.0 mLpH = (c) 12.0 mLpH = (d) 18.0 mLpH = (e) 24.0 mLpH = (f) 45.6 mLpH =
Explain well with proper answer.
Please answer all part asap.
1) Determine the pH during the titration of 74.5 mL of 0.348 M nitrous acid (Ka = 4.5×10-4) by 0.348 M NaOH at the following points. (a) Before the addition of any NaOH ? (b) After the addition of 18.0 mL of NaOH ? (c) At the half-equivalence point (the titration midpoint) ? (d) At the equivalence point ? (e) After the addition of 112 mL of NaOH ?
I dont know how to do this question.
The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K₂ for the weak acid? 14.0- 12.0 10.0 € 8.0 6.0 4.0 2.0 0.0 + 0.0 10.0 20.0 ÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄKAAAAA 30.0 Volume of titrant (mL) 40.0 50.0
Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl. (Calculate each below using ICE and ICF tables.) Note you should NOT use M1V1=M2V2 (a) the initial pH of base? (b) the pH at 5.00mL added? (c) the pH at 1/2 the HCl needed to reach the equivalence point. (d) the volume of added acid required to reach the equivalence point? (e) the pH at equivalence point.
Determine the pH during the titration of 22.8 mL of 0.415 M acetic acid (K₂ = 1.8x10-5) by 0.344 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 6.40 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 41.3 mL of NaOH

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K₁ = 5.2 × 10-4), with 0.1000 M HCl solution after the following additions of titrant. (a) 11.00 mL: pH = (b) 20.10 mL: pH= = (c) 29.00 mL: pH = X X X