Calculating the pH at equivalence of a titration0/5IzabellaA chemist titrates 80.0 mL of a 0.7536M dimethylamine ((CH3)2NH) solution with 0.0940M HBr solution at 25 °C. Calculate the pH at equivalence. ThepK of dimethylamine is 3.27.bRound your answer to 2 decimal places.Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added.pH=☑ك18ArB?

pH = 5.90Explanation:Given: V(CH3)2NH=80.0mL;[(CH3)2NH]=0.7536M;[HBr]=0.0940M;pKb=3.27at the…

Answered: Calculating the pH at equivalence of a…

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

i need the answer quickly
65 mL of 0.65 M benzoic acid (Ka = 6.4×10-5) is titrated by 0.05 M NaOH. 1)Calculate the pH of the acid solution before any titrant is added. 2)Calculate the pH after 795.9 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 3)Calculate the pH after 845 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid. 4)Calculate the pH after 1.58 x 10^3 mL of 0.05 M NaOH is added to 65 mL of 0.65 M benzoic acid.
A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box
Consider the titration of 40 mL of 0.2 M NH3 with 0.5 M HCI. Calculate the pH after addition of the following amounts of 0.5 M HCI at 25 °C Part A O mL (initial pH) ? νη ΑΣφ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part B 5 mL ? Πν ΑΣφ Submit Request Answer Part C half-way to equivalence point
O ACIDS AND BASES Calculating the pH of a buffer A solution is prepared at 25 °c that is initially 0.077M in trimethylamine ((CH3)3N), a weak base with K₁=7.4× 10-4, and 0.50M in trimethylammonium Calculate the pH of the solution. Round your answer chloride ((CH3), NHCI) to 2 decimal places. pH = 1/3 X
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
Do not give answer in image and hand writing
The following table shows the values of ionization constants for a number of acids and bases at 25 °C: Formula Ka HC2H302 1.8x10-5 HCIO2 NH3 HCIO 1.1x10-2 2.9x10-8 Kb 1.76x10-5 For the best system, calculate the ratio of the masses of the buffer components required to make the buffer. Express your answer to two significant figures. PH = 7.30
Please assist with this question. I am confused.
Titus titrates 45 mL of 0.750 M lactic acid (HC₂H₂O², Ka NaOH. = 1.5 × 104) using 0.250 M Calculate the pH of the resulting solution at each of the following points in the titration. After adding 24.750000000000004 mL of the NaOH solution: At the equivalence point: After adding 191 mL of the NaOH solution:
Please don't provide handwritten solution... A 1.0 L solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value for Ka HC2H3O2 is 1.8 X 10-5. What is the pH of the buffer after adding 0.010 mol NaOH to the buffer.
Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?

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