Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Jsing the table of the weak base below, you have chosen Ethylamine as your weak base in the buffen solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline Pyridine NH3 CH;NH2 C2H5NH2 CH;NH, C3H;N NH,+ CH;NH3+ CH5NH3+ CH;NH;+ C3H;NH* 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 1. Compute the poH of the buffer solution. (round off final answer to 2 decimal places)

Jsing the table of the weak base below, you have chosen Ethylamine as your weak base in the buffen solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline Pyridine NH3 CH;NH2 C2H5NH2 CH;NH, C3H;N NH,+ CH;NH3+ CH5NH3+ CH;NH;+ C3H;NH* 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 1. Compute the poH of the buffer solution. (round off final answer to 2 decimal places)

Chemistry
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
icon
Related questions
Question

please show the solution with explanation thanksmuch love u

Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH4+ CH;NH3+ CH;NH;+ CH;NH;+ C;H;NH+ 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C3H;N 3.8 x 10-10 Pyridine 1.7 x 10-9 1. Compute the poH of the buffer solution. (round off final answer to 2 decimal places)
Transcribed Image Text:Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH4+ CH;NH3+ CH;NH;+ CH;NH;+ C;H;NH+ 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C3H;N 3.8 x 10-10 Pyridine 1.7 x 10-9 1. Compute the poH of the buffer solution. (round off final answer to 2 decimal places)
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Chemical Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS