4. Calculate the pH of a 0.100 M solution of alanine prepared from the form shown below. pKa(-COOH) = 2.344 and pKa (-NH;") = 9.868.H*H;N-CCO-CH3pH = 6.1065. Referring to Question 4, calculate the concentration of the fully protonated form of alanine inthe solution described in Question 4.[H2A*] = 1.72*10-$ M

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Calculate the pH of a 0.100 M solution of alanine prepared from the form shown below. pKa (-COOH) = 2.344 and pKa (-NH3")=9.868. H +H;N- С—с—о- CH3 pH = 6.106

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.16QAP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

4. Calculate the pH of a 0.100 M solution of alanine prepared from the form shown below. pKa
(-COOH) = 2.344 and pKa (-NH;") = 9.868.
H
*H;N-
C
C
O-
CH3
pH = 6.106
5. Referring to Question 4, calculate the concentration of the fully protonated form of alanine in
the solution described in Question 4.
[H2A*] = 1.72*10-$ M

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