Answer to Question #205747 in General Chemistry for Jerry

Question #205747

For alanine, Ka1 = 5.1 x 10 -3, Ka2 = 1.8 x 10 -10

 a) Calculate the ratios [Z] / [C

+] and [Z] / [A

−] at pH = 10.50

 b) Calculate the pH when [Z] = [C

+] and when [Z] = [A

−] if pH= - log [H

+]


1
Expert's answer
2021-06-11T06:44:21-0400

In strongly acidic conditions, most of the alanine molecules will gain a proton. but there is no pH at which every alanine molecule gains a proton.


Likewise, in strongly alkaline conditions, most of the alanine molecules will lose a proton. but there is no pH at which every alanine molecule loses a proton.


On reflection, I guess I misunderstood the question. When you say, “[Z] = [C+]”, I read it that you meant that every alanine molecule gains a proton. But now I reckon you mean that the concentration of zwitterions is equal to the concentration of positive ions. And similarly for when you say “[Z] = [A−]”.


I assume that each Kₐ is defined as [H⁺][ion without H]/[ion with H]. Because, in each scenario, [ion without H] = [ion with H], these cancel in the arithmetic so Kₐ=[H⁺].


For Kₐ=5.1 × 10⁻³, [H⁺]=5.1 × 10⁻³ and pH=-log(5.1 × 10⁻³)=2.3

For Kₐ=1.8 × 10⁻¹⁰, [H⁺]=1.8 × 10⁻¹⁰ and pH=-log(1.8 × 10⁻¹⁰)=9.7

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be the first!

Leave a comment

Ask Your question

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS