# 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
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

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