6th Edition 12.59

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Fionna Shue 4L
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

6th Edition 12.59

Postby Fionna Shue 4L » Wed Jan 16, 2019 11:45 am

Calculate the pH, pOH, and percentage protonation of solute in each of the following aqueous solutions: (a) 0.057 m NH3(aq); (b) 0.162 m NH2OH(aq); (c) 0.35 m (CH3)3N(aq); (d) 0.0073 m codeine, given that the pKa of its conjugate acid is 8.21.

For parts b, c, and d, how are we supposed to determine if the molecule is an acid or base?

Helen Zhao 1F
Posts: 31
Joined: Fri Sep 28, 2018 12:20 am

Re: 6th Edition 12.59

Postby Helen Zhao 1F » Wed Jan 16, 2019 2:05 pm

They're all bases because the question says "given that the pka of its conjugate acid". "its" refers to the molecules listed in each subsection (a, b, c, d) and because the question says conjugate acid, then "its" are bases.

Michael Torres 4I
Posts: 92
Joined: Thu May 10, 2018 3:00 am
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Re: 6th Edition 12.59

Postby Michael Torres 4I » Wed Jan 16, 2019 2:10 pm

Because the question asks for the percentage protonation of the following solutes, then you can assume that the solutes that are given are bases. Bases can become protonated whereas acids become deprotonated.

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