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6th Edition 12.59

Posted: Wed Jan 16, 2019 11:45 am
by Fionna Shue 4L
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?

Re: 6th Edition 12.59

Posted: Wed Jan 16, 2019 2:05 pm
by Helen Zhao 1F
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.

Re: 6th Edition 12.59

Posted: Wed Jan 16, 2019 2:10 pm
by Michael Torres 4I
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.