TEXTBOOK PROBLEM 6A.1

[Sophia Kangavari 1D]

Hi, I was working through the textbook problems for focus 6A and I am a bit confused as to why the conjugate acid of CH3NH2, which is CH3NH3+ is positively charged. Shouldn't it be neutral? Likewise, shouldn't the conjugate acid of NH2NH2, which contains two neutrally charged polyatomic ion groups be neutral as well? I've atatched a picture to show the answer in the textbook that I'm, not quite getting.Thanks!

[Natalie Keung 1D]

Hi, I believe that is because the conjugate acid gains a proton, which is positively charged.

Also where did you find the focus 6A.1 questions?

[Allison Li 2F]

Hi! The conjugate acid gains a proton, so it is CH3NH3. Because the proton is positive, it has an overall positive charge, making it CH3NH3+. Likewise, if you lose a proton, the compound will be slightly negative.