- #1
SMc21
- 10
- 0
We just got a worksheet about acids and bases today. One of the questions said:
"Using the Bronsted-Lowry theory of acids and bases, write equations for the following acid-base reactions and indicate each conjugate acid-base pair."
One such reaction was CH3NH2 + H2O
I checked a ton of websites, and nearly every answer I can find says that CH3NH2 is a base, and the products of this reaction are OH- + CH3NH3+.
However, my teacher seeemd to think that CH3NH2 was an acid, because if it was a Bronsted base and another H+ was added to it, it wouldn't make sense, since NH3 is a stable compound itself and wouldn't be part of a larger compound.
I know that CH3NH2 should be a base, but I also see my teacher's point about it being an acid. How can this compound accept another hydrogen? It'd also help if I could see a Lewis dot structure of CH3NH3+.
"Using the Bronsted-Lowry theory of acids and bases, write equations for the following acid-base reactions and indicate each conjugate acid-base pair."
One such reaction was CH3NH2 + H2O
I checked a ton of websites, and nearly every answer I can find says that CH3NH2 is a base, and the products of this reaction are OH- + CH3NH3+.
However, my teacher seeemd to think that CH3NH2 was an acid, because if it was a Bronsted base and another H+ was added to it, it wouldn't make sense, since NH3 is a stable compound itself and wouldn't be part of a larger compound.
I know that CH3NH2 should be a base, but I also see my teacher's point about it being an acid. How can this compound accept another hydrogen? It'd also help if I could see a Lewis dot structure of CH3NH3+.