[slayer]

(CH₃)₂NH₂BrO

This is the answer that I got:

(CH₃)₂NH₂⁺ (aq) + H₂O (l) <---> OH^- + (CH₃)₂NH (aq)

where (CH₃)₂NH₂⁺ (aq) = Acid

where (CH₃)₂NH (aq) = Conjugate base

why is this wrong?

[Borek]

How strong a base is BrO^-?

[slayer]

weak base?

[Borek]

HBrO pKa = 8.7

[mdlhvn]

(CH₃)₂NH₂⁺ (aq) + H₂O (l) <---> OH^- + (CH₃)₂NH (aq)

definitely wrong reaction. Unbalance charge
Please check!

[slayer]

Im still stuck on this problem. I dont know what my acid or base is.

[slayer]

So, what i should be concentrated on is...

BrO^- (aq) + H₂O (l) <----> HBrO (aq) + OH^- (aq) ??

[slayer]

Borek,

why did you decide to rule out the (CH3)2NH2 from potentially being the base?

[Borek]

BrO^- (aq) + H₂O (l) <----> HBrO (aq) + OH^- (aq) ??

Yep. pKa for hypobromous acid is 9.7, pKb for dimethylamine is 3.3. Dimethylamine is much stronger base than HBrO is an acid. When they are in the form of salt situation reverses - conjugated base of HBrO (BrO^-) is stronger then dimethylamine conjugated acid.

why did you decide to rule out the (CH3)2NH2 from potentially being the base?

Looks like you have a problem recognizing Bronsted-Lowry acids and bases. Protonated amine is an acid. It is a base BEFORE it gets protonated, as it is ready to accept proton. Once it gets protonated it is ready to donate a proton and as such it is an acid.