True enough, dipole movement and hydrogen bonding are enough to dissolve ammonia in water molecularly.
But, I dunno, I was browsing a bit on wikipedia, as a general overview of what the chemistry conventions are, and most people seem to say that ammonium hydroxide is a weak base. And I don't agree, it seems to form a solution of very high pH, which makes it seem strong to me. But then again, with a pKb of 9.25, so yeah, not a very strong base.
Back to the original question, ammonia, dissolved in water, acts like anhydrous ammonia suspended in water? Ummm, no, I don't think so. In any reaction, it's going to behave like NH4+ and OH-, right?
And how do I draw the arrows on the forums?