Actually both comments perhaps, to quote:
"because Ellingham Diagrams tell us that Ag(OH) being unstable gets converted into Ag2O which is a much more stable compound for silver to be in. However in aqueous solutions, an equilibrium of such a kind can always exist"
"NH3 is a stronger ligand than OH−"
Assuming a starting Ag2O presence from the reaction, some Ag+ ions from limited solubility, and noting, "a ppt of AgOH appears and dissolves in excess ammonia", see https://books.google.com/books?id=uwJbSFRIqyAC&pg=PA37&lpg=PA37&dq=radical+attack+on+silver+Ag+%2B+%E2%80%A2OH++--%3E+AgOH&source=bl&ots=jG9-2NG9x3&sig=V9nVefopAXXKP3lFnxQYnJriG14&hl=en&sa=X&ved=2ahUKEwjasar_g7ffAhWlhOAKHQEDA_4Q6AEwGHoECAcQAQ#v=onepage&q&f=false :
2 AgOH = Ag2O + H2O
both comments may be right.
Further, in the presence of visible light leading to the photocatalyst Ag2O/Ag, which per research out of P.R. China (published 2011 in the ‘Chemistry, a European Journal’), which has been cited as a powerful stable visible light photocatalyst capable of generating electrons (e-) and holes (h+) (see https://onlinelibrary.wiley.com/doi/abs/10.1002/chem.201101032 ):
Ag2O/Ag + hv --> e− + h+
Ag+ + e- --> Ag
And, in the presence of active electron holes, any OH- created via:
XOH = X+ + OH- (where X = H or NH3 or Ag)
could be converted into •OH radical:
OH- (aq) + h+ --> •OH (aq)
which may attack Silver metal directly (see https://pubs.acs.org/doi/abs/10.1021/acs.jpca.7b08081?src=recsys&journalCode=jpcafh and superacidity related redox couples at http://beta.chem.uw.edu.pl/people/WGrochala/Ag2+_mechanism.pdf, and more generally radical attacks on metals in their lower valence states at https://srd.nist.gov/NSRDS/NSRDS-NBS-65.pdf , where one could postulate the half cell reactions: Ag = Ag+ + e- and •OH + e- = OH- with the net reaction below):
Ag + •OH (aq) --> AgOH (aq)
2 AgOH = Ag2O + H2O
Or: AgOH (aq) = Ag+ (aq) + OH- (aq) (based on some limited solubility of Ag2O)
producing the oxygen free Silver ion to complex with NH3 (or OH-, depending on the respect ion concentration) in a photo cyclic reaction. Note: the hydroxyl radical can be largely scavenged at high ammonia concentration (creating •NH2), so this path is pH sensitive.