To a 250 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100 M AgNO3, 0.100 M NaBr, and 0.100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously. What mass of AgBr would precipitate from this mixture? [Hint: Ksp of AgBr=5.4*10^-13 and Kf of Ag(CN)2  ^- 1.0*10^21]

PLEASE HELP ME WITH THIS. I WOULD BE VERY THANKFUL

Formation constant of Ag(CN)2- is so high that the amount of Ag+left to react with Br- can not exceed the ksp of the AgBr
Hence no precipitate forms
you can work out this mathematically also by making ICE tables