(A) Will AgCl(s) precipitate from 1.50 L of a solution that is 0.100 M AgNO₃ and 0.225 M NH₃ if 1.00 mL of 3.50 M NaCl is added? What are [Ag⁺] and [Cl^-] immediately after the addition of the 1.00 mL of 3.50 M NaCl? Take into account the dilution of the NaCl(aq), but assume the total volume remains at 1.50 L.

(B) A solution is prepared that is 0.100 M in Pb(NO₃)₂ and 0.250 M in the ethylenediaminetetraacetate anion, EDTA^4-. Together, Pb²⁺ and EDTA^4- form the complex ion [PbEDTA]^2-. If the solution is also made 0.10 M in I^-, will PbI₂(s) precipitate? For PbI_2, K_sp = 7.1 x 10^-9; for [PbEDTA]^2-, K_f = 2 x 10¹⁸.