Question

http://papers.xtremepapers.com/CIE/Cambridge%20International%20A%20and%20AS%20Level/Chemistry%20%289701%29/9701_w09_qp_42.pdf
q2dii)

Answer 1

@aaronq

Answer 2

so you have: \(K_c=\dfrac{[Ag(NH_2)_2]}{[NH_3]^2[Ag^+]}\)

\(Ag^+(aq) + 2NH_3(aq) \rightleftharpoons [Ag(NH_3)_2]^+\)

you have \([Ag(NH_3)_2]^+=0.1~M\), find \([NH_3]\) and \([Ag^+]\) in this solution.

You want \([Ag^+]\) to be what you found in (c) (i), so find the difference from what you want to what you have then use the equilibrium expression. Try it and i'll look at it

Answer 3

got it! thanks @aaronq :)

Answer 4

good stuff! no problem, dude