suppose we are given the following experimentally observed facts regarding the r

Question

suppose we are given the following experimentally observed facts regarding the reactions of silver ion. a) Ag^+ reacts with Cl^- to give white AgCl(s). b) Ag^+ reacts with ammonia to give a quite stable complex ion, Ag(NH3)2^+. c) A black suspension of solid silver oxide, Ag2O(s), shaken with NaCl solution, changes to white AgCl(s). d) AgCl(s) will dissolve when ammonia solution is added, but AgI(s) does not dissolve under these conditions. Write equations for any net reactions in the cases above; then, based on these observations, arrange each of the substances AgCl, AgI, Ag2O, and Ag(NH3)2^+ in such an order that their solutions with water wold give a successively decreasing concentration of Ag^+

Explanation / Answer

Net ionic equations are as follows we omit the spectator ions- the ions that appear on both sides of the equation

a) Ag+ (aq)+ Cl- (aq) ---> AgCl(s)

b) Ag+(aq) + 2 NH3 (aq) --> [Ag(NH3)2]+ (aq)

c) Ag2O (s)+ 2 Na+ (aq) + 2 Cl- (aq) --> 2 AgCl (s) + Na2O

in this reaction Na2O reacts with water (because we have taken NaCl solution) and forms NaOH as

Na2O + H2O ==> 2NaOH

d) AgBr and AgI are less soluble than AgCl; AgBr will go into solution in 15 M NH3 , but AgI is so insoluble that it will not.

e) Arranging in decreasing concentration of Ag+ from top to bottom

Ag(NH3)2+
Ag2O
AgCl
AgI

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