Usually HCl is used, but my question is whether NaCl can be used as well. If so, why? Does it have to do with the activity series? If so, doesn't the activity series reveal that none of the silver group can replace the hydrogen ion?
2007-02-23 06:33:21 · 2 answers · asked by Blarepen 2 in Science & Mathematics ➔ Chemistry
Usually HCl is used, but my question is whether NaCl can be used as well. If so, why? Does it have to do with the activity series? If so, doesn't the activity series reveal that none of the silver group can replace the hydrogen ion?
In the net ionic equation for the precipitation of these silver groups, H+ is not present. In light of this fact, why is pH important for this particular precipitation reaction?
2007-02-23 08:23:53 · update #1
Sodium chloride could be used to precipitate the Silver group cations. All you need is a source of chloride ion.
Why is pH important for this particular precipitation reaction?
What you want to avoid is the following (which might happed in basic solutions):
Ag+ (aq) + OH- (aq) --> AgOH (s)
Pb+2 (aq) + 2 OH- (aq) --> Pb(OH)2 (s)
Hg+2 (aq) + 2 OH- (aq) --> Hg(OH)2 (s)
2007-02-28 11:57:34 · answer #1 · answered by Richard 7 · 11⤊ 0⤋
In precipitation reactions is important the value of pH so these reactions are possible only at acid pH and NaCl can't be used because it contains Cl- but is not acid
2007-02-23 15:38:28 · answer #2 · answered by Non più attiva su answers 7 · 0⤊ 0⤋