For each reaction that produces a precipitate, write a balance molecular equation and net ionic equation. For molecular equations, assume that all tested cations are in the form of nitrates, such as AgNO3, Pb(NO3)2, Ca(NO3)2, Fe(NO3)3, and Cu(NO3)2. Equations for No. 2(a) are given as examples; (a) Reaction: AgNO3 + Na2S Molecular equation: 2AgNO3(aq) + Na2S(aq) ® Ag2S(s) + 2NaNO3(aq) Net ionic eqn.: 2Ag+(aq) + S2-(aq) ® Ag2S(s) (Organize your equations according to the letter in each observation box. You don’t have to write any equation for those reactions that did not produce a precipitate.) Ag+ Pb2+ Ca2+ Fe3+ Cu2+ NaCl (Cl-) (k) White Precipitate AgCl (l) White Precipitate PbCl2 (m) No Precipitate (n) Yellow Percipitate FeCl3 (o) Light Blue Precipitate CuCl2
For each reaction that produces a precipitate, write a balance molecular equation and net ionic equation. For molecular equations, assume that all tested cations are in the form of nitrates, such as AgNO3, Pb(NO3)2, Ca(NO3)2, Fe(NO3)3, and Cu(NO3)2. Equations for No. 2(a) are given as examples;
(a) Reaction: AgNO3 + Na2S
Molecular equation: 2AgNO3(aq) + Na2S(aq) ® Ag2S(s) + 2NaNO3(aq)
Net ionic eqn.: 2Ag+(aq) + S2-(aq) ® Ag2S(s)
(Organize your equations according to the letter in each observation box. You don’t have to write any equation for those reactions that did not produce a precipitate.)
Ag+ Pb2+ Ca2+ Fe3+ Cu2+
|
NaCl (Cl-) |
(k) White Precipitate
AgCl |
(l) White Precipitate
PbCl2 |
(m) No Precipitate
|
(n) Yellow Percipitate
FeCl3 |
(o) Light Blue Precipitate
CuCl2 |
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