The complete question is:
An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of calcium nitrate.
The net ionic equation contains which of the following species (when balanced in standard form)?
a. 2NO3-(aq)
b. Ca2+(aq)
Answer:
b. Ca2+(aq)
Ca2+ (aq) + SO4^2-(aq) --------------> CaSO4(s)
Explanation:
The overall ionic equation is:
Ca2+(aq) + 2NO3-(aq) + 2NH4+(aq) + SO4^2-(aq) ---------------> CaSO4(s) + 2NH4NO3(aq)
The NO3- and NH4+ are spectator ions as they do not participate in the formation of the precipitate CaSO4.
The net ionic equation is:
Ca2+ (aq) + SO4^2-(aq) --------------> CaSO4(s)
The spectator ions form the soluble ammonium trioxonitrate V
Im not 100% sure, but I think the answer is C. If not, Im sorry for bothering you.
It can allow the molecule (like water) to be polar because it has a negative and positive side to it (oxygen holds the negatives tight causing the hydrogens to be positive).
Answer:
0.01836 M
Explanation:
Again the reaction equation is;
Fe(s) + Mn2+(aq) → Fe2+(aq) + Mn(s)
E°cell= 0.77 V
Ecell= 0.78 V
[Mn2+] = 0.040 M
[Fe2+] = the unknown
n=2
From Nernst's equation;
Ecell= E°cell- 0.0592/n log Q
0.78= 0.77 - 0.0592/2 log [Fe2+] /[0.040]
0.78-0.77= - 0.0592/2 log [Fe2+] /[0.040]
0.01/ -0.0296= log [Fe2+] /[0.040]
-0.3378= log [Fe2+] /[0.040]
Antilog(-0.3378) = [Fe2+] /[0.040]
0.459= [Fe2+] /[0.040]
[Fe2+] = 0.459 × 0.040
[Fe2+] = 0.01836 M