Write the net ionic equation for the precipitation reaction between ammonium sulfide and cadmium nitrate.
Cd^2+(aq) + S^2-(aq) ==> CdS(s)
how does the addition of a nonvolatile solute affect the vapor pressure of the solvent into which it is dissolved?
To write the net ionic equation for the precipitation reaction between ammonium sulfide and cadmium nitrate, we first need to write the balanced equation for the overall reaction.
The balanced molecular equation for the reaction is:
(NH4)2S(aq) + Cd(NO3)2(aq) -> CdS(s) + 2NH4NO3(aq)
Now, let's write the ionic equation by dissociating all the soluble compounds into their respective ions. In this case, ammonium sulfide (NH4)2S and cadmium nitrate Cd(NO3)2 are both soluble in water, so they will dissociate into their constituent ions:
(NH4)2S(aq) -> 2NH4+(aq) + S2-(aq)
Cd(NO3)2(aq) -> Cd2+(aq) + 2NO3-(aq)
The ionic equation can be written as:
2NH4+(aq) + S2-(aq) + Cd2+(aq) + 2NO3-(aq) -> CdS(s) + 2NH4+(aq) + 2NO3-(aq)
Finally, we can eliminate the spectator ions, which are the ions that appear on both sides of the equation unchanged. In this reaction, the NH4+ and NO3- ions are present on both sides of the equation, so we can remove them. The net ionic equation for this precipitation reaction is:
S2-(aq) + Cd2+(aq) -> CdS(s)
This equation represents the key species involved in the precipitation reaction, showing the formation of solid cadmium sulfide (CdS) from the reaction between ammonium sulfide and cadmium nitrate.