Use the References to access important values if needed for this question. The f

Question

Use the References to access important values if needed for this question. The following equation represents the reaction that occurs when aqueous solutions of ammonium chloride and lead(I nitrate are combined. Ph(NO3)2(aq) + 2NH4CI(aq)- PbCh(s) + 2NH4NOg(aq) Write a balanced net ionic equation for the reaction. Assume that all ionic compounds that are in aqueous solution are dissociated Use the pull-down choices to specify states such as (aq) or (s). If a box is not needed leave it blank Submit Answer Retry Entire Group 8 more group attempts remaining

Explanation / Answer

Start off with the double replacement reaction:
Pb(NO3)2 + NH4Cl --> PbCl2 + NH4NO3
NH4NO3 is soluble because NH4+ is soluble
PbCl2 is insoluble, however. It's the precipitate.
Your balanced equation with phases is:
Pb(NO3)2(aq) + 2NH4Cl(aq) --> PbCl2(s) + 2NH4NO3(aq)
The overall ionic equation is:
Pb^2+(aq) + 2NO3^-(aq) + 2NH4^+(aq) + 2Cl^-(aq) --> PbCl2(s) + 2NH4^+(aq) + NO3^-(aq)
and taking out the ions that are on both sides, the net ionic equation is:
Pb^2+(aq) + 2Cl^-(aq) --> PbCl2(s)

(the ^ means it's a superscript)

2 K+ + S2- + Co2+ + 2 Cl- >> 2 K+ + 2 Cl- + CoS

Co2+ + S2- >> CoS

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