Question #739af

1 Answer
Apr 20, 2016

Answer:

All nitrates are soluble; #PbX_2# is insoluble.

Explanation:

#Pb(NO_3)_2(aq) + 2KI(aq) rarr PbI_2(s)darr + 2KI(aq)#

Of course I could make this a net ionic equation. However, this question illustrates aqueous solubility rules. All nitrates are soluble; this allows us to get #Pb^(2+)# or #Ag^(+)# into aqueous solution. Most halides are soluble. The exceptions are silver halides, mercurous halides, and LEAD HALIDES. #PbI_2# wil precipitate from solution as a yellow solid. You should have done experiments to illustrate the reaction.