Many ionic compounds are water soluble, so, for example, we canmake solutions of sodium iodide, NaI, and lead(II) nitrate,Pb(NO3)2, by simply dissolving the ionic solids in water. In theprocess of dissolving, the ions from the ionic solutes (sometimesreferred to as salts) are split apart and hydrated (surrounded) bywater molecules. We represent the species in the sodium iodidesolution as Na+(aq) and I–(aq), and in the lead(II) nitratesolution as the species Pb2+(aq) and NO3–(aq).

A) Complete the balanced overall ionic equation for sodiumiodide dissolving in water. NaI(s)...

b) Complete the balanced overall ionic equation for lead(II)nitrate dissolving in water. Pb(NO3)2(s)

c)What will happen if we combine the solution of sodium iodideand the solution of lead(II) nitrate? The solutions will mix, soall of the ions will be evenly distributed throughout the entiresolution. But sometimes mixing solutions containing dissolved ionsleads to a precipitation reaction: the formation of a new insolublecompound. Based on the information presented in that table,complete the balanced overall ionic equation for the mixing ofthese two solutions. 2Na^+(aq)+2I^-(aq)+pB^2+(aq)+2NO^-3(aq)