In a double replacement reactions aqueous Silver Nitrate reacts with aqueous Calcium Chloride and a silver to form the solid Silver Chloride and aqueous Calcium Nitrate. I took the silver out of the equation because isnt a double replacement reaction just two aqueous solutions? Is that right? need some help show me the answer you guys got.

Question

anonymous · Answer

oh Im looking for the final balanced equation

anonymous · Answer

i'm assuming you want an equation that follows the solubility rules. if so, then the equation would be 

$$Ag^ (+3) + CaCl \rightarrow AgCl + Ca^ (+2)$$

The reason is because nitrate is ALWAYS soluble, hence you don't have to consider it in an equation even for double replacement. Also, any halides are soluble EXCEPT when in a combined with Ag, Pb, or Hg.

So, since in silver nitrate you get rid of the nitrate, you are left with a silver (just the ion) and you continue with the reaction prediction by treating it similar to a single replacement.

Hope this helps!

preetha · Answer

It is a double displacement, but, one of the products AgCl is insoluble.  So everything else cancels out and you get Ag(+) + Cl(-) -> AgCl(s)  This is the net ionic.