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.
oh Im looking for the final balanced equation
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!
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.
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