1. What is the net ionic equation for the reaction that occurs when aqueous solutions of AgNO3 and CaCl2 are mixed and a precipitate forms? A. Ca+2(aq) + NO3-(aq)  Ca(NO3)2(aq) B. Ag2+(aq) + 2Cl-(aq)  AgCl2(s) C. Cl−(aq) + Ag+(aq) ⟶ AgCl(s) D. None of the above because no reaction occurs

C.

Explanation:

In this question our options are:

A.

B.

C.

D. None of the above because no reaction occurs

We have to remember that the ions produced by are:

 and

And the ions produced by are:

and

Additionally, we will have a double displacement reaction so the compounds produce are:

and

If we remember the solubility rules, all the nitrate salts are soluble and the salts made with silver are not soluble. With this in mind, we will have a solid-state for and an aqueous state for  .

If this is true, the final answer can be B or C. The charge of Ag is +1 so the final answer is C.

I hope it helps!

wher is the rest of the question