Question

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

Answer 1

C.
`Cl^−_(_a_q_) + Ag^+_(_a_q_)->AgCl_(_s_)`

Step-by-step explanation:

In this question our options are:

A.
`Ca^+^2_(_a_q_)+NO_3^-_(_a_q_)->Ca(NO_3)_2_(_a_q_)`

B.
`Ag^2^+_(_a_q_)+2Cl^-_(_a_q_)->AgCl_2_(_s_)`

C.
`Cl^−_(_a_q_) + Ag^+_(_a_q_)->AgCl_(_s_)`

D. None of the above because no reaction occurs

We have to remember that the ions produced by
`AgNO_3` are:

`Ag^+` and
`NO_3^-`

And the ions produced by
`CaCl_2` are:

`Ca^+^2` and
`Cl^-`

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

`AgCl` and
`Ca(NO_3)_2`

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
`AgCl_(_s_)` and an aqueous state for
`Ca(NO_3)_2_(_a_q_)`.

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!