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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

Respuesta :

Answer:

C. [tex]Cl^−_(_a_q_) + Ag^+_(_a_q_)->AgCl_(_s_)[/tex]

Explanation:

In this question our options are:

A. [tex]Ca^+^2_(_a_q_)+NO_3^-_(_a_q_)->Ca(NO_3)_2_(_a_q_)[/tex]

B. [tex]Ag^2^+_(_a_q_)+2Cl^-_(_a_q_)->AgCl_2_(_s_)[/tex]

C. [tex]Cl^−_(_a_q_) + Ag^+_(_a_q_)->AgCl_(_s_)[/tex]

D. None of the above because no reaction occurs

We have to remember that the ions produced by [tex]AgNO_3[/tex] are:

[tex]Ag^+[/tex]  and [tex]NO_3^-[/tex]

And the ions produced by [tex]CaCl_2[/tex] are:

[tex]Ca^+^2[/tex] and [tex]Cl^-[/tex]

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

[tex]AgCl[/tex] and [tex]Ca(NO_3)_2[/tex]

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 [tex]AgCl_(_s_)[/tex] and an aqueous state for  [tex]Ca(NO_3)_2_(_a_q_)[/tex].

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!

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