Net Ionic Equations

Date: November 2nd, 2012
Homework: Net Ionic Equations Worksheet

On Friday, we learned how double replacement reactions occur in water. Also, we learned how to write molecular equations in the form of ionic and net ionic equations.
The following reaction takes place in water:

AgNO_{3 (aq)} + NaCl _(aq) AgCl _(s) + NaNO_{3 (aq)}

_{AgCl is the precipitate formed in the solution.}

_{When the reaction occurs the soluble compound (NaNO3) is broken down into its ions (Na+ and Cl-).}

_{The ionic formula of this reaction is:}

Ag⁺ + NO₃^- + Na⁺ +Cl^-  AgCl _(s) + Na⁺ + NO₃^-

AgCl would remain in its compound form since it was formed as a precipitate.The rest of the products, if are soluble, would remain in their ionic form. In this reaction, not all the ions reacted. NO₃^- & Na⁺ did not combine to form a compound.

Therefore, the net ionic equation, an equation with only the reacting ions, is:

Ag⁺_(aq) + Cl^-_(aq) AgCl _(s)

                                                   Silver nitrate and sodium chloride are put into water.

                                         When inside the water, both compounds break into their ionic forms.

The silver and chloride ions react to form a precipitate. While the nitrate and sodium ions remain in the ionic form and don't react.

THE NET SCRIBE WILL BE.............. JOSH M.