Question

Show the complete ionic and net ionic forms of the following equations. If all species are spectator ions, please indicate that no reaction takes place. Note! You need to make sure the original equation is balanced before proceeding! A set of solubility rules are given at the end of this document.

AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)

Answer 1

To write the complete ionic equation of the reaction between AgNO3 and KCl, first balance the equation. Then, separate the dissolved ionic compounds into their respective ions to get the complete ionic equation. Finally, remove the spectator ions to obtain the net ionic equation.

Step-by-step explanation:

To write the complete ionic equation of the reaction between AgNO3 and KCl, we first need to balance the equation:

AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)

Next, we can write the complete ionic equation by separating the dissolved ionic compounds into their respective ions:

Ag+ + NO3- + K+ + Cl- → AgCl(s) + K+ + NO3-

In the complete ionic equation, the spectator ions (K+ and NO3-) appear unchanged on both sides of the equation. The net ionic equation can be obtained by removing the spectator ions:

Ag+ + Cl- → AgCl(s)