What is the net ionc equation of the reaction AgNO3+Mgl2
The net ionic equation for the reaction AgNO3 + MgCl2 is:
Ag+ + Cl- → AgCl(s)
Mg2+ + NO3- → Mg(NO3)2
To determine the net ionic equation of the reaction between AgNO3 and MgCl2, we need to first write out the balanced molecular equation and then convert it into the net ionic equation by removing any spectator ions.
1. Write the balanced molecular equation for AgNO3 + MgCl2:
AgNO3 + MgCl2 → AgCl + Mg(NO3)2
2. Next, we need to determine which ions are spectator ions. These are the ions that appear on both sides of the equation without undergoing a chemical change. In this case, the nitrate (NO3-) and chloride (Cl-) ions are spectator ions.
3. Finally, we can write the net ionic equation by removing the spectator ions:
Ag+ + Cl- → AgCl
So, the net ionic equation for the reaction between AgNO3 and MgCl2 is Ag+ + Cl- → AgCl.
To determine the net ionic equation of the reaction between AgNO3 and MgCl2, we first need to write out the complete ionic equation.
1. Begin by writing out the reactants: AgNO3 and MgCl2.
AgNO3(aq) + MgCl2(aq)
2. Identify the ions present in the reactants:
AgNO3 dissociates into Ag+ ions and NO3- ions.
MgCl2 dissociates into Mg2+ ions and 2Cl- ions.
Ag+(aq) + NO3-(aq) + Mg2+(aq) + 2Cl-(aq)
3. Determine the products of the reaction:
The reaction will result in the formation of AgCl, which is insoluble in water, and Mg(NO3)2.
AgCl(s) + Mg(NO3)2(aq)
The net ionic equation is obtained by eliminating the spectator ions, which are ions that appear on both sides of the equation and do not participate in the reaction.
4. Removing the spectator ions gives us the net ionic equation:
Ag+(aq) + Cl-(aq) → AgCl(s)
The net ionic equation for the reaction between AgNO3 and MgCl2 is Ag+(aq) + Cl-(aq) → AgCl(s).