1. Write a balanced molecular equation for the reaction of solid AgNO3 with aqueous NaCl. Be sure to include the correct number of coefficients and the state of the species (aq, s, l or g).
2. Write the total ionic equation for this reaction, including all physical states.
3. Write the net ionic equation for this reaction, including all physical states.
4. Identify the spectator ions.
5. If the chloride ion is usually soluble, how can solid AgCl form? Identify the rules from Table 4.1 and explain the physical state of the products. (Be sure to discuss the exception to the chloride rule.)
Your other post under Kate should give you some hints on how to do this.
The spectator ions are the ionx that ARE NOT in the net ionic equation.
1. To write a balanced molecular equation, we need to first identify the reactants and products involved in the reaction. In this case, the reactants are solid AgNO3 (silver nitrate) and aqueous NaCl (sodium chloride). The products will be solid AgCl (silver chloride) and aqueous NaNO3 (sodium nitrate).
The balanced molecular equation for this reaction is:
AgNO3 (s) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
2. To write the total ionic equation, we need to separate all the aqueous compounds into their individual ions. In this case, AgNO3 will dissociate into Ag+ and NO3-, while NaCl will dissociate into Na+ and Cl-. The solid compounds, AgCl and NaNO3, will not dissociate since they are in their solid state.
The total ionic equation for this reaction is:
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) → AgCl (s) + Na+ (aq) + NO3- (aq)
3. To write the net ionic equation, we need to eliminate the spectator ions, which are ions that appear on both sides of the equation and do not participate in the actual reaction. In this case, the Na+ and NO3- ions appear on both sides of the equation, so they are spectator ions and can be eliminated.
The net ionic equation for this reaction is:
Ag+ (aq) + Cl- (aq) → AgCl (s)
4. The spectator ions in this reaction are Na+ and NO3-. They are present as both reactants and products in the total ionic equation but do not actively participate in the reaction.
5. The chloride ion (Cl-) is usually soluble and can typically form aqueous solutions. However, in this reaction, solid AgCl is formed. According to Table 4.1, chloride salts are typically soluble, but there are exceptions.
The exception to the chloride rule is when chloride ions are combined with silver ions (Ag+). Silver chloride (AgCl) is insoluble and forms a solid precipitate. This is because, in the presence of silver ions, the equilibrium shifts towards the formation of the insoluble silver chloride compound rather than staying in solution. Therefore, when solid AgNO3 reacts with aqueous NaCl, it forms solid AgCl.
The physical state of the products in the balanced molecular equation is solid AgCl and aqueous NaNO3, since they are both labeled accordingly.