Procedure 1:

1. Identify the mass of each reactant ion and the total mass of the reactants.

2. Identify the mass of each product and the total mass of the products.

3. Explain how this experiment confirms the Law of Mass Conservation.

Procedure 2:

1. Write a balanced molecular equation for the reaction of solid AgNO3 with aqueous NaCl. Be sure to include the correct coefficients and the state of the species (aq, s, l, or g).

2. Write the chemical equation as total ionic equation. Be sure to include the correct number of coefficients and the state of the species (aq, s, l or g).

3. Write the net ionic equation, including all physical states.

4. Identify the precipitate and the spectator ions. (See Textbook Sections 4.2 and 4.3).

5. If the chloride ion is usually soluble, how can solid AgCl form? Use the rules from Table 4.1 to discuss this.

Problems:

Using the Solubility Rules on page 143 in Table 4.1, write the balanced molecular, total ionic, and net ionic equations (including physical states) for the following:

Hints: There is no such thing as an Na3+. Na is in group 1A, so you know it can only form a +1 charge. It will form 3 Na+ ions for each Na₃PO₄.

There is a diatomic molecule Cl2. But when ionic compounds are dissolved in water, they form ions so the dissociation is to 2 Cl- from the MgCl₂.

1. Na₃PO₄ (aq) + MgCl₂ (aq) →

2. Al(CH₃COO)₃ (aq) + KOH (aq) →