I need some help to answer my chemistry lab

Written Assignment:

Procedure 1

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

• Identify the mass of each product and the total mass of the product.

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

Procedure 2

• 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).

• Write the total ionic equation for this reaction, including all physical states.

• Write the net ionic equation for this reaction, including all physical states.

• Identify the spectator ions.

• 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.)

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.

• Na3PO4 (aq) + MgCl2 (aq) →

• Al(CH3COO)3 (aq) + KOH (aq) →