Precipitation Titration of CoCl2 with NaOH

Question

How to tackle the following questions:

1. "Calculate the moles, and mass (theoretical yield), of the precipitate that you were expecting to collect based on the product being Co(OH)2. Again, if you cannot figure out where to start, create an arrow diagram, like the one in Figure 2 (not required). Provide the dimensional analysis statements showing the cancelling of all units throughout in either multi step-by-step statements or the one-line statement."
2. As it turns out, the product of your reaction is not pure Co(OH)2 but is a “hydrate” with the chemical formula Co(OH)24H2O and a molar mass = 164.95 g/mol. Use the number of moles of product you calculated in the previous question to calculate a more accurate theoretical yield (mass) based on the Co(OH)24H2O product.
3. For the precipitation between CoCl2 and NaOH, write the overall balanced, total ionic, and net ionic equations. Make sure you show all phase labels (s) (l) (g) or (aq).

Overall Balanced Equation:

Total Ionic Equation (circle and cancel the spectator ions):

Net Ionic Equation:

Answer 1

3.) Overall, total ionic and net ionic equations including phases:

CoCl₂(aq) + 2NaOH(aq) ==> Co(OH)₂(s) + 2NaCl(aq) .. balanced equation

Co²⁺(aq) + 2Cl-(aq) + 2Na⁺(aq) + 2OH^-(aq) ==> Co(OH)₂(s) + 2Na⁺ + 2Cl^- .. total ionic equation

Co²⁺(aq) + 2OH^-(aq) ==> Co(OH)₂(s) .. net ionic equation

1.) Not enough information provided to calculate moles of Co(OH)₂. We need to know amount of NaOH that was added (volume and molarity, or number of moles at least)

2.) Not enough information since we need the answer to #1 in order to answer #2.