Continuations...

...For Abel and Anthony, your job is to catch up on last week's homework, so scroll down...  and for everyone else, it is to make sense of last week's homework, so keep plugging on.

Specifically, choose 6 or more reactions from the lab that produced a precipitation, and write out (for each equation)  the balanced molecular equation, with the (aq) and the (s) as needed,  the ionic equation, and the net ionic equation. Make sure you balance the charges when you write down the products.  And then write down why you think which compound is the precipitate, according to the solubility rules on page 218 (Table 8.1 or Figure 8.3)  in your textbook.  For example: "Most nitrate (NO3-) salts are solulble. Most hydroxide compounds are only slightly soluble, expections are sodium, potassium  and calcium."
In summary, for six reactions of your choosing:

1. Balanced molecular equation
2. Ionic equation
3. Net ionic equation
4. Solubility rule applied

The tricky bit might be to consider which elements combine to form the precipitate.  Your textbook section 8.2 and 8.3 will help you, particulary the solubility rules. You may also review the videos from last week's homework. (Don't be confused:  precipitates are solid because they are insoluble!  and ions are aqueous/soluble because they are dissolved in the solution.)

You may also review the videos from last week's homework, as needed.