Question

What are the rules for net ionic equations? I know you must follow the solubility chart, but I'm confused about the other aspects. When the compound is solid, gas or liquid, I don't break apart the compound right? Unless the compound is a strong acid and base? I already know the steps of finding the net ionic equation. I'm just not sure about the rules. So if you could provide an example for the different reactions, can you also include the differences when using the rules?

Answer 1

Solubility rules:

1. All Na+, K+, and NH4+ salts are soluble.

2. All NO3-, C2H3O2-, ClO3-, and ClO4- salts are soluble.

3. All Ag+, Pb2+, and Hg22+ salts are insoluble.

4. All Cl-, Br-, and I- salts are soluble.

5. All CO32-, O2-, S2-, OH-, PO43-, CrO42-, Cr2O72- and SO32- salts are insoluble. Except group IIA S2- and Ba(OH)2 are soluble.

6. All SO42- salts are soluble except CaSO4, SrSO4, and BaSO4 are insoluble.

Key steps:

- Determine the state of each substance in reaction (gas, liquid, solid, aqueous).

- Use the solubility rules to determine which of the ionic compounds are soluble in water.-

- Soluble ionics are identified with an (aq), insoluble ones with an (s). Most elements and covalent compounds are insoluble in water and should be shown with an (s), (l) or (g).

- Start with a balanced molecular equation.

- Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions indicate the correct formula and charge of each ion indicate the correct number of each ionwrite (aq) after each ion

- Bring down all compounds with (s), (l), or (g) unchanged.

Compounds in solid, liquid and gas state will remain undissociated.

Case 1. All substances are water soluble

Case 2. One reactant in solid phase and one product in gas phase.

Case 3. Reactants are water soluble and one of products is solid