My teacher showed us these examples in class, he says he need to be able to know when something is soluble in something else but i have no idea how to know. anyone have any rules on how to know?

This is the examples he gave us:
is CsI soluble in H2O? yes
is CH3OH soluble in H2O? Yes
is CH3OH soluble in NH3? Yes
is NaCl soluble in H2O ? yes
is C6H12O6 soluble in C6H6 ? No
is C6H12O6 soluble in H2O? Yes
is C6H6 soluble in C6H12? No
is CH3OH soluble in C6H6? No

... Please help i have a test soon. he says there will be other examples on test and not the ones above...

Generally, like dissolves like.

CsI is polar. H2O is polar. yes.
CH3OH has OH. H2O has OH. yes.
I think C6H6 (is that benzene?) will dissolve in C6H12 (is that hexene). Both are non-polar solvents.

i see, thanks for the help!

To determine if a substance is soluble in another substance, you need to understand some general rules and concepts. The solubility of a substance depends on the nature of both the solute and the solvent. Here are some guidelines to help you determine solubility:

1. "Like dissolves like": Substances with similar intermolecular forces are more likely to be soluble in each other. Polar solutes tend to dissolve in polar solvents, while nonpolar solutes dissolve in nonpolar solvents.

2. Ionic compounds: Ionic compounds, like CsI and NaCl, are often soluble in water (a polar solvent) because the solvent molecules can surround and stabilize the separated ions through ion-dipole interactions.

3. Small organic compounds: Small organic compounds, like CH3OH, are usually soluble in water because they can engage in hydrogen bonding with water molecules. Hydrogen bonding occurs when a hydrogen atom bonded to an electronegative atom (e.g., oxygen or nitrogen) is attracted to another electronegative atom.

4. Larger organic compounds: Larger organic compounds, like C6H12O6 (glucose), tend to be less soluble in nonpolar solvents like C6H6 (benzene) because their structures are dominated by nonpolar carbon-carbon and carbon-hydrogen bonds.

Based on the examples provided, here are the conclusions for each case:

- CsI is soluble in H2O because it is an ionic compound and water is a polar solvent.
- CH3OH is soluble in H2O because it can form hydrogen bonds with water molecules.
- CH3OH is soluble in NH3 because both substances are polar and can engage in hydrogen bonding.
- NaCl is soluble in H2O for the same reasons as CsI.
- C6H12O6 is not soluble in C6H6 because both substances are nonpolar.
- C6H12O6 is soluble in H2O because it can form hydrogen bonds with water molecules.
- C6H6 is not soluble in C6H12 because both substances are nonpolar.
- CH3OH is not soluble in C6H6 because both substances are nonpolar.

Remember, these rules can be used as general guidelines, but there may be exceptions based on specific cases. It would be beneficial to review and understand the concepts of intermolecular forces, polarity, and hydrogen bonding to apply these rules effectively. Additionally, you can consult reference materials such as solubility tables to learn more about specific solubility patterns.