Water is polar and has hydrogen bonds so it can dissolve polar and hydrogen bonded intramolecular molecules.
Substances that are not polar will dissolve substances that are not polar like gasoline and oil.
As we spoke about before, LIKE DISSOLVES LIKE!
Remember that solutions and mixtures are made possible by intermolecular bonding.
Dynamic Equilibrium: remember that the reactions are done, but they keep exchanging material. The ratio of products to reactants is now stable, it isn’t changing anymore.
Heterogeneous: Two different things are mixed, they can be separated by filtering or picking out. Mixture.
Homogeneous: Two or more things mixed together that can’t be visually seen as a mixture. Also known as solultions.
Suspensions: Heterogeneous mixtures where small particles of a solid are floating around in a liquid.

Colloids: Heterogeneous mixtures in which mixtures consist of two phases of matter that are stable and don’t settle out no matter how much time you give them.

Brownian motion is when the particles of the thing that’s dispersed are hit from all directions by the particles of the thing it’s dispersed in.
Because the particles of the thing that is dispersed are so small, they keep it
 from settling.
To be able to tell if a substance is a colloid is the Tyndall effect. When light shines through a colloid, you can see the rays of light as they travel though the solid because the suspended particles reflect/scatter it.
Solutions: Homogeneous mixtures, in which one material completely dissolves in another.

Solvent: The thing that does the dissolving.

Solute: The thing that gets dissolved.
How to tell if it is a solution? If you let it sit for a long time, nothing settles to the bottom. Additionally, it doesn’t experience the Tyndall effect
Concentration: Any measurement of how much solute is dissolved in a solution.

Unsaturated: More solute can be added to the solvent

Saturated: No more solute can be added to the solvent without it coming out of the solution

Supersaturated: More solute was added to the solvent than the solution usually can hold. Temperature has been increased or the pressure has been changed. These solutions are never stable, they will crystalize as soon as anything changes.

o Two ways of making them:
 Cool a saturated solution.
 Evaporate solvent from a saturated solution.

Notes for Dilutions on page 179
Molarity: moles of solute / liter of solution. This is the math that makes it possible to change the strength of a solution. 𝑚𝑜𝑙𝑒𝑠
= 𝑀 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦
𝐿𝑖𝑡𝑒𝑟
 What’s the molarity of a solution that contains 0.5 moles of
NaCl dissolved to make 1.5 L of solution?
 If I have 30 g LiOH dissolved in 300 mL of solution, what’s the molarity?
How to make a 5 molar solution of NaCl with 100 grams of water to start with and
1000 mls as your desired volume?
Dilutions:
1
1
2
2
o Example: If I add 25 mL of water to 5 mL of 0.15 M NaCl, what’s the final concentration of the NaCl solution? o Example: If I dilute 5 mL of 0.15 M NaCl solution to a final volume of 25 mL, what is the final concentration of the NaCl solution?

Honors: Stoichiometry with Molarity problems
If 525 mL of 0.80 M HCl solution is neutralized with 315 mL of Sr(OH)2 solution what is the molarity of the Sr(OH)2?
__ HCl + __ Sr(OH)2 __ SrCl2 + __ H2O
Step 1: balance the equation.
Step 2: switch the mls to liters for both volumes
Step 3: determine how many moles you have using the M=mole/L
Step 4: using mole ratio to determine the amount of moles you need for second species. (convert moles of HCl to moles of Sr(OH)2)
Step 5: divide the moles of the desired result by the volume in Liters.
Hint: always use the mole ratio if you have volume and molarity to switch species.
Solubility curve Table/Graph notes already given on Friday: Go over any misconceptions
Solutions= Homogeneous mixtures, in which one material completely dissolves in another.

Mixtures=suspensions (small particles are suspended of one substance are floating around in the other substance) and colloids (two phases of matter are mixed together) Brownian motion keeps them mixed, also Tyndall effect identifies them as a mixture rather than a solution.
Concentration is moles divided by liters. It is called Molarity. Also it is identified as saturated, unsaturated, or supersaturated.
Solubility curves are useful because below the line of any given substance is unsaturated, on the line is saturated, and above the line is supersaturated.
Dilution problems- moles, volume and Molarity is useful to dilute concentrated reagents to a more useful or desired concentration.
Honors and IB-
Stoichiometry problems with molarity- If you have grams of a substance and volume of any of the reagents one can find the concentration and the mass,
Molarity and volume of all of the other reagents. The math is a very useful tool in chemistry.