Let Chemistry Absorb You. Ha.

Alright, boys and girls, this here's a chemistry post and it's about to get real.

Mr. Lieberman reviewed the test with us, like a boss, and gave us two points because of an error and because of leniency. Then he reviewed with us the basic principles of solutions.

• A solute is the substance that is being dissolved
• A solvent is the liquid in which the solute is dissolved
• Solute dissolves in solvent
• Aqueous = solution with water as solvent

Easy, right?

A saturated solution is a solution where the solute has dissolved into it at a maximum. No more solute can be dissolved in this saturated state.

In the notes that Mr. Lieberman explained in class, there is a diagram of NaCl dissolving in H2O showing the driving forces that cause the dissolving of this solute, NaCl, into this solvent, H2O (most of the solvents in this unit will be H2O and all of them will be liquids! Awesome!). In the diagram, the H2O molecules, which are polar, attach themselves to the Na+ or Cl- atoms according to polarity. So an H2O molecule's negative pole will attach to the positive Na atom. And an H2O molecule's positive pole will attach to the negative Cl atom. This will pull the crystal-like structures of NaCl apart. This is a demonstration of an ionic solute dissolving by dissociation into its ions. There are two more types: Covalent solutes dissolving by H-bonding to water and covalent solutes dissolving by London dispersion forces (LDF).

This process is carried out instantaneously, it cannot be viewed through a microscope or observed at all, for that matter.

Furthermore, there are three stages to this same solution process explained in further detail here.

1. Primarily, there is the separation of a solute, and in order of this to happen, the solute's molecules must surpass their intermolecular forces (IMF) and it requires energy, making it endothermic.
2. Secondly, the separation of a solvent occurs when the solvent overcomes its intermolecular forces. This also requires energy, also making it endothermic.
3. Thirdly, the interaction of these two substances occurs. An attractive bond forms between the solvent and solute molecules and this releases energy, making it exothermic.

Phenominal! Now we understand the heat exchanges that occur within this process, let's continue!

We continued with the in-class notes and took a look at the factors affecting the solubility.

We know that Like dissolves like, which means that molecules with the same type of intermolecular forces will dissolve in eachother. E.g. dipole-dipole, Hydrogen bonds, and LDF.

Cool, huh?

Tell you what's not cool, that the raise of temperature in these solutions causes more collisions which allows easier access into these crystal structures, allowing for further saturation of a solution.

Finally, there is pressure. Solids and liquids are hardly affected by pressure changes in relation to solutions, but gas, under higher pressure, will have a higher solubility.

Well done, Captain, you have successfully acquired knowledge of solutions and can continue on your path to success. Enjoy your good HEALTH:

The next scribe is Becky N. (Rebecca N.)