Ionic Solubility

Dear period 8,

Today in class we did the Ionic Solubility lab. You were to observe the reactions of two compounds that either formed a reaction or not. After recording the data on the first page of the lab, we were to do the following pages according to the first page.

Homework: Finish lab, and finish problem #'s 3,4,5 from the Reaction Solubility 1 notes packet.

Thank you for reading my post, have a nice day.

a.v.

Solutions

Yesterday in class we finished our Mixtures Lab. We took each of the four mixtures and completed the evaporation test and went on to the filtrate lab. To fill out the back sheet of the paper, we can use the notes we took in class on Wednesday. If you want to check if you got the correct results, they are on moodle.
We also learned about solubility and dissolving. We learned that there are two categories of solutions: the solutes and the solvents.

Solutes:
-What is being dissolved
-Usually smaller amount

Solvents:
-What deos the dissolving
-Usually the greater amount

Ionic Compounds: When they are dissolved in water they split into ions (dissociation)
Covalent Compounds: When they are dissolved in water they do not split

*When the compounds are dissolved in water you change the subscrips to (aq), which means in water*

The homework is to finish the Mixtures Lab.
[The notes Mrs. Mandarino gave us in class are on moodle, in the notes section.
If you missed ChemDay, the make up assignment can be found in the homework log section on moodle.]

Mixtures

Homogeneous


The particles are evenly distributed

Heterogeneous

The particles remain thoroughly mixed throughout the mixture while the liquid is being mixed, but later settle to the bottom.



examples:

anything with "shake before use"

salad dressing

orange juice with pulp

children's medicine

* these are all known as suspensions



suspensions

after the particles settle out, the tyndall effect may be seen in the top liquid portion





Homogenous Mixtures

Solutions

are too small to reflect light or settle out
No tyndall effect
Examples:
Coke
Kool aid
Lemonade

Colloid
Are big enough to reflect light but not big enough to settle out.
Tyndall effect is seen

Examples:
milk solution


Today Mrs. Mandarino gave us our test back and our revised grade print outs. We began the new unit taking notes on mixtures. We learned there are two types of mixtures:


Kendall K
Mixtures

Limiting Reactants

 Limiting Reactant Strategy

If a problem mentions amounts of more than one reactant, its probably a limiting reactant problem.

1. Go from each reactant to amount of product (grams of each reactant to grams of product)
2. The reactant that produces the lower amount of predicted product is the limiting reactant.  This amount of product is also the amount that can be produced.
3. The other reactant is your excess reactant.

For Example:

Fe + S  à  FeS

If I have 28g of Iron (56 g/mol) and 24g of Sulfur (32 g/mol), how much FeS can be made and what is the limiting reactant?

28 g Fe  x  1 mol Fe  x  1 mol FeS  x  87.92g FeS  =  44 g FeS

                 55.85 g Fe     1 mol Fe       1 mol FeS

24 g S  x  1 mol S  x  1 mol FeS  x  87.92g FeS  =  66 g FeS

                32.07 g S     1 mol S         1 mol FeS

Fe is the Limiting reactant because it runs out first and produces less FeS.