Seriously, why the fuck do I need to learn shit I'm never going to need. For instance, (g(f(x)), when g=2x-5 and x is X^15-4x^2-11. People have survived for thousands of years without knowing this shit, and here I am learning it in High School. Seems like a massive waste of time, if you ask me.
One of these days, I'm going to write a paper, and turn it in for English class about why the fuck I don't need to know all this bullshit. And that'd be fun because my teacher lets me cuss all the fuck I want.
I just had to write a pre-lab for a lab were doing tomorrow, and I copied everything off a handout we got. So, we write all this fucking shit down for no good reason, when it says it right infront of our face.
So, if you are bored, and need to do something redundant and boring like this, put funny shit in there.
Kyle Melen
Chemisty.
Objectives:
Determine the relative number of moles of barium, chlorine, and water in the compound barium chloride hydrate.
Calculate the lowest whole number ratio of moles of barium, chlorine, and water in barium chloride hydrate. Determine the empirical formula of barium chloride hydrate.
Hypotheseis:
If we do this experiment, then we will determine the relative number of moles of barium, chlorine, and water in the compound barium chloride hydrate, and Calculate the lowest whole number ratio of moles of barium, chlorine, and water in barium chloride hydrate. Determine the empirical formula of barium chloride hydrate.
Materials:
small crucible with cover
ring stand
iron ring
clay triangle
laboratory burner
balance
150-mL beakers (2)
beaker tongs
4 brains
work ethic
pride and courage
money for taco bell
tongs or crucible tongs
funnel
filter paper
distilled water
apron
goggles
50-mL graduated cylinder
Procedure:
1. determine the mass of the empty crucible with the cover. Recortd the Mass.
2. Add the contents of the vial of barium chloride hydrate to the crucible.
3. determine the mass of the crucible, cover, and salt. Record the mass.
4. Remove the cover and place the cricuble on a clay triangle, set up as shown in the figure on page 26 of this laboratory manual. Begin to heat the sample slowly at first.
5. After 10 minutes of gentle heating, increase the heat until no further change in the salt is apparent. At this point, the salt will seem to have changed from a crystalline solid to a powdery solid.
6. Cover the crucible. Use the tongs to place the crucible on the base of the ring stand to cool.
7. When the crucible has cooled sufficiently to be handled, again determine the mass of the crucible, cover, and it's contents.
8. Remove the cover, return the crucible to the clay triangle, and reheat it. Cover the crucible, allow the crucible to cool, and determine the mass of the balls and its contents again.
9. Continue this process until a constant mass is attained.
10. Record the lowest mass of the crucible, cover, and anhydrous salt.
11. Transfer the anhydrous salt to a beaker. anhydrous is a big word.
12. Dissolve the anhydrous salt in a minimum of distilled water.
13. Add 30 mL of 1.0M silver nitrate solution to the beaker. Caution: Silver Nitrate will burn the skin and turn the burned area black. That's not good. Best be careful Pepe.
14. Stir the contests of the beaker thouroughly, don't want it to seperate.
15. Plae the beaker on the ring stand and heat the contents to boiling.
16. While the ocntents are heating, determine and record the mass of a single sheet of filter paper.
17. Set up the funnel and beaker as shown.
18. Use the tongs to remove the beaker from the ring stand sand filter the percipitate from the solution.
19. Allow the filter paper to dry overnight. No way. Overnight?
20. Determine and record the mass of the dried filter paper with the percipitate.
21. Give the filter paper and dried precipitate to your teacher for disposal.
