Wednesday, May 30, 2007

Today's class was comprised of a lab, "Determining the Percent of Acetic Acid in Vinegar." By determining the certain data from the two titrations, we'll figure out the percentage. I'm not too sure how right now, but probably tomorrow. Oh, don't forget to do the Pre-lab, I'm pretty sure we have to do it. For those who weren't present, the lab was quite easy. That's all i guess. (okay this isn't the "best" post, but I tried)
Jennie to scribe for Thursday

Monday, May 28, 2007

Monday: Finally Ms. K is here.
the topic for the day is about Acid and Base Dissociation Constant.
Acid Dissociation Constant:
- strong acids/base dissociate completely :. do not establish equilibrium
- if Ka > 1 = strong acid
- weak acids/base - establish equilibrium
- The equilibrium law: Ka= [H₃O⁺][A^-] / [HA]
-the Ka reflects the equilibrium that exists for as acid

Kb=[B⁺][OH^-] / [BOH]

-the larger the Ka/Kb, the stronger the acid/base.
-the smaller the Ka/Kb, the weaker the acid/base.

that's about it.

note: June 1, due date of research project

: )

Scribe Post.

Okay, today we went over the work sheet called Ionization Equations and Constants, that was given to us on Monday, the answers are as follows:

1.If they have more than one Hydrogen, there will be more ionization equations.
2.The Ka decreased as you go down the list
3.HCO₃^- is weaker because its Ka is smaller than H₂PO₄^-.
4. phosphorous <-> H⁺ + H₂PO₃^-, phosphorous - 1H <-> H + HPO₃, phosphorous - 2H <-> H + PO₃.
5.
a) Ka=[H][HCl]/[H₂CO₃]
b) Ka=[H⁺][HCOO^-]/[HCOOH]
6. because it's a 1 to 1 ratio.

also we are to do questions 6 to 15 by tomorrow.
next scribe is "romina".

Ka Problems

May 23, 2007

Okay, so today for class, we had a sub ... Mr. Newman. Yeah, all we basically did was review that "mini-booklet" Ms. Kozoriz gave to us about a week ago. I'm not sure what it's called, but it had the information about Arrhenius and Bronsted-Lowry and their definitions of acids and bases.

We also went over the Kw problems that was assigned to us last Thursday I think?

Yeeah, thats pretty much it, and I think we're having Mr. Newman again as a sub since he kept saying "tomorrow I'm going to go over ..." yeah but I'm not sure.

Anyway, the next scribe can be SERGIO.

May 22 LAB

well hello there fellow chemistry people. im here to scribe on todays class..
k so today we did an awesome lab...it was very colorful and fun :) haha. but yeea. the lab showed us the pH level of acids and bases...i think. but yeea then Ms.K handed out a booklet .."GR 12 chem acids and bases" - read it over and yeea that was all for todays class... next scribe will be...kayyy

May 16th

I can't remember exactly what we did last thursday..all I can remeber is that Ms.K gave us our test papers back and corrected it and did some questions about Acid and Bases..Oh and the job fair,I got a free pen yay!..sorry for the last post...the next scribe is BOOT5

Assignment on B-L and Arrhenius Acids/Bases

Arrhenius Acids and Bases

Acids and bases

Today was a test day so we really didn't do much so I won't have much to say during this post. As many of you will know the next section seems to be on acids and bases. Some points which can be found in the text are the pH concept which includes the method of finding the pH of acid and base solutions by way of calculations. Another set of information you might need to know will be the names of the researchers/scientist who contributed their theories into the research of acids and bases. Actually that might be all at the moment so really all I can say is to remind everyone to get pages 431 to 452 read and to get the question done.

The next to scribe today will be vehcsur.

Solubility Problems...

Uhhmm today it was supposed to be jennie who will scribe,but she skip...opppsss... haha so i decided to scribe today...

well we didn't do that much we just

answered the Solubility Equilibria Assignment No. 3 and it's pretty much straightforward..we did this one over the past few days...

and also Ms K. gave us a hand out and it's all about using solubility Product Constants,it is all about the Ksp of each compounds.There`s the Compound and its Ksp.So for those of you who were absent today,guess what!

we will be having our quiz tomorrow and don`t forget to review o.k.!!!!see yah the next scribe would be phoebe..something,it's sean

Common Ion Problems #2

May 10: Thursday's Scribe

On Thursday, we had a work class, and we had to finish our labs and answer the 4 questions from the yellow booklet.
and that's about it ;)

SOLUBILITY & COMMON IONS!

Today class we went over the rest of the Chemical Equilibrium booklet that Ms. K handed out last weeek, started from page 3. We did the examples 4 and 5 for "Solubility" and examples 1, 2, and 3 for "Common Ions"! So for those who weren't in class, Ms. K had posted the steps of the solutions in the slide show below. It's pretty much about finding the Ksp and the concentrations of each ion, but in different cases, where we might have initial concentration for one of the ion. And if you have any questions, or dont understand the steps, please ask Ms. K?!?! Other than that, the test has moved to Tuesday, which is yay for those who are lazy to study in the weekend! And that's about it. Homework will be Assignment # 3, question from 1-3!

And the next scribe will be keith!!

Common Ion Problems, Ksp

Assignment 1 Ksp Problems

Equilibium Review Day

Friday's class was mostly about reviewing for Monday's test. We started by correcting some of the questions for Chapter 18- Chemical Equilibrium. Then we went over the questions from Worksheet 20- Determining Equilibrium. Near the end of class we reviewed for tomorrow's test. Remember everyone the two factors needed for equilibrium are: a closed system and constant temperature. This is a certain question that is worth four marks. Yea free marks! Alright, everyone study hard and good luck!! =D

The next scribe is... jess.

Equilibrium Review for Test

Ch.18.2 Equilibrium Study Guide

The Haber process

To recap on what we've done today for those who might or might not remember as usual we went over the corrections for the equilibrium worksheets, this includes the reactant or product concentration graph and the state of dynamic sheet. That being said there really isn't much more to do then to give a summary on the "Haber Process". During the late nineteenth century it seemed that both North America and Europe begun to run out of edible crop and found that their soil just wasn't cutting it, so what could be done, simple (or not depending on your knowledge on farming) by adding to the soil a nitrogen-based fertilizers. Now for those who might not know plants have a tendency to use nitrate to promote protein formations and other plant benefiting functions. This was a good idea, however nitrogen was used in development of explosives, and with all the fighting going on a lot needed to be used . That's about when a German professor named Fritz Haber found a way to oxidize ammonia created from nitrogen to make nitrates and nitrites required for the production of nitrate fertilizer. The process went more or less as followed, he took nitrogen gas and hydrogen gas placed them in a closed container with a iron oxide catalyst, raised the temperature to 500 Celsius with a pressure of 40 MPa, the end result is a product yielding about 40% ammonia. That's about the general description of the Haber process created by Fritz Haber, that's Fritz Haber and for reference sake Le Chatelier, have those memorized? That's all I have to say so read this or the sheet, which ever is clearer and keep them in mind.

Today's daily reminders include- Review pages have them done! (or not)
Test on Monday. (doubt anyone will forget though)
I'm feeling a bit tired so I'll chose crystal as the next scribe being at the top of the list.(not that I have much of a selection).

Ch.18 Review Chemical Equilibrium

May 02, 2007

What we did in class today:
[+] Corrected Chapter 19 Worksheet
[+] Chemical Kinetics Test was given back
[+] Worksheet on Concentration vs. Time Graph
was handed out
[+] Chapter 18 Chemical Equilibrium
Worksheet was given to work on


We didn't really do much lesson today, but the
Concentration vs. Time Graph was explained.

* However, here are some things that we should remember!

- When the system is initially at equilibrium & a stress is added, after an instantaneous change, the system will allow to reestablish equilibrium.

- When reaction is at equilibrium, the concentration of both reactant and product are constant.

- When more reactant is added, the concentration of the reactant increases immediately. As the reactant is consumed in the reaction, its concentration decreases to a constant value. Therefore, more product is formed and the concentration of the product increases to a new constant value, which reestablish a new equilibrium position.

- When a reactant is removed, the concentration of the reactant decreases immediately. As more reactant is being produced its concentration increases to a new constant value. Therefore, the product can no longer be form at the same rate, so the concentration of the product decreases to a new constant value, which reestablish a new equilibrium position.

- Also remember that when adding a catalyst, it does not speed up the reaction, but stays unchanged.
Tomorrow's scribe is Sean.

Ch.19 Worksheet

Disrupting Equilibrium Systems

In this morning in grade 12 chemistry class we have done an interesting lab. The main purpose of the lab is to describe Le Chatelier's principle the effect that applying various types of stress will have on the position of equilibrium.These stresses include changes in such factors as concentrations of reactants or products, temperature of the system for reactions involving gases,pressure. This lab is due tomorrow.
Crystal is the scribe for tomorrow

THURSDAY'S SCRIBE

Hey guys excuse the late scribe, no net for me. On Thursday, most of you know we had somewhat of a review. In the beginning we were all "reminded" of what equilibrium was. IT IS WHEN THE RATE OF THE FORWARD REACTION = THE RATE OF THE REVERSE REACTION.

Necessities Include;
- must be a closed system
- applies only to a gas and aqueous reactions
- reversible
- dynamic
- rates are equal

That same day, we received a handout on Le Chatelier's Principle. remember he stated that "WHEN A SYSTEM IS SUBJECTED TO STRESS, THE SYSTEM WILL ADJUST SO AS TO RELIEVE THE STRESS." Also, there were various "rules" to follow to figure out if the product or reactant was favoured. Some factors included changing concentration, pressure changes and temperature changes. Don't forget what we were reminded several times, "TEMPERATURE IS THE ONLY FACTOR WHICH WILL CHANGE THE VALUE OF KC" Also, something tricky, adding a catalyst to a system, lowers the activation energy of both the forward and reverse reaction equally thus it will not effect the equilibrium position. Although, if it wasn't at equilibrium the catalyst would make the system reach equilibrium much faster.