In the beginning of the class, Ms. K showed us an animation about redox. To review this animation, click here:)...
After the animation, Ms. K went over Section 20.2 of OXIDATION-REDUCTION REACTIONS worksheet that the sub gave us. If you missed the class or simply wants to see the answers again, check the slideshow below.
Ms. K then started a new lesson about BALANCING USING OXIDATION METHOD. (note. this lesson is not on the yellow booklet).
To balance using the oxidationnmethod, we have to follow these steps:
STEP 1. DETERMINE THE OXIDATION NUMBERS.
STEP 2. DETERMINE THE NUMBER OF ELECTRONS TRANSFERRED PER ATOM/ION FROM THE CHANGED IN THE OXIDATION #s.
STEP 3. DETERMINE THE # OF ELECTRONS TRANSFERRED PER MOLE FROM THE SUBSCRIPT IN THE CHEMICAL FORMULA.
STEP 4. MAKE THE # OF ELECTRONS LOSS = # OF ELECTRONS GAINED BY FINDING THE SIMPLE COEFFICIENTS TO BALANCE THE # OF ELECTRONS TRANSFERRED.
STEP 5. BALANCE THE EQUATION AS YOU NORMALLY WOULD.
To see examples for each of these steps, pls see Ms. K's slideshow below....
We then answered SECTION 20.3 , # 1 question. Ms. K went over the answers for letters A to D, and can also be found in the slide show below...
IMPORTANT
TEST will be on TUESDAY. If you missed the class, dont forget to ask Ms K for the review worksheet she gave us, STUDY GUIDE, REDOX REACTIONS.
Thats it for this day..merci:) HAVE A NICE LOONG WEEKEND ^_ _ _ _^
the next scribe is...ASHLEY:)
Saturday, February 28, 2009
Thursday, February 26, 2009
Wednesday, February 25, 2009
Redox Continued
February 25, 2009
Finally I've joined this darned blog but yeah. Moffatt picked me to scribe today knowingly I had other stuff to do like sleep. Anyways, here's the following things we've done in class.
1. We were shown an experiment between Aluminum paper and an acid. As shown in class, the Aluminum broke down into a red-ish color from it's original silver color prior to being placed into the acid.
2. Corrected page 14 in our yellow "Grade 12 Chemistry Aqueous Reaction" booklet.
I honestly would have put the answers down but I didn't accomplish to copy them in class. Sorry about that.
3. Lastly, we were assigned Section 20.2 (1-4) on the handout sheet "Oxidation - Reduction Reactions" given out last week by Ms. Hall. ( I think )
Anyways, I have no idea who to pick to scribe for tomorrow but we'll see what comes up.
- Tony
Finally I've joined this darned blog but yeah. Moffatt picked me to scribe today knowingly I had other stuff to do like sleep. Anyways, here's the following things we've done in class.
1. We were shown an experiment between Aluminum paper and an acid. As shown in class, the Aluminum broke down into a red-ish color from it's original silver color prior to being placed into the acid.
2. Corrected page 14 in our yellow "Grade 12 Chemistry Aqueous Reaction" booklet.
I honestly would have put the answers down but I didn't accomplish to copy them in class. Sorry about that.
3. Lastly, we were assigned Section 20.2 (1-4) on the handout sheet "Oxidation - Reduction Reactions" given out last week by Ms. Hall. ( I think )
Anyways, I have no idea who to pick to scribe for tomorrow but we'll see what comes up.
- Tony
Wednesday, February 25th
At the beginning of class, Mrs. K handed our titration lab back. When doing labs, she reminded us to do what has been asked, like stating the purpose of the lab, the qualitative observations of the substances involved, and the calculations of how we got our answers.
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We also reviewed what a Redox Reaction is and the definition of an Oxidation Reaction and a Reduction Reaction.
A Redox Reaction is a reaction wherein oxidation and reduction occur at the same time.
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Next up, Ms. K showed us an experiment involving a Redox Reaction where:
The aluminum lost electrons and the copper gained electrons.
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For the remainder of the class, we worked on the questions in the booklet and the worksheet as practice for determining the oxidation number of atoms; and indicating the element reduced, the element oxidized, the oxidizing agent, and the reducing agent.
The next scribe will be MARIE :)
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We also reviewed what a Redox Reaction is and the definition of an Oxidation Reaction and a Reduction Reaction.
A Redox Reaction is a reaction wherein oxidation and reduction occur at the same time.
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Next up, Ms. K showed us an experiment involving a Redox Reaction where:
- She added copper (II) chloride to a beaker of water.
- Because of that, the water turned blue-green.
- She got a piece of crumpled aluminum foil and placed it inside the beaker.
- After a few minutes, the aluminum started to have a dark orange colour and it little by little dissolved away.
The aluminum lost electrons and the copper gained electrons.
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For the remainder of the class, we worked on the questions in the booklet and the worksheet as practice for determining the oxidation number of atoms; and indicating the element reduced, the element oxidized, the oxidizing agent, and the reducing agent.
- An oxidized element increases its oxidation number because it loses electrons.
- A reduced element decreases its oxidation number because it gains electrons.
- An oxidizing agent is a chemical compound contains the atom that gains electrons in a redox reaction.
- A reducing agent is a chemical compound that contains the atom that loses electrons in a redox reaction.
The next scribe will be MARIE :)
Tuesday, February 24, 2009
Friday's class
Sorry for prolonging this blog for Friday, but as they say "better late than never". Friday was a breeze all we did was finish our titration lab. We didn't do much more than that, so there you go.
Tuesday, February 24th add on
Just to add on to what MsK.s slide show, we also had to answer questions from the Aqueous Reactions Booklet, numbers 1-17 on pages 13 and 14. We also got two worksheets from Ms. Hall that we were supposed to do (even though we didn't understand her explanations) so they would be good practice. Even though I am not scribe for today i guess i will pick dangerfield for next scribe.
Wednesday, February 18, 2009
Reminder: Test Tomorrow!!!
T O D A Y' S C L A S S!
Binary Acids: have 2 elements. For ex. HBr and HCl
Monoprotic Acids: have one hydrogen atom HCl
Diprotic Acids: have two hydrogen atoms H2SO4
Triprotic Acids: have three hydrogen atoms H3PO4
Oxyacids: have one hydrogen, one oxygen, and one other element
Naming Acids
* Hydrogen _____ide --> Hydro _____ic Acid
* Hydrogen _____ate --> __________ic Acid
* Hydrogen _____ite --> __________ous Acid
Examples:
*H + Cl --> Hydro chloric Acid
*H + SO4 --> Sulfuric Acid
*H + SO3 --> Sulfurous Acid
Naming Bases
Name of the positive ion + hydroxide(OH) on the end
Examples:
Mg(OH)2 Magnesium + hydroxide = Magnesium Hydroxide
NaOH Sodium + hydroxide = Sodium Hydroxide
H A N D O U T S
Worksheets: Formulas of Common Acids and Ternary Nomenclature: Acids and Salts
Notes : Neutralization Reactions- sums up todays work and notes in class well
A N S W E R S
These are the answers to today's problems done in class.
Formulas of Common Acids
4-1
LAB IS DUE FRIDAY AND FIRST TEST IS TOMORROW!
Test:
Aq reactions,
Solutions,
Neutralization,
Yellow booklet,
Note: In the beginning of the semester we received a yellow handout
called "Grade 12 Chemistry Outcomes".
The test will include the first 5 objectives.
- Ms K. handed back our Neutralization problems worksheet that was due TUESDAY!
- Discussed naming Acids and Bases.
- Received handouts.
- Went over the answers to the problems done in class.
Binary Acids: have 2 elements. For ex. HBr and HCl
Monoprotic Acids: have one hydrogen atom HCl
Diprotic Acids: have two hydrogen atoms H2SO4
Triprotic Acids: have three hydrogen atoms H3PO4
Oxyacids: have one hydrogen, one oxygen, and one other element
Naming Acids
* Hydrogen _____ide --> Hydro _____ic Acid
* Hydrogen _____ate --> __________ic Acid
* Hydrogen _____ite --> __________ous Acid
Examples:
*H + Cl --> Hydro chloric Acid
*H + SO4 --> Sulfuric Acid
*H + SO3 --> Sulfurous Acid
Naming Bases
Name of the positive ion + hydroxide(OH) on the end
Examples:
Mg(OH)2 Magnesium + hydroxide = Magnesium Hydroxide
NaOH Sodium + hydroxide = Sodium Hydroxide
H A N D O U T S
Worksheets: Formulas of Common Acids and Ternary Nomenclature: Acids and Salts
Notes : Neutralization Reactions- sums up todays work and notes in class well
A N S W E R S
These are the answers to today's problems done in class.
Formulas of Common Acids
- HF
- HNO3
- H2SO4
- H3PO4
- H2CO3
- CH3COOH or HC2H3O2
- H2OOCCOO
- HBO3
- H2SiO3
- HClO3
4-1
- Iodic Acid
- Sodium Bromate
- Calcium Phosphate
- Periodic Acid
- Iron (III) Iodite
- Hydroastatic Acid
- Benzoatic Acid
- Mercuty (I) Hypoiodite
- Phosphorous Acid
- Ammonium Bromate
- H2C4H4O6
- Ca(ClO)2
- T2Te
- Cu(NO3)2
- H2CO3
- HiO
- HOCN or HCNO
- H2C8H4O4
- Sn(CrO4)2
LAB IS DUE FRIDAY AND FIRST TEST IS TOMORROW!
Test:
Aq reactions,
Solutions,
Neutralization,
Yellow booklet,
Note: In the beginning of the semester we received a yellow handout
called "Grade 12 Chemistry Outcomes".
The test will include the first 5 objectives.
Tuesday, February 17, 2009
I DIDN'T KNOW
Hello.I didn't realize I was the scribe for today but oh wells.
So anyways what we did in class today was we hand in our worksheet that was due today the "Neutralization Problems."
Next what we did in class was a Lab. The Lab was called, "Titration Lab."
So anyways what we did in class today was we hand in our worksheet that was due today the "Neutralization Problems."
Next what we did in class was a Lab. The Lab was called, "Titration Lab."
- What we did was we measured out 1.0 mL of distilled water into a 10 mL graduated cylinder. Must repeat 3 times to get an accurate result.
- After that was done, we had to measure out 5 mL of distilled water into the graduated cylinder and then place that amount into a 50 mL beaker. And after we added a DROP of PHENOLPHTHALEIN INDICATOR. And swirled it a bit.
- Next we took H2SO4 (SULFURIC ACID) and added 20 DROPS into the beaker and then transfered that solution into the graduated cylinder to measure the volume. Then we placed it back into the beaker.
- Next we then took NaOH (SODIUM HYDROXIDE) and had to COUNT the NUMBER OF DROPS that made the solution in the beaker to a permant pink color.
- Then we place that solution back in the graduated cylinder and measure the volume of that solution.
- After that was done, we cleaned out the equipment and did that lab again 2 more times so we can get an accurate result
- And after we cleaned out the equipment and cleaned up.
And that was pretty much what we did in class today. No notes, no homework (unless you didn't finish the other assignments.), and that was all. =D
So the next scribe for tomorrow will be : KAYLA =D
Monday, February 16, 2009
hi~o(*∩_∩*)o~everybody
Hi~~o(*∩_∩*)o
On friday we corrected page 9 the problems 1 to 9 . . .
Here the answers : . . .
1. NaOH + HNO3 NaNO3 + H2O
mol NaOH = 0.20 mol /1 * 1 = 0.20 mol
2. HCl + KOH H2O + KCl
x (0.45 mol/L) = 25.0 mL (1.00 mol/L)
x = 56 mL
3. a) HCl + NaOH H2O + NaCl
mol HCl = 0.20 mol / 1 * 1 = 0.20 mol
b) 2HCl + Ca(OH)2 2H2O + CaCl2
mol HCl = 0.10 mol /1 * 2 = 0.20 mol
4. HCl + NaOH H2O + NaCl
28.0 mL / 1000 = 0.028 L
mol HCl = 0.028 L (1.00 mol/L) = 0.028 mol
20.0mL / 1000 = 0.020 L
C NaOH = 0.028 mol / 0.020 L = 1.40 mol/L
5. End point - when performing a tritration the standard is added until one drop permanently change the colour of indicator.
Equivalence point - As the two solution are mixed, the system will reach a point at which the acid and base will have neutralized one another.
- The point at which the number of mole of acid are equivalent to the number of moles of base.
6. C NaOH = x (43.0 mL) = 32.0 mL (0.100 mol/L)
x = 0.0744 mol/L
7. C NaOH = x (40.0 mL) = 25.0 mL (0.120 mol/L)
x = 0.075mol/L
8. C KOH = x (50.0 mL) = 30.0 mL (0.250mol/L)
x = 0.15 mol/L
9. mol of acid = 25.0 mL / 1000 * 1.44 mol/L = 0.036 mol
mol of base = 36.0 mL / 1000 * 2.00 mol / L =0.072 mol
Acid must be diprotic ( the base has one OH ion molecules and twice as many moles of base are required to neutralize the acid)
And don't forget to do the worksheet~~
The next scribe Rawra
o(*∩_∩*)o
On friday we corrected page 9 the problems 1 to 9 . . .
Here the answers : . . .
1. NaOH + HNO3 NaNO3 + H2O
mol NaOH = 0.20 mol /1 * 1 = 0.20 mol
2. HCl + KOH H2O + KCl
x (0.45 mol/L) = 25.0 mL (1.00 mol/L)
x = 56 mL
3. a) HCl + NaOH H2O + NaCl
mol HCl = 0.20 mol / 1 * 1 = 0.20 mol
b) 2HCl + Ca(OH)2 2H2O + CaCl2
mol HCl = 0.10 mol /1 * 2 = 0.20 mol
4. HCl + NaOH H2O + NaCl
28.0 mL / 1000 = 0.028 L
mol HCl = 0.028 L (1.00 mol/L) = 0.028 mol
20.0mL / 1000 = 0.020 L
C NaOH = 0.028 mol / 0.020 L = 1.40 mol/L
5. End point - when performing a tritration the standard is added until one drop permanently change the colour of indicator.
Equivalence point - As the two solution are mixed, the system will reach a point at which the acid and base will have neutralized one another.
- The point at which the number of mole of acid are equivalent to the number of moles of base.
6. C NaOH = x (43.0 mL) = 32.0 mL (0.100 mol/L)
x = 0.0744 mol/L
7. C NaOH = x (40.0 mL) = 25.0 mL (0.120 mol/L)
x = 0.075mol/L
8. C KOH = x (50.0 mL) = 30.0 mL (0.250mol/L)
x = 0.15 mol/L
9. mol of acid = 25.0 mL / 1000 * 1.44 mol/L = 0.036 mol
mol of base = 36.0 mL / 1000 * 2.00 mol / L =0.072 mol
Acid must be diprotic ( the base has one OH ion molecules and twice as many moles of base are required to neutralize the acid)
And don't forget to do the worksheet~~
The next scribe Rawra
o(*∩_∩*)o
Thursday, February 12, 2009
Aqueous Reactions Unit
Hi...Classmates^_^
Yup.. I'm your scribe for today's class...Let's get started
Today, Mrs. Kozoriz corrected page 6 and 7 from the booklet the one that assign as to do for homework yesterday
"Calculating an Unknown Concentration"
Page 6...
Calculate the concentration of hydrochloric acid, if 25.00 mL is just neutralized by 40.00 mL of a 0.150 mol./L sodium hydroxide solution.
Solution...
Step 1: Write the balanced neutralization reaction.
Step 2: Calculate the numbers of moles of sodium hydroxide
moles = Concentration x Volume = C x V
Step 3: Calculate the moles of hydrochloric acid used.
Step 4: Calculate the concentration of the HCl
C = n/V
"Calculating Volume Needed to Neutralize"
Page 7...
What volume of a 0.250 mol./L solution of carbonic acid is needed to neutralize 30.0 g of sodium hydroxide?
Solution...
Step 1: Write the balanced neutralization reaction.
Step 2: Determine the number of moles of base
Step 3: Calculate the moles of 
needed to neutralize the base.
needed to neutralize the base.
Step 4: Calculate the volume of 
required
requiredV = n/C
Mrs. Kozoriz also gave us a worksheet to work on and this have to be hand in by TUESDAY!
Reminder: Don't forget to answer {PROBLEMS Page 9 (1 - 9) on our booklet}
Sayonara (bye) =) .......next scribe yicong...^_^
Wednesday, February 11, 2009
Precipation Correction
hello everybody.....
reminder..don't forget to do page 6 and 7 from your booklet...
the next scribe will be larlyn :)
Today we corrected the worksheets we got from Mrs. K the first one was Identification of Unknown Solutions (questions 1 & 2) then Analytical Problem Solving also, we started a new topic "Defining Neutralization", it is in page 5.
corrections....
corrections....
Identification of Unknown Solutions
1)
1)
2)
3)
4)
reminder..don't forget to do page 6 and 7 from your booklet...
the next scribe will be larlyn :)
Tuesday, February 10, 2009
tue..feb 2
Hi! There…
First off, Ms.K. gave us a sheet entitled IDENTIFICATION OF UNKNOWN SOLUTION; this sheet explained the step by step process in identifying an unknown solution. Like....
Carefully observe the unknown solution (colour) .....
- Some Aqueous solutions can be recognize by their colours such as the Copper (blue),Chromium(green),iron( pale yellow) etc.
Observe according to their solubility.....
- This can be recognize by mixing the solution to other solutions, be sure to list the products or the outcome (whether they precipitate or not), this may be helpful in identifying the unknown compound.
This experiment must be done meticulously to avoid any mistakes.....!*_*
First off, Ms.K. gave us a sheet entitled IDENTIFICATION OF UNKNOWN SOLUTION; this sheet explained the step by step process in identifying an unknown solution. Like....
Carefully observe the unknown solution (colour) .....
- Some Aqueous solutions can be recognize by their colours such as the Copper (blue),Chromium(green),iron( pale yellow) etc.
Observe according to their solubility.....
- This can be recognize by mixing the solution to other solutions, be sure to list the products or the outcome (whether they precipitate or not), this may be helpful in identifying the unknown compound.
After she went over the sheet, she let us to choose our partner and gave each pair a four different types of unknown solution (*different in each pair). And the only equipment that we’d used to identify the unknown solution are the following: spot plate, stir stick, a solubility chart and the solution themselves.
This experiment must be done meticulously to avoid any mistakes.....!*_*
All solutions were in dropper bottles, where you just need to add a few drops of an assign unknown solution from the dropper bottle to the plate. Observe if the solution precipitates or the colour changes(list your observation). Repeat the process from the rest, Remember that all the observation you came out with ,are very helpful in identifying the unknown solutions.
So,that's all for today........
the next scribe will be hmmmmm...Ramina!:>
Monday, February 9, 2009
Tuesday, February 3, 2009
Scribe List
This is The Scribe List. Every possible scribe in our class is listed here. This list will be updated every day. If you see someone's name crossed off on this list then you CANNOT choose them as the scribe for the next class.
This post can be quickly accessed from the [Links] list over there on the right hand sidebar. Check here before you choose a scribe for tomorrow's class when it is your turn to do so.
This post can be quickly accessed from the [Links] list over there on the right hand sidebar. Check here before you choose a scribe for tomorrow's class when it is your turn to do so.
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