Kyle-Wednesday, 2/23 Solubitity

1) We got our ChemThink Homework stamped by Mr. Tucker.

2) We went over problem #5 on the Solubility Practice worksheet.

• NaNO3(aq) + AgNO3(aq) ------> NaNO3(aq) + AqNO3(aq)

• Their is no reaction because all four coumpounds are soluble in water(aq).
• You just put a line through the problem or say NR.

3) We also did a Solubility Lab in which we mixed six different solutions with each other and we watched to see if their was a reaction. We made a 6 by 6 grid with the solutions and their reactions. If their is an X through one that means we didn't try the solutiuon. NR means no reaction and Rxn means a reaction occured. Here is the chart we did in class.

	MgCl2	K3PO4	NaNO3	Na2CO3	AgNO3	CuSO4
MgCl2	X	X	X	X	X	X
K3PO4	Rxn-Cloudy color	X	X	X	X	X
NaNO3	NR	NR	X	X	X	X
Na2CO3	Rxn-Cloudy color	NR	NR	X	X	X
AgNO3	Rxn-Cloudy color	Rxn-turned yellow	NR	Rxn-Cloudy color	X	X
CuSO4	NR	Rxn-Cloudy color	NR	Rxn-Cloudy color	NR	X

Here are some examples of a reaction taking place. Make sure to use the Solubility Rules worksheet as a cheat cheat. Notice how one product is a solid(s) and the other is aqueous(aq).

1. K3PO4(aq) + 3MgCl2(aq) ------> 6KCl(aq) + Mg3(PO4)2(s)
2. Na2CO3(aq) + MgCl2(aq) ------> 2NaCl(aq) + MgCO3(s)
3. 2AgNO3(aq) + MgCl2(aq) -------> 2AgCl(s) + Mg(NO3)2(aq)
4. 3AgNO3(aq) + K3PO4(aq) -------> Ag3PO4(s) + KNO3(aq)
5. 3CuSO4(aq) + K3PO4(aq) -------> Cu3PO4(s) + 3KSO4(aq)

Now here are a couple examples of no reactions or NR. Notice how the products are both aqueous(aq).

1. 2NaNO3(aq) + MgCl2(aq) -----> 2NaCl(aq) + Mg(NO3)2(aq)
2. AgNo3(aq) + NaNO3(aq) -------> AgNO3(aq) + NaNO3(aq)

4. The last thing we did today was get a sheet called Solution Stoich 1. Mr. Tucker went over problem #3a. For homework we have to try problem 3b.

3a. What volume of 0.150 M AgNO3 is needed to react with 45.0 mL of 1.50 M CaCl2?

3b. What mass of AgCl will be produced when 150mL of 0.650 M CaCl2 reacts?

Natalie- Tuesday, 2/22

1) We picked up one sheet: ChemThink Precipitate Lab

2) We went over lab quiz we took on friday

• Molarity= unit of concentration
• Use formula to determine how many mols of solute needed to make 0.15 M of solution
• If you need help with the formula use this video as a reference: http://www.youtube.com/watch?v=8oTqwBAvbnY&feature=fvwrel
• 
  

  .015 mol NaCl	58.44g NaCl
  	1 mol NaCl

  
  
• Fill beaker with 50 mL of water
• Then mix in .88g of Solute (NaCl)
• Then fill rest of the beaker to 100 mL

3) Went through IV. Solubility Notes

• 
• Soluble in water= dissolves in water (aqueous)
• In soluble= does not dissolve in water (solid)
• There are some exceptions though, mentioned on the sheet

4) Went through V. Solubility Practice #1-3:

• 
• If the balanced equation has aqueous on both sides, then no reaction has taken place

5) Homework are questions #1 and #2 on the ChemThink precipitate lab sheet we picked up in

class. Use www.chemthink.com to answer the questions under Solubility

Shayne - Friday, 2/18

I. We picked up two sheets at the beginning of class - (Molarity 2 and Reaction Stability 1)

II. We went through the Molarity 2 notes:

EXAMPLES:

1.) What will be actually present in the solution when each of the following is added to water?

a. KCL ----------> K+ (aq) plus Cl- (aq)
b. NaNO3 ----------> Na+ (aq) plus NO3- (aq)
c. C2H6O ----------> C2H6O (aq)

3.) Calculate the mlarity (M) of the following solutions. (M = Mol/L)

a. M = 0.0346 Mols/0.250 Liters = 0.138M
b. (405 g NiCl2 X 1 mol NiCl2)/129.59 g NiCl2 = 3.12524 mols NiCl2
M = 3.12524 Mols/7.54 Liters = 0.414M
c. (22.57 g H2SO4 X 1 mol H2SO4)/98.09 g H2SO4 = 0.23009 mols H2SO4
100 Ml = 0.1 L so.....
M = 0.23009 Mols/0.1 L = 2.301M

5.) Calculate the mass of the solute present in the following solutions.

a. Mol = M x L so...
0.125M x 0.200L = (0.25 Mols Kbr x 119 g KBr)/1 Mol KBr = 2.98 g KBr
b. Mol = M x L so...
Mol = 0.150M x 0.1L
(0.015 Mols Na2SO4 x 126.05 g Na2SO4)/1 mol Na2SO4 = 1.89 g Na2SO4

III. We took a lab test in groups of two, having to make a solution of 0.15M of NaCl and show calculations

Th-2/17-Gabuzzi

1. We picked up 2 sheets.

• Molarity 1
  
• Dissolving 1

2. We took a quiz on the mixtures notes we took on wednesday.

3. We then review the different types of substances and mixtures.

4. We finished the Solution Notes

III. Solutions . (we used salt water as an example)

A. Solute- dissolved (salt)

B. Solvent- doing dissolving (water)

C. Solution- solute and solvent (mixture of salt water)

D. Concentration of solution:

M=molarity

M= 1 mol solute per liter of solution. 1.0m=1 moler.

E. Preparation of solution:

1. find total volume
2. fill container 1/2 way with solvent
3. add a solute and mix
4. fill container to desired volume with solvent

We filled out the Molarity 1 and Dissolving 1 Worksheets (see photos at top for answers)

Homework: Finish Molarity 1 worksheet or we will be doing webassigns for the rest of the year.

Wednesday, February 16

1. Pick up 6 sheets:

• 4 pages of Solutions Notes

• 2 pages of Mixtures Lab

2. Got Lab Test and Stoich Test back

3. Started the Mixtures lab

There are 4 unknown liquids as shown below


(liquids in order left to right)

they must be observed based on:

1. how they look
2. what happens when shaken
3. whether there is an odor
4. whether a light shines through or not
5. how quickly it filters

(all 4 liquids being filtered)

6. what's left when liquid evaporates

4. Data:

1. look at picture above
2. unknown 1: stays the same, unknown 2: same, unknown 3: mixes but settles, unknown 4: same
3. none had much of an odor
4. light shined through unknowns 2 and 4 but not 1 and 3
5. 2 and 4 filtered quickly. 1 and 3 filtered slowly
6. unknown 1: white powder, unknown 2: blue residue, unknown 3: muddy paste, unknown 4: evaporated clean

5. Solution notes

I. Types of Substances:

A. Pure - can be one substance

B. Mixtures - can be more than one substance

C. Examples:

1. mixture
2. mixture
3. pure

II. Types of Mixtures:

A. Solutions

• shake - no change
• uniform
• light passes through
• everything goes through filter
• evaporate - residue

B. Suspensions

• shake - change
• settling
• light does not go through (Tyndall Effect)
• substance is filtered out
  
• evaporate - residue

C. Colloids

• shake - no change
• does not settle
• Tyndall Effect
• everything goes through filter
• evaporate - residue
  

Thursday February 10 2011-Matt Ploetz

1)We went over our Quiz 5.

2) We then learned about Percent Yield and did one problem on it. (See Pictures)

3) Then we worked more on our Penny Lab.

4) We took Quiz 6.

Wednesday, February 9, 2011, David Colston

1)First, we picked up two new worksheets. The page numbers were 33 and 34, and they had the same title: Limiting Reactants 4

2) We then proceeded to go over the Penny lab we did in class. In the Penny Lab, we put the CuCl2 and the nails in water and stirred it up. After stirring it for a while, the blue-tint to the water caused by the Copper Chloride disintegrated, and the water remained there. By this we know that CuCl2 is the limiting reactant, but you can also do this by writing the problem out like this:

First you must balance the equation, so it would be:

3CuCl2 + 2Al ----> 2AlCl3 + 3Cu

Then, you need to put your data in your tables:

3.0 grams CuCl2	1 Mole CuCl2	3 Mole Cu	63.55 grams Cu
	134.45 grams CuCl2	3 Mole CuCl2	1 Mole Cu

Answer: 1.417 grams Cu - We know this is the limiting reactant because CuCl2 has less then the Excess reactant, Al

1.25 grams Al	1 Mole Al	3 Mole Cu	63.55 grams Cu
	26.98 grams Al	2 Mole Al	1 Mole Cu

Answer: 4.416 grams Cu - Excess Reactant... Can only make as much as the limiting reactant though, so it can only make about 1.4 grams of CuCl2

To answer the second question, we can go backwards from grams needed to grams CuCl2.

3) We went over quiz number 4

A.

12.5 grams Al	1 Mole Al	2 Mole Al2O3	101.96 grams Al2O3
	26.98 grams Al	4 Mole Al	1 Mole Al2O3

12.5 grams O2	1 Mole O2	2 Mole Al2O3	101.96 grams Al2O3
	32.00 grams O2	3 Mole O2	1 Mole Al2O3

Answers

A. 23.6 grams Al2O3 = Limiting Reactant

and

26.6 grams Al2O3 = Excess Reactant

B. The mass of the product can only be as much as its limiting reactant, so it would equal 23.6 grams

4) We went over a problem on page 33

Problem Number 2: 2NH3 +5F2 ----> N2F4 +6HF

If 120 g of NH3 is allowed to react with 590 g of F2,

What mass of HF can be formed?

120 grams NH3	1 Mole NH3	6 Mole HF	2 grams HF
	17.04 grams NH3	2 Mole NH3	1 Mole HF

Answer =422.7 grams HF or 420 grams HF (Sig Figs)

590 grams F2	1 Mole F2	6 Mole HF	20.01 grams HF
	38 grams F2	5 Mole F2	1 Mole HF

Answer= 372.8 grams HF or 370 grams HF (Sig Figs)

Limiting Reactant

What is the Excess Reactant?

372.8 grams HF	1 Mole HF	2 Mole NH3	17.04 grams NH3
	20.01 grams HF	6 Mole HF	1 Mole NH3

120 grams NH3 -105.8 grams NH3=14.2 grams NH3 or 14 grams NH3 (Sig figs)

5) We took Quiz Number 5, covering the things that we learned in class today (That are on here)

6) We went over the newest Lab, that is just one day out of our 3 day lab test. If you missed yesterday, you may want to see Mr. Tucker, but it isn't the end of the world seeing as we only spent about 10 minutes on it. What we began to do was: We put the CuCl2 and the nails in water and stirred it up. The nails become a rusty gray color. We will work more on this in class tomorrow.

HOMEWORK/NOTES: PREPARE FOR QUIZ, AND FUTURE QUIZZES. IF YOU DON'T UNDERSTAND SOMETHING, GO OVER IT OR GET HELP WITH MR. TUCKER, A FELLOW CLASSMATE OR IN THE TLC. DO AS MUCH OF PAGE 33 and 34 AS POSSIBLE. THINK ABOUT THE LAB EXAM!!!

If you read this, thank you! I hope it was a help!

Tuesday-02/08-Tucker

Today we did a chemistry scene investigation lab to help us understand limiting reactants. It looks like this:

1.The chemical equation for this lab was:

3CuCl2 + 2Al --> 2AlCl3 + 3Cu

2. We worked with 1.25g of aluminum, 3g of CuCl2, and 175mL of water

3. To complete the lab we had to figure out how many chemicals w

e need to produce 1.8g of copper

4. In the lab some of the CuCl2 was used up, some of the aluminium turned into copper but there was still some aluminum left

5. CuCl2 was the limiting reactant

This is a picture of the CuCl2 and pieces of aluminum from the lab:

Homework:

Answer the 2 questions from the lab:

1.Which supplier made the mistake?

2. How much more of the chemicals will you need?

M-2/07-Scott

-Passed back the Mole Quiz. You have untill the end of tomarrow to make it up.

-went over Stochmerty Quiz 3

- Did limiting reactents notes

1) put the two muesurement in grams of the chemical that is given on the left side, with one on top, and another below that (two diffrent equations)

2) Put the the grams of the product and the right side of both equations (jusst like how we set it up before)

3) solve using the mole island going from grams of A, to grams of b.

4) Look at the equation that comes out with the least amount of your product. The intial chemical that was given in grams is your limiting reactent. The other is called the Exessive Reactent.

5) The lowest answer is the most of this product that can be made.

-Took Stochmetry Quiz 4

- Homework: journal page 29

Fri 6/2-Koh

Today we learned how to do limiting reactions.
1. Mr. Tucker showed us how to do Limiting Reactants using the grilled cheese example.
Say you have ten grams of bread and twenty five grams of cheese. How much sandwich would you be able to make? Since ten grams of bread only makes .8 sandwiches (using conversions factors), and since twenty five grams of cheese makes and entire 1.85 sandwiches, (also using simple conversion factors), then we'd only be able to make .8 of sandwiches. We only have enough bread to make .8 sandwiches and the entire 25 grams of cheese would be too much and we'd have excess cheese. This works the same way with molecules. You can't make 2 water molecules with four hydrogen atoms and one oxygen atom. You'd just have one molecule of water and two left-over hydrogen atoms.

2. We went over a limiting reactants sheet. It looked something like this.

3. Lastly we got our quizzes back and took the new one.

Extra Stoich Practice!!

For a problem that gives moles of Substance A and asks for mols of substance B use 1 step.  For this one step you will just use the balanced equation ratios.

For a problem that gives moles of Substance A and asks for grams of substance B use 2 steps.  Start with the balanced equation ratios for the first step and then use the molar mass (from periodic table in grams/mole) of substance B for the second.

For a problem that gives grams of Substance A and asks for mols of substance B use 2 steps.  Start with the moalr mass of substance A and then use the bal. eq. ratios.

For a problem that gives grams of Substance A and asks for grams of substance B use 3 steps.  Start with the molar mass of substance A, then use bal. eq. ratios, and then finish off with the molar mass of substance B.

For a problem that gives ml of Substance A and asks for grams of substance B use 4 steps.  Start with the DENSITY, then use moalr mass of substance A, then bal. eq. raitos, then finish off with the molar mass of substance B.  If you are ever given the grams and asked for ml, just reverse this order.

Now try to identify how many steps the following problems contain and what the steps involve (no need for any math, X and Z just hypothetical substances, just set problems up!!)

1.  How many moles of X react wirh 25.0g of Z?

2.  How many grams of Z will be produced from 12.35g of X?

3.  How many ml of Z can be produced if we also produced 35.245g of X?

4.  How many moles of Z can react with 500.0moles of X?

5.  What mass of Z would be needed to produce 10.1moles of X?

BONUS:  How many atoms of X can be produced from 25g of Z?  Use mol island for this one