Abstract: We conducted this experiment to work on enthaply and calculating deltaT.  The problem that ws address to us was that can we dissovle a .2g of Mg in HCL. We had a calorimeter and HCL and Mg and a temperature prob.  The major results that we found in this experiment is that when you out a .2g of Mg in 50 ml of HCL it raises that temp and it will dissolve in about 3mins The overall conclusion is that we found the missing temperature and the mass of the Mg we needed.

Saftey Considerationsb: The saftey considerations that we took was wearing saftey glasses and carfully pouring the HCL in the caloirmeter.  Cleaning the table after we were done and cleaning the utensalls that we used.

Materials:

• Saftey glasses
• one Calorieter
• 50ml of HCL
• .2g of Mg ribbon
• Spark temperature prob
• rubber gloves
• graduated cylinder

Procedure: We first got one caloirmeter rinse it with distilled water, then obtained 50ml of HCL in a graduated cylinder. We recorded that mass of the empty calorimeter and record that mass of the colrimeter with the HCL in it.  Record the temperature of the HCL in the calorimeter. Measure out .2g of Mg, record the mass. Roll up the Mg into a loose ball then place it in the colarimeter.  Record the temperature every 15 seconds until you can not hear the gas anymore.  rinse the prob of and dispose of the liquid in it proper place, then clean the table. 

Evidence Collected:

caloirmeter mass: 26.90g

calorimeter + HCL 76.45g

HCL Temperature: 24.5 C

Magniseum Ribbon: .2g

 00:15 - 26.8 C

00:30 - 29.8 C

00:45 - 31.1 C

1:00 - 32.5 C

1:15 - 37.4 C

1:30 -39.3 C

1:45 - 40.8 C

2:00 - 41.5 C

2:15 - 41.8 C

2:30 - 41.8 C

2:45 - 41.8 C

3:00 - 41.8 C

1) 2HCl + Mg = MgCl(2) + H(2)

2) Q= m x deltaT x C

      = 49.55 x 15 x 4.2

      = 3121.65 J

3) 3121.65 x 1 kJ/1000 J = 3.12165 kJ

4) .2g x 1 mol/24.3050g = .00822876

5) 3.12165 kJ/.00822876 = 379.35 kJ/mol

6) delta H = (-801.15)+0 - 2(-167.2)+0

              = -466.75 kJ

7) 379.35 - (466.75)/(466.75) x 100

          = -18.72522 % error

Claim: The claim that we found was the temperature that Mg makes is 41.6 C and does the Mg dissolve all the way.

Scientific Explanation: What i learned form this experiment is the temperature and the number of Joules that takes to dissolve that Mg in HCl.  I learned more exquatiuons to solve the questions that we were assigned. i also found my percent error that i had after the experiment. 

The feedback that i got was very positive.  What Brendon Babcock said about the body of my paper was good. He said that the paper was well written and had good recommendadtion that was good. 

There were not five things for me to change to my paper, that he gave me. I do plan on changing the fisrt and the sceond paragraphs around.  i have read over my paper and i will change alot of my sentences that begin with There, The, These, This. 

I dont really have anymore questions about my topic.

Holden Clark

Research question:

What is the pH and the pOH of each of the deluted solutions, and what is the [H+] and the {OH-] of each solution?

Abstract:

we conducted this experimet to get better at confirming the level of pH for each solution.  The main problem is what is the pH and the poH.  The method we used was using the pH card to idenfiy the level of each soultion.  the results that we obtained form each of the soultions were that they were close to each other.  The other all conclusion of the experiment is that we leanred more about how to use the pH leveling card.

Safety Considerations:

The safety concerns that our group took were to wear our dafety glasses and manke sure to be carful when pouring the solutions into their cuvettes and their beakers. we also made sure that the lab tabel was clean when we were finished with the experiment.  We deposed of the solutions to their correct place. 

Materials:

The materials that we used were 16 cuvettes and about 5 droppers.  The solutions that we used were HCl, KOH, NH4OH, and Acetic Acid. 

Procedure:

We first took .1M of each of the soultions and put them in seprate cuvettes.  We labeled the cuvettes with each of the names of the solutions.  From there we took 2 drops from the first cuvette into the second one, and then added to 18 drops of distilled water.  From the second cuvette we took 2 more drops and placed them into the third cuvette and added 18 more drops of distilled water.  Then fromf the third cuvette we took 2 more drops and placed them into the fourth cuvette and added 18 more drops of distilled water. Now after we finished with all of the cuvettes we took a drop from each of the 16 cuvettes onto a seperate piece of pH paper.  We waited for 90 seconds to determind the pH of each of the 16 soulutions, becuase we had to wait for the reactions to finish. After the reaction we compared the color to the pH card.

Evidence Collected:

Claim:

The claim that i have is that the high the pH level the srotnger the soultion is. 

Scientific Explanation:

The number one thing that I learned was how to use the pH strips and what on the pH level is a base a nuetral and a acid.  The evidence that i collected help my clam because we you see the level of the pH of each of the solutions get closer 14 on the pH level the stronger the solution.  The farther away form 14 the weaker it gets. 

Proving Beer's Experimnet

II  Absrtact

we want to see the different red absorbance of the CUSO4 concentration when we took different amounts of the concentrations.  the problem that we were solving was to see how much red absorbance of light is absorbed in each of the six cuvette.  we dilutided the concertartion six times unitl there was just water left in the last cuvette.  the more water that we had in the test tubes the more red absorbance there was.  the less water, and more CUSO4 solution the more red absorbance. 

III  SAFETY CONSIDERATIONS

wear safety glasses so that the solution doesnt get into your eyes.  keep the solution away from your body just incase that it spills it doesnt get on your cloths.   use the correct amount of the sloution in the experiment so that nothing bad could happen like bad chemical reaction.

IV  MATERIALS

the materails that we used where a vile to combine the water and the CUSO4.  a cork to close the vile.  six test tubes and six cuvettes, colorimeter and a trasnfer pipet. 

V  PROCEDURE

take 25ml of water put it into a vile add 3.121 grams of the CUSO4 to the water. shake until it is completely dissovled.  in the first test tube take 1ml of the stock soltion and add 4 ml of water. in the second test tube take 2ml of the stock soultion and 3ml of water, the third tube take the 3ml stock solution and 2ml of water.  the fourth tube take 4ml stock solution and 1 ml of water.   the fifth tube take 5ml stock solution and 0ml of water.  in the sixth and final test tube take none of the stock solution and 5ml of the water.  once you have all the test tubes filled with 5ml total pour each of them in a colorimeter cuvette. and test the read absorbance. 

VI  EVIDENCE COLLECTED

i found that if you add more CuSO4 solution to the water the more red absobance there is.  like when we had 5ml of the stock solution and none of the water it was 2.223 absorbance. when we only had 5ml of water we had 0 red absorbance. 

VII  CLAIM

the more the solution the more the red absorbance their is. the less solution the less absorbacne.

VIII SCIENTIFIC EXPLANATION

i learnd what the sloution CuSO4 is what it looks like.  i also learned mixed with water less redabsobance it has. from the evidence that i collected i found this out,  from the beginning of the experiement i had no idea what to expect from the CuSO4.  it was a fun experiment and i had fun proving Beer's law.

ABSTRACT:

To test how much light passes through the cuvette that we put into the colorimeter. The problem that we were test was how much a concentrated sloution allows light shine through.  our method was to to start with a solution with blueing in it. then test the sloution with the coloimeter, then dilut the solution by taking 0.5ml of that solution into another test tube. and test it with the colormieter.  the major resukt that we obtained was 100% of light passing through the soultion.  i learned that you can use a colorimeter to caliprate the concentration of a soultion. 

SAFETY CONSINDERATIONS:

Wear your saftey glassess at all times when we are in the lab area and clean the test tube before putting it away.  measuring the correct amount of bluing and the correct amount of drops in each cuvette.  then cleaning up the lab table after done with the experiment. 

MATERAILS:

- Liquid Bluing solution (blue iron suspension)

- Dilution well plate

- Plastic Dropper

- Distilled Water

- 10 - glass test tubes

- Pasco SPARK w/colorimeter

- Glass cuvettes 4 or 5

PRODUCE:

label your test tubes 1 through 10.  then place 5ml of liquid bluing in test tube #1. this test tube can labeled as 1x.  then take 0.5mL (exactly 12 drops) from the test tube 1x and then out into the second test tube. then using the clean dropper add 4.5mL of distilled water to the 0.5mL of orignal solution.  repeat the process until you can barley see the blue dye in the test tubes, record the concentrations as you go.

EVIDENCE COLLECTED:

1x test tube has 0.0% visable light.  test tube 2 is one tenth of the soultion of test tube 1.  there was 0% of visable light.  test tube 3 has 9.7% of visable light, test tube 4 has 66.3% of visable light, test tube 5 has 98.2 visable light, and finaly test tube 6 has 100% of visable light.  test tube 6 has no bluing in the solution. 

CLAIM:

how much bluing will be in the sloution will be in the test tube when there is 100% of visable light shining through.  

SCIENTIFIC EXPLANATION:

it takes six dilalations to get 100% visable light passing through the cuvette.  the concertration was .00001 tenth of the orginal concenrtaion.  i learned that you have to take many percise step so that you can get 100% of visiable light through you concertration and if you make a mistake yu have to start over along ways back to make the correction.  so it was a very fun experiment because i learn how to use a colorimeter. and waht bluing is.   

1. it helps scientists classify the subatmoic particles, so that they can use them in thier experiment.

2.each subatmoic particle is classified according to what they make up. like Leptons make up electrons, quarks make up protons and nuetrons.

3.each category could go more in depth and add a newe category could be added.

Resesrch question:In what location will the given objects be found when dropped into the density cloumn?

Abstarct: this experiment was conducted to see what item would be locatded in corn syrup, water and canaola oil.  we found the mass of each object and found the volume of each object.

Safety cinsiderations: the safety steps that i took was that i did not break any glass wear that i used.

Materials:

-Zinc

-Acrylic

-Brass

-Steel

-Wax

-Cork

-Low density Polyethylore

Procedure: we took each item found the mass, the mass and the volume of each item is

-Zinc m  6.62g  v .5ml

-Acrylic m 4.71g v 4.3ml

-Brass m 34.28 v 4.5ml

-Steel m 31.29 v 4.5ml

-Wax m 20.18g v 12ml

-Cork m 1.829 v 0 ml

-(15) Low Density Polyethylore m 0.68g v 1.05

Evidence collected: the info that we found was not a big suprise bceuase from holding the object i guess where it would located in the column. 

Claim: just about everything will just about be at the bottom execpt for the cork and the low density polyethlore. 

Scientific Explanation: basically what i found was that all the items would sink to all the way to the bottom or just about the bottom.  if you dropped the brass and the steel in the column in the same time they would both go to the bottom.  if you dropped the cork and the low density polyethylore they would be about the same place becasue they are have about the same mass and the same volume.  

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