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9/12/24 Partner: Jeff Somvorachith Lab 1. Physical and Chemical Changes Lab  Purpose: To identify physical and chemical changes through different experiments. Procedure: Experiment A Dissolve a small amount of copper sulfate pentahydrate in...

Experiment D Place 5 drops of silver nitrate into a test tube. Add 5 drops of sodium chloride into the test tube. Rinse test tube in the sink. Experiment E Put about 50ml of water into an Erlenmeyer flask and take...

- There are some popping noises when heating and a smell is produced(water boiling smell). - When mixed, the mixture is a transparent blue. - It mixes as the water boils and becomes slightly darker and less transparent. - After the liquid evaporates, there ...

9/12/24-9/13/24 - End mixture is clear. - End mixture is 29oC. Experiment - It cooled by 30C. Experiment F - Water is clear, sodium polyacrylate is white. - The mixture is a solid, opaque substance that sticks to the beaker. - The sodium polyacrylate ab...

milky, cloudy substance with chunks floating in it. Experiment D was a chemical reaction because mixing the silver nitrate and sodium chloride yielded a white and cloudy liquid. Experiment E was a chemical changes because it was an endothermic reaction. It coo...

Physical and Chemical Changes Lab: Page 1 to Page 5. Mole Concept II: Page 6 to Page 7. Hydrated Compounds: Page 8 to Page 10. Empirical Formula Determination: Page 11 to Page 13. Reactions in Solution Precipitation: Page 14 to Page 17....

9/19/24 Partner: Jeff Somvorachith Lab 2. Mole Concept II Purpose: To practice using the mole and making mole calculations. Procedure: A. Mass a penny. Assuming it is pure copper, calculate: The number of moles of copper. The number of co...

Analysis: A. 3.07g/63.546 amu =0.0483 mol <-1.     0.0483 mol *6.022*1023=2.91*1022 atoms Cu. <-2. B. 0.72g/20=0.036g 0.036g/(1.00794+15.9994)=0.0021 mol <-1.     0.0021 mol *6.022*1023=1.26*1021 molecules <-2. C. 6.49/[2(12.0107)+3(1.00794)]=0.104 mol PV...

10/11/24 Lab 3. Hydrated Compounds Purpose: To use hydrated compounds to practice calculating how much water molecules are attached to other molecules and compounds. Procedure: Clean the crucible with water, dry it with a paper towel, and heat it fo...

Mass of crucible and hydrated compound: 16.08g Mass of crucible and anhydrous compound(first heating): 14.55g Mass of crucible and anhydrous compound(second heating): 14.55g Observations: The MgSO4•xH2O turned a more white color and seemed to melt into a s...

10/14/24 I get a ratio of 1:9.6 mol MgSO4:H2O, the correct ratio is 1:7. My results are pretty accurate. The water must have been pretty close to completely evaporated, assuming the scale was 100% accurate. The error most likely comes from an inaccurate scale...

10/15/24 Partner: Connor Engels Lab 4. Empirical Formula Determination Purpose: To determine the empirical formula for a tin-oxygenated product. Procedure: Clean and dry an evaporating dish and a watch glass cover. To dry them, heat strongly for 2-...

Data: Mass of tin: 2g Mass of tin, evaporating dish, and watching glass: 39.21g Mass after 1st heating: 39.76g Mass after 2nd heating: 39.71g Mass after 3rd heating: 39.71g Observations: It started to bubble, turn orange, and let off orange vapor. Bad, ...

10/16/24 Analysis: Mass of Sn 2.00 g/118.7 g/mol=0.0168 mol Sn 39.71g-39.21g=0.5g O mass O 0.5 g/16.00 g/mol=0.0313 mol O 0.0313 mol O/0.0168 mol Sn=1.86≈2 O 0.0168 Sn/0.0168 Sn=1 Sn Empirical Formula=SnO2 Conclusion: The purpose of the lab was to det...

Partner: Jeff Somvorachith 10/31/24 Lab 5. Reactions in Solution Precipitation Purpose: To practice identifying reactions that result in precipitation and practice recognizing and writing equations for double replacement reactions by testing pairs of reage...

solutions to the proper location. Some of the solutions contain transition metal ions, so should not be washed down the drain. Instead, dump the contents onto a paper towel in the tray labeled "transition metal waste". Wash some items with water and clean othe...

Conclusion: a. Formula of Precipitates CoCl2 CuCl2 AlCl3 BaCl2 NiCl2 NaI CuI2 Na2CO3 CoCO3 CuCO3 Al2(CO3)3 BaCO3 NiCO3 Na3PO4 Co3(PO4)2 Cu3(PO4)2 AlPO4 Ba3(PO4)2 Ni3(PO4)2 Na2SO4 BaSO4 NaOH...

11/1/24 c. Net ionic formulas Cu2++2I+->CuI2  Co2++Co32-->CoCO3 Cu2++Co32+->CoCO3 2Al3++3CO32-->Al2(CO3)3 Ba2++CO32-->BaCO3 Ni2++CO32-->NiCO3 3Co2++2PO43-->Co3(PO4)2 3Cu2++2PO43-->Cu3(PO4)2 Al3++PO43-->AlPO4 3Ba2++2PO43-->Ba3(PO4)2 3Ni2++2PO43-->Ni...

Partner: Jeff Somvorachith 11/4/24 6. Stoichiometry and Limiting Reagent Purpose: To practice using stoichiometry and identifying and calculating the limiting reagent by reacting copper(II) sulfate with iron, determining the limiting reagent, and observing...

The tape on our beaker burned. Took about 1 minute 50 seconds to dissolve. Letting off steam. Seems to heat up more when adding the iron. Solution turned from blue to grey. Iron seemed to rust. Combined to form Fe3O3. Has an iron sort of smell. Precipitate set...