Synthesis Of An Iron ( IIi ) -Oxalate Complex

Synthesis Of An Iron ( IIi ) -oxalate Complex
EXPERIMENT 4A: Synthesis of an Iron(III)–Oxalate Complex: To begin, a filtering crucible was washed, labeled, and dried in an oven for one hour.
While the experiment was performed, the filtering crucible was set–aside in a desiccator to cool and stay dry. After this was done, a mass of about 1.2
g (В±0.2 g) of iron(II) ammonium sulfate hydrated salt (Fe(NH4)2(SO4)2 в€™ 6H2O) was measured and recorded. It was then placed in a 50
–mL
beaker with 3 mL of deionized water and 1–3 drops of 6M sulfuric acid. The beaker was then swirled until all of the salt particles dissolved. Then,
about 6 mL of 1 M oxalic acid was added to the solution in the 50–mL beaker. At this point, the pH was checked to ensure that solution was acidic. If it
wasn't acidic, then an addition of 6 M sulfuric acid may have been needed. This solution was then gently boiled, with boiling chips, for about five
minutes to break down the precipitate. While the solution boiled, it was essential to swirl the solution. Once the solution had cooled down, the
supernatant was decanted and put in a waste beaker, and the precipitate was washed with clean, hot deionized water. This precipitate was rinsed three
times. The supernatant and wash solution wastes were then thrown away in waste containers. Then, 3.5 mL of 1.7 M potassium oxalate solution were
added to the beaker with the rinsed precipitate. This solution was warmed to about 40в„ѓ and it was constantly stirred. The solution was then removed
from the Bunsen burner, and
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Antacids Lab Report
CHM 2046L Lab Report: Antacids
Katie Wong
Lab Partner: Kealie Do
June 27, 2017
Abstract:
The build up of stomach acid may cause irritation and excess pain to individuals. Luckily, antacids being a weak base can help relieve the symptoms
and pain. Antacids, such as Gelusil, Medi–Firs, Alka Seltzer, and Alcalak are neutralizing agents of acids that become helpful to the human body when
heartburn occurs. Heartburn, also known as acid reflux is a common medical issue that occurs when hydrochloric acid (HCl) from the stomach moves
backward along the digestive track to the esophagus (located within the throat). This reverse flow of fluids causes a burning sensation due to and
possible sour taste that is characteristic of acids [1].
Introduction:
The purpose of the experiment was to compare antacids by the amounts acid they neutralize to find the most effective antacid. Finding the most
effective antacid is important because it will help others by allowing them to choose the best product for their heartburn. Titration is the process of
which the unknown solutions concentration reacts with a known solution concentration. During the experiment, titration was used to calculate the
moles of HCl neutralized by the antacid in this case was gelusil, by knowing the moles of HCl initially added to the flask and moles of HCl
neutralized by the NaOH.
Methods: Five 250mL Erlenmeyer flasks were obtained. Then, 200mL of hydrochloric acid (HCl) was poured into a 600mL beaker. The gelusil

Panacetin Lab Report
To begin the separation of the sucrose from the Panacetin, approximately 3 grams of Panacetin was transferred to a 125–mL Erlenmeyer flask. Added
to the flask was 50 mL of dichloromethane to dissolve the Panacetin to aid in the separation. A fluted filter paper was used to filter the Panacetin and
dichloromethane mixture by gravity using a glass funnel. The remaining filtrate was set aside than transferred to a separatory funnel and the substance
on the filter paper was dried and weighed. The filtrate was extracted with 2 increments of 25–mL portions of aqueous 1 M sodium hydroxide. During
this step the filtrate in the separatory funnel was shook and vented 3 times. In the separatory funnel there will be two visible layers of filtrate with

Experiment 8 Phenol Alkylation
Experiment 8: Phenol Alkylation Amber Chavis CHEM 2753– 007 November 15, 2017 Objective/Purpose: This experiment was designed by
conducting a substitution reaction to construct a complex compound (2–methylphenoxyacetic acid) from two simple parts; also known as synthesis –
converting simple molecules into more complex molecules. A purification technique known as crystallization was used to purify the product. Suction
filtration was used to filter out the product. The experiment was completed over a three–day experimental period. Procedure: In this experiment, 0.31 g
(2.87 mmol) of 2–methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a
hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2–methylphenol, 0.957 mL (0.00287 mmol) NaOH was
calculated and collected in a syringe. The NaOH was then added to the 2–methylphenol solution and allowed to mix completely. In another 10 mL
Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2–methylphenol and placed into the flask along
with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the
2–methylphenol and NaOH solution after it was fully dissolved using a microscale funnel. Then the apparatus was put together. The glass portion of a
medicine dropper was attached and placed inside of a

Bromopropane And Potassium Hydroxide Lab Report
The purposes of this experiment were to model a bimolecular nucleophilic substitution reaction between potassium hydroxide (KOH) with
1–bromopropane and determine whether it follows a second–order rate law mechanism. A rate constant of 0.0684 M–1 min–1 was obtained for this
reaction at 45.1В°C, which was determined through equilibrating the reaction and performing titrations of 0.390 M KOH with 0.1000 M hydrochloric
acid (HCl). The activation energy calculated from class data was 50.188 kJ/mol, which deviated largely from the literature range value of 72.80–83.76
kJ/mol. It was concluded that the reaction was consistent with the predicted SN2 mechanism, based on the regression of a trendline.
Many reactions that exist in nature involve a double displacement between ions and reactants with solvents. A bimolecularnucleophilic substitution, or
SN2 reaction, involves a nucleophilic attack on a substrate and the departure of a leaving group. Anucleophile is a compound or ion that donates
electrons to promote bond formation (Caldwell, 1984). In order for a leaving group in a compound to leave, it must possess the characteristics of a
weak base and be able to occupy electrons. Several factors affect the rate and favorability of such reaction, such as (Bateman, 1940). In addition, the
substrate that is attacked by the nucleophile is commonly an unhindered primary substrate to allow the reaction to occur quicker. An SN2 reaction
follows the second–order rate law. In this

Negative Effects Of Eutrophication
Abstract: In order to better understand cultural eutrophication a lab was performed on aquatic systems and the concentration of nutrients in those
systems. The lab was analyzed once a week for a total time of two weeks. After the two weeks, a trend (treatments with higher concentrations of
fertilizer had a higher cell count and lower pH) was discovered and noted the results.
Introduction:
Eutrophication is a natural process that lakes and certain bodies of water undergo. Eutrophication happens by having a significant level of
biodegradable waste in a body of water. The nutrients in the water promote growth of primary producers which has a positive impact on consumers.
These nutrients usually cause bodies of water to be cloudy, turbid, have a high number of primary producers, and promote the excessive growth of
algae (Koechli, 2015). This then causes the body of water to reduce its dissolved oxygen level, and dead biomass to accumulate. Although it is a
natural process, humans can affect these bodies of water by inserting a surplus of nutrients. This process is called cultural eutrophication, which is
considered a form of water pollution (Koechli, 2015). This pollution is often caused by fertilizer run–off and much more. It causes the overgrowth of
aquatic plants. These plants quickly become crowded and have to compete for space and sunlight. Because of this, aquatic life is threatened due to the
low dissolved oxygen, and blocked sunlight. Cultural eutrophication is

Chemical Properties Of Binary Compounds
Experiment 1
Prelab : CompoundMolecular Weight (g/mol)Melting / Boiling Point (В°C)Density (g/гЂ–cmгЂ—^3)Characteristics
Sodium Bromide, NaBr103747 / 13903.2White crystal, cause skin and eye irritation
Bromine, гЂ–BrгЂ—_2160–7.2 / 58.83.1Red liquid, corrosive Chemical properties of binary compounds of group 1 : Halides Hydrides Oxides
Diagonal relationship
Purpose :
Part I
Part II – To diagnose diagonal relationship.
Step–wise procedure :
Part I Prepare 40mL of concentrated гЂ–NaгЂ—_2 гЂ–COгЂ—_3в¦ЃгЂ–10HгЂ—_2 O solution. Weight Fe powder on XXXX balance and transfer
to a 250mL Erlenmeyer flask. Measure 16mL of water using a graduate cylinder, mixed it with Fe in Erlenmeyer flask and set into ice bath in fume
hood. Add 3.8g ( XXmL) of гЂ–BrгЂ—_2 dropwise from burette to Erlenmeyer flask and stir the solution with a glass rod simultaneously. Filter the
mixture using gravity filtration method into porcelain dish and add 1.4g (XXmL) of гЂ–BrгЂ—_2. Boil the content in the porcelain dish on a hotplate.
At the same time, add concentrated гЂ–NaгЂ—_2 гЂ–COгЂ—_3гЂ–10HгЂ—_2 O solution dropwise with Pasture pipette and stir it. Test the
basicity of the solution using universal indicator (strips turned blue). Filter off the precipitate when solution reached room temperature. Wash
precipitate with 10 – 15mL hot distilled water. Transfer filtrate to large evaporation dish. Heat the content on hot plate together with not more than 2
boiling chips in fume hood. Cool it in ice bath when crystals

Pyridinium Hydrobromide
In a 125 mL Erlenmeyer flask, 20 mL of glacial acetic acid were mixed thoroughly with 1.0 g of (E)–stilbene (which was synthesized in the previous
week's experiment). The flask was then placed in a hot plate in order to allow the (E)–stilbene to dissolve in the acetic acid. Once the (E)–stilbene had
completely dissolved, 2.0 g of pyridinium hydrobromide perbromide (also known as pyridinium tribromide) were added and the solution was mixed
thoroughly by swirling the flask. If necessary, some additional acetic acid may be used to wash down the walls of the flask in order to ensure the
proper reaction with complete amounts. It was observed that the flask acquired a very strong dark–red or brown tint, presumably due to the pyridinium
hydrobromide

Characteristics Of Aspirin
SYNTHESIS AND CHARACTERISTICS OF ASPIRIN– ACETYLSALCYLIC ACID
Summary:
The lab experiment was divided into parts and the synthesis of the aspirin occurred during the first week. Using 4.032g of salicylic acid 8.0mL of
acetic anhydride on a hot bath the reaction was speeded up by the use of a catalyst phosphoric acid. Once the sample was then left to dry in the drawer
for a week using the melting point apparatus we conducted the purity assessment of the dried sample.
Introduction:
Aspirin (acetylsalicylic acid) is a commonly known drug used to treat fever, pain and inflammation, aspirin can also be purchased over the counter
medication or by prescription from a doctor. The synthesis of aspirin occurs by combining acetic anhydride and salicylic acid, salicylic acid is a
naturally occurring product that can be found in the bark of a willow tree1. Since it is highly acidic and salicylic acid would potentially damage the
gastric membrane hence the addition of the acetic anhydride. C7H6O3+ C4H6O3 C9H8O4 +C2H4O2
A few drops of phosphoric acid are added to the reaction, phosphoric acid acts as a catalyst so as to speed up the rate of the reaction. The use of the
acetic anhydride cautions us to prematurely use any water so as to prevent any hydrolysis of the acetic anhydride from occurring.
Results and Discussion:
A 400–600mL beaker was filled with water and placed on a hot plate to create a hot water bath and a

Reaction Lab Report Essay
To perform the experiment, we had to carry out this experiment in well–ventilated area because the volatile unknown liquid could have been
flammable, toxic, or irritant. In addition to that, we also had to wear department safety goggles, avoided skin/clothing contact, and most importantly,
tried not to inhale any of the vapor. Now to actually perform the experiment, we placed a boiling stone into a 25 mL Erlenmeyer flask. Using a small
piece of aluminum foil and a rubber band we sealed the mouth of the flask. We pinched a small hole in the center of the aluminum foil, and we
measured the mass of the dry flask, boiling stone, and foil cap to the nearest 0.001 g. We obtained about 25mL of an unknown volatile liquid using a
10 mL graduated cylinder. We meticulously took... Show more content on Helpwriting.net ...
We fasten a clamp to the neck of the flask, covering the foil cap with the clamp. We prepared a hot
–water bath by placing approximately 150–200 mL
of tap water into a 400 mL beaker. We attached a support ring to a ring stand. We placed the beaker through the ring. Adjusted the ring to stabilize the
beaker while it was sitting on a hot plate. We suspended the flask at a slight angle, up to its neck in the water bath, making certain that the water never
touched the foil cap. To suspend a thermometer in the water we rolled a piece of napkin paper, and used a clamp to supported to the apparatus, making
certain that the thermometer bulb didn't touch the bottom of the beaker. We turned on the heating plate, and boiled the water in the water bath. We
waited for the whole unknown liquid to vaporize, and recorded the water–bath temperature. As soon as the liquid completely vaporized, we removed
the clamp–flask assembly from the water bath. We turned off the hot plate. By holding the flask and its contents under cold tap water we cooled
down. After the flask cooled down, and the flask vapor condensed back into a liquid, we removed the clamp from the

Lab Report On Titration
Introduction: The Objective of the lab is to determine the mass percent of ascorbic acid in a vitamin C tablet by titration with a sodium hydroxide
solution of known concentration. A titration is a procedure in which we measure the volume of a solution of a solution of known concentration that is
needed to completely react with volume of NaOH analyzing. A buret is used to measure the amount of NaOH intitration and it is a piece of calibrated
glassware used to accurately deliver volumes of a liquid or a solution. To determine when the neutralization reaction is complete by adding an acid–base
indicator(Phenolphthalein) and it changes color at the end point. To calculate the mass percent ascorbic acid in the sample by using mass of ascirvuc
acid, gmass of sample, g100%. Materials: Mortar
Pestle
Vitamin C tablet
2 Erlenmeyer flasks 250 mL
Balance
50 mL buret
Buret clamp
Support stand
250 mL beaker
Short –stem funnel
Sodium hydroxide(NaOH)
150 mL dry beaker
Stirring rod
Phenolphthalein solution Procedure: 1.Two 250 mL erlenmeyer flasks was labeled 1 and 2 and weighted
2.Vitamin C tablet was crushed into powder and transferred roughly equal into the labeled erlenmeyer flasks.
3.The mass of erlenmeyer flasks that contained the powder of vitamin c was measured.
4.The buret was mounted on the support stand by using the buret clamp.
5."Discarded solutions" was labeled on a 250 mL beaker.
6.The stopcock of the buret was

Police Need The Identity Of An Unknown Substance Essay
Introduction
Forensic labs are often called into action when police need the identity of an unknown substance to be identified as it could be an illicit drug. There are
two major types of tests that can be performed. One is presumptive tests, which indicate the type of substance used, and the other is a confirmatory test,
which actually determines the identity of a substance (Watson, 2008).
Recently, new drugs have appeared in the illegal drug market. The new substances claimed to contain "non–Illegal" compounds yet still deliver the
psychoactive effects desired. This new class of compounds are now commonly known as "SmartDrugs" and are distributed through internet commerce
or "Smart Shops". Some of the drugs included in the mixtures are cathinones and trytamine analogs of psylocin. The current method of identification is
toxicological screening and is proven to have some ineffectiveness at identifying the new compounds. However, new advances in mass spectrometry are
expected to broaden the diagnostic spectrum of the toxicological screening, capable of detecting hundreds of compounds at nanomolar levels. New
liquid phase separation techniques are coupled with the mass spectrometry for high accuracy at identification (Favretto, 2013).
Other than mass spectroscopy, other methods for the identification of unknown inorganic compounds come from other tests, such as the flame test,
solubility test, conductivity test, and pH test. There are also tests using gravimetric analysis,

Erlenmeyer Flask Synthesis Lab Report
Get a hot plate, two 50 ml Erlenmeyer flask, and a magnetic bar. Set up the hot plate under neither the fume hood and put on low heat. Using the
pipettes provided, gather .4 ml of salicylaldehyde and place it in one of the 50 ml erlenmeyer flask. With the other 50 ml erlenmeyer flask add .2 ml of
ethylenediamine and the magnetic stir bar. Add 10 ml of methanol to each flask, make sure that this step is completed underneath the fume hood, and
swirl the mixtures thoroughly. Once completed carefully add the aldehyde solution to the flask that contains the ethylenediamine solution, this should
result in a cloudy yellow color forming. Then place the flask on the hot plate that's underneath a fume hood and bring the material to a boil. Once
boiling

Separation Of P-Acetamidobenzoic Acid
The objective of this procedure is to produce a sample of p–acetamidobenzoic acid from the oxidation of p–acetotoluidide with potassium
permanganate.
Procedure Part A– Preparation of p–Acetamidobenzoic Acid
In a 250 mL Erlenmeyer Flask, 5 g (0.02 mol) of magnesium sulfate crystals were mixed with 1.9 g (0.013 mol) of p–acetotoluidide in 125 mL of
de–ionized water. The resulting solution was placed on a hot plate and was steadily boiled until the solution reached 85В°C, or until the solution
reached a gentle boil (it was emphasized that the solution should be heated slowly, in order to maximize the efficiency of the reaction). While this was
occurring, a separate solution was prepared from 5.1 g (0.032 mol) of potassium permanganate and 20 mL of boiling water, which were placed in a
separate 250 mL beaker, which was placed on a slowly heating hot plate (in order to keep the solution as warm as possible, but not warm enough that
the water could evaporate). It was observed that this solution was characterized by a very distinct purple color, and a small amount of precipitate
could be observed at the bottom of the beaker. Once the p–acetotoluidide solution had reached a gentle boil, it was vigorously stirred with a stirring
rod, and every so often (about every 5 minutes) a small portion of the potassium permanganate solution was added to the solution; at this point, it was
emphasized that the potassium permanganate solution, or the oxidizing agent, should be added in small

Methods And Analysis
CHAPTER THREE
MATERIALS AND METHODS
3.1 Equipments
The equipment used were FAAS (AA 6300 Shimadzu), XRD (D2 Phaser Model– Bruker), centrifuge (Eppendorf 5810), Fisher brand test sieve aperture
250 microns (ISO3310/ 1.mill), XRD mccrone micronizing mill (Glen creston company), EDX spectrometer (800HS), XRF model (S1 titan), electric
shaker model SHR–2D and model D–3162, electric weighing balance (ATY224 Shimadzu), muffle furnace Eisklo type LN 120, aspirator pump (model
7049–05), water still (model WSB/4), grinding mill model Reutsch SR 200, FTIR (model IRTracer– 100), fabricated ball mill, UV–VIS model
(Specord 200 plus), pH meter (Starter 2000) and scanning electron microscope (SEM) model (Zeiss Evo LS 15).
3.2 Chemicals
Pb (NO3)2, ... Show more content on Helpwriting.net ...
Alumina, silica and other constituent components in the ashes were analysed in situ using the method described by (KГјpper et al., 2000).
3.5 Synthesis, functionalization and characterization of geopolymer
3.5.1 Synthesis of geopolymer samples
The procedure was adopted from LГіpez et al. (2014) but with slight modifications. 20 g of rice husk ash (RHA) was weighed and placed in three
different 250 mL Erlenmeyer conical flasks. Alkaline activating solution of sodium hydroxide was prepared 24 hours prior to mixing with calcined
clays (Ferone et al., 2013). 100 mL of 8.0M NaOH was added in each conical flask and the mixture stirred using a magnetic stirrer for 15 minutes. 50 g
of calcined clays (CC) was weighed and added to each of the three Erlenmeyer conical flasks labeled GP–1, GP–2 and GP–3 respectively. The mixtures
were then transferred to 250 mL plastic bottles and shaken in a ball mill for 5 hours (LГіpez et al., 2014). The fluid matrix was then poured into
ceramic crucibles and cured in an oven at a temperature of 80 В°C for 12 hours. The temperature conditions was then adjusted to 200 В°C for another
12 hours to facilitate complete polycondensation (LГіpez et al., 2014). The ultimate geopolymer materials obtained were washed with distilled water
severally to a pH of 7.0 В± 0.5. Filtration was then done using aspirator pump model 7049–05. The residues were

Qualitative Observation Of A Chemical Reaction Lab Report
Qualitative Observation of a Chemical Reaction
Purpose: Carefully observe and interpret a chemical reaction.
Apparatus:
Equipment– 250mL beaker, 125mL Erlenmeyer flask, cardboard square, chemical scoop, metric ruler, lab countertop, rubber stoppers, safety goggles,
lab apron
Materials– candle ( 2cm diameter), matchbook, 2 toothpicks, Limewater solution, string, aluminum foil, Cobalt Chloride paper
Procedure:
Note appearance, odor, and feel of the unlighted candle.
Heat the bottom of the candle and secure it to a cardboard square on your lab counter. Light the candle and allow it to burn for several minutes. Note
any changes. Briefly describe the burning candle.
Blow out the flame and immediately place a lighted match in the "smoke" ... Show more content on Helpwriting.net ...
– During: The wax began dripping down the sides of the candle once the wick was lighted. The flame was blue at the bottom and ombred up to yellow
at the top of the flame. The flame was jumpy and not steady.
– After: Liquid wax was puddled around the wick of the candle.
– Results: When a lighted match was held 2cm away from the unlighted candle in its smoke, the flame would jump from the match to the wick having
been carried by the smoke.
Test 2 (procedure 4)
– Before: There were more wax drips down the sides of the candle.
– During: The liquid wax was exposed to the heat of a lighted match.
– After: The liquid wax underwent a physical change after being exposed to the heat of the match.
– Results: When liquid wax is exposed to the heat of a match, it transforms back into its original solid state.
Test 3 (procedure 5)

– Before: The area around the wick was all solid wax instead of liquid wax as in previous tests. The wood toothpick was placed in the solid wax around
the wick.
– During: The toothpick was lighted using a match and began to burn, but not for very long.
– After: Only the top of the toothpick was burnt. The candle remains in the same shape as it was at the beginning of the test.
– Result: Once the toothpick had been lighted, the flame went out before it hit the body of the toothpick. Only the tip of the toothpick had been
exposed to the

Analysis of a Commercial Bleach Essay
Analysis of a Commercial Bleach
Purpose: The purpose of this lab is to determine the amount of sodium hypochlorite (NaClO) in commercial bleach. This can be done by forming
triiodide ions. To make the measurement more accurate, starch was added to help determine the endpoint of the solution. The significance of this lab is
that industry can use these techniques to determine the amount of NaClO in the bleach of the rival industry and improve it.
Hypothesis: The hypothesis is that, an accurate determination of NaClO in commercial bleach can be done. By mixing the acidified iodide ion to the
hypochlorite solution, the iodide is oxidized to iodine which forms complex triiodide ions that give the red–brown color to the solution. Because the ...
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moles Na2S2O3
Moles of ClO– in diluted bleach = (Average moles added) Г· 2
(1.383 Г— 10–3) Г· 2 = 6.915 Г— 10–4 moles ClO–
Average molarity of ClO– in diluted bleach = (Moles of ClO– in diluted bleach) Г· (Volume of diluted bleach)
(6.915 Г— 10–4) Г· 0.025 = 0.02766 M ClO–
Molarity of the original bleach = [(Average molarity of ClO– in diluted bleach) Г— (0.100 L)] Г· (Volume of original bleach)
(0.02766 Г— 0.100) Г· 0.005 = 0.5532 M ClO–
Mass of NaClO = [(Molarity of the original bleach) Г— (Volume of original bleach)] Г— (Molar mass of NaClO)
(0.5532 Г— 0.005) Г— 74.44 = 0.2059 g NaClO
Mass of

Synthesis Of Acetaminophen Lab Report
o prepare Acetaminophen a water bath was set up in a 400–mL beaker and then placed onto a hotplate where it reached a boil. During the time it took
for the water bath to boil, a 125–mL Erlenmeyer flask was obtained. P–aminophenol (1.5g) was weighed and then placed inside the Erlenmeyer flask.
Deionized water (25 mL) was added to the flask followed by 35 drops of concentrated phosphoric acid. An additional 15 drops were added to the
solution, since the initial 20 drops of concentrated phosphoric acid was not dissolving the p–aminophenol. Phosphoric acid was added to the reaction
mixture because it acted as a catalyst for the reaction. The flask was then swirled gently until all of the p–aminophenol had dissolved. Once the water
bath came to... Show more content on Helpwriting.net ...
The calculated theoretical yield of the product was 2.12g. This was calculated by identifying the limiting reactant of the reaction to be p–aminophenol
and then by multiplying its number of mols by the mass of acetaminophen. The percent yield of the product was 43.4%. The percent yield was
calculated by the dividing the theoretical yield (2.12g) by the actual yield (0.92g). Some reasons that could have caused the percent yield to be less
than 100% could have been from the crystallization and the filtration process. During the crystallization process, some of the acetaminophen may
have not fully crystallized resulting in a lower mass of both crude and purified acetaminophen. This would have caused our calculations to become
less accurate. Additionally, during the filtration process, crystals could have been lost due to them being stuck to the filter paper that was being used.
After completely filtering the crystals, there was a thin layer of crystals that were stuck to the top of the filter paper. This would have caused a lower
mass of both crude and purified acetaminophen since the crystals that were stuck to the filter paper were not weighed. This could have been a cause
for the 43.4%

Electrophilic Aromatic Substitution And Column...
Experiment FIVE: Electrophilic Aromatic Substitution and Column Chromatography Reaction Procedure A hot plate was preheated to 100В°C. A dry
5–mL long–neck round–bottom flask was clamped over an aluminum block placed on the hot plate. Ferrocene (0.09 g), acetic anhydride (0.35 mL),
and 85% phosphoric acid was added to the flask in that order of addition. A magnetic stir bar was added to the flask. Solution was stirred and
heated for 10 minutes. Flask was removed and allowed to cool to ambient temperature. DI water (0.5 mL) was added and the solution was cooled to
0В°C by ice bath. The solution was neutralized with 3M sodium hydroxide dropwise while stirring and cooling. PH was monitor by pH indictor paper.
Solid product was isolated by vacuum... Show more content on Helpwriting.net ...
The yellow band, ferrocene, elute from the column with the like non–polar phases of hexanes. Theoretically speaking an additional orange band,
representing acetylferrocene, should have eluted after the shift in mobile phases. Considering that the mobile phase changes from a non–polar content
to that of higher polarity with the addition of ethyl acetate, it is logical that a polar species like acetylferrocene would elute. After collecting and
evaporating the solvent portion of the darkest yellow fraction, the resulting mass was 0.017 g, an 18% yield from the starting the amount. This yield
could be raise if the additional yellow fractions were collect. The melting point of this collected fraction was 170В°C, which reasonably close to the
literature value of 172. Considering that the species sampled was the started reactant, thus there was no chemical change, it safe to assume the purified
product is

Molarity Of Hcl
This experiment is designed to demonstrate how to use volumetric tools and how to calculate the molarity of an unknown based on the usage of these
tools. Volumetric tools include burets, pipets, and volumetric flasks and can be used to react an unknown substance with a substance of known
concentration to find the molarity of an unknown. This specific experiment sought to find the concentration of an HCl solution by reacting it with a
standard NaOH solution. An indicator was added to show when this reaction had occurred (Beran 2012). The hypothesis predicted that the molarity of
the unknown substance would have a concentration of HCl that lied between .07M and .09M. This was based on the prelab activity with practice
calculations that had numbers ... Show more content on Helpwriting.net ...
This is most likely because the hypothesis was based on the pre–lab activity, which had calculations very similar to the predicted molarity range, though
was not actually based on the experiment performed. Additionally, the standard deviation indicates that the data is quite precise, with a deviation of
only .002. This deviation could be due to slightly inaccurate measurements, potentially caused by instruments that were not cleaned properly or NaOH
not falling into the Erlenmeyer flask when it was being swished during titration. For example, the buret may not have been rinsed to the fullest extent,
causing minor contamination. However, small errors are inevitable in experiments and can only be minimized.
Conclusion
This experiment appropriately exemplified how to use volumetric instruments when finding molarity of an unknown concentration. It also showed how
to calculate the molarity of one substance based on titration recordings. Although the data had small divergence, the data recorded was still fairly
precise due to an experiment with minimal user

Lab Assignment On The Heat Transfer Lab
Heat Transfer Lab Assignment
SCH 4U1
Brad Bonner
Mrs. Hsia
August 30, 2017
Question: How does increasing the temperature of water affect the temperature of the entire solution? Hypothesis: If the temperature of the water
increases, then the temperature of the entire solution slowly increases because there is an increase in kinetic energy in water, so when thermal
equilibrium is reached, the temperature of the solution is higher and the water exchanges the heat with compound Y and the total temperature rises.
Materials
2 250 mL Erlenmeyer flasks
150 mL Distilled Water
300 mL of Compound Y
Variables Independent: Temperature of water
Dependent: Temperature of solution
Control: Volume of Water Volume of Compound Y Temperature of Compound Y
Procedure:
1.In the Stockroom, click on the Glassware tab and select a 250 mL Erlenmeyer flask. It will appear on the lab bench.
2.Right click on the flask and then click on Rename. Name this flask "Water".
3.Return to the Stockroom. Click on the Solutions tab. Add the 3000 mL of Distilled Water container to the lab bench.
4.Click and hold the carboy of Distilled Water and move it over on top of the flask marked "Water." A measurement box will appear. Transfer 50.00
mL of distilled water into the flask. Return to the Stockroom.
5.In the Stockroom, add the Erlenmeyer flask containing 100.00 mL of Compound Y to the lab bench. Assume that Compound Y has a

Chemistry Experiment : The Experiment Of An Erlenmeyer...
In part one of the experiment, Flourene (0.1 g, 0.0006 mole) was measured and added to a 25 mL Erlenmeyer flask. Next, 10 M of NaOH (7 mL, 0.2
mole) was added to the flask with a ВЅ inch stir bar. The mixture was stirred until the fluorene dissolved completely. Then, Stark's Catalyst, Aliquat
336 (5 drops) was added to the solution. The color of the solution turned yellow and two layers formed. The reaction was then stirred vigorously.
Next, a comparison TLC was conducted against the starting material in a 20% dichloromethane and 80% hexanes solution. The reaction stirred for 5
minutes and after that a TLC was conducted. The mixture was not complete and after another 5 minutes another TLC was conducted. Next, the
reaction was poured into a separatory funnel and the organic layer was separated from the aqueous layer. Then, 5% HCl (5 mL) was added to the
separatory funnel to wash the organic layer, this was repeated two more times. Next, saturated NaCl, Brine (5 mL) was added to the separatory funnel
and was drained. The organic layer was then poured to an Erlenmeyer flask and Na2SO4 was added to dry it. The organic layer dried for 5 minutes then
a gravity filtration was conducted to remove Na2SO4. The filtrate was collected in a pre–weighed 100 mL beaker (46.7208 g). Na2SO4 was rinsed
with toluene (3 mL) twice. The beaker was labeled and placed in the hood. In part two of the experiment, alumina (12 cm) was measured in the column.
Next, the measured alumina was poured into

6.03 Calorimetry Lab
If there is an additional unmeasured amount of water in the Erlenmeyer flask, then this would reduce the concentration of the HCl, and therefore reduce
the molarity. The volume of the amount of HCl solution added would increase, yet the concentration of the HCl would remain the same, which would
ultimately result in the molarity of the HCl being lower than in reality.
If there is an additional unmeasured amount of HCl in the Erlenmeyer flask, then this would increase the concentration of the HCl, and therefore
increase the molarity. The number of moles of HCl in the solution would increase, which would increase the molarity of HCl in the solution. This will
ultimately result in the molarity of the HCl being recorded as higher than it should be.
If the NaOH managed to absorb water before measured, then the measured mass of the NaOH ... Show more content on Helpwriting.net ...
A higher volume of NaOH will result in more moles of NaOH being added to the HCl, which results in more HCl reacting. This makes the calculated
molarity of the HCl be smaller than the actual molarity of the HCl.
Adding three drops of phenolphthalein instead of two drops to the HCl will result in small differences to the molarity of the solution. Since volume
(phenolphthalein) is being added to the solution, the molarity of the HCl solution is expected to drop. This will make the calculated number of HCl be
slightly smaller than the actual value of the original HCl solution.
If an air bubble was present in the buret during titration, it would affect the calculated molarity of the HCl. The air bubble takes up volume in the buret,
making the volume of NaOH in the buret artificially high. If the bubble came out during titration, then the volume of the NaOH added would appear to
be higher than what it actually was, and would ultimately result in the calculated HCl concentration be higher than what it actually

Vinegar Lab Report
How Much Acetic Acid Is in Vinegar?
The chemical makeup of certain acids and bases that are not managed reacted properly can be harmful and a result of improperly measured acids
and bases. This could have a negative effect on humans pertaining to different liquids that could be consumed or physically hazardous to the body.
However, due to decades of research in the department of science, it can be confirmed that ideas like the HSAB Principle and the Lewis Principle
help categorize acids and bases between being harmful or not and secondarily help humans be more cautious, according to professor Tse–Lok Ho.1
However, experimental these measurements can be specified and determined through titrations. According to Jakub Ederer and other researchers,
titrations have quick and determinable results and do not require a lot of money and are commonly used for acids.2 The Lab Manual provides an
experiment that includes a titration to determine the moles of acetic acid (HC2H3O2) in a specific amount of vinegar.3 To follow through with this
experiment, the acid–base reaction has a known molar concentration of NaOH solution that reacts with an unknown molar concentration of acetic acid
to make water and NaC2H3O2, resulting in a titration. Before the initial trial titration, a thorough cleaning procedure of the buret and materials was
necessary to ensure there is no contamination of other chemicals or solutions. The buret was washed out with soap, tap water, and distilled water with no

Grignard Reagent From An Unknown Aryl Halide
7) Discussion:
In this experiment, the goal is to prepare a Grignard reagent from an unknown aryl halide and identify the identity of the aryl halide by converting it to
a carboxylic acid to determine its melting point and molar mass (determined by titration). The experiment began by dissolving 0.25g of magnesium
powder in a 25mL round–bottom with 5mL of anhydrous ether and stirring with a stir bar. Then the round–bottom flask was set up for reflux using a
Claisen adapter where the vertical part is covered with a septum to prevent air from mixed with the solution. The septum is very important because the
Grignard product can react with oxygen to produces a carboxylic acid, which is not wanted. Also, the choice of anhydrous solvent is important because
the Grignard product can react with water to produce an alkane. With the reflux set up, the next step was to add the halide. 1.2mL of the unknown
bromoarene mixed with 2.5mL ether was slowly added dropwise through the septum using the needle and syringe. The bromoarene had to be added
slowly because there Grignard product would undergo another unwanted side reaction by reacting with the unknown bromoarene. The product with be
a new carbon–carbon bond between the unknown bromoarene and the Grignard product. If the bromoarene is added slowly, the chances of the
Grignard product reacting with the bromoarene over the magnesium is low because magnesium exists in larger concentration in the solution. Once all
the unknown bromoarene

Trimyristin Synthesis Lab Report
Objective: To isolate trimyristin from Nutmeg and purify trimyristin recrystallization from acetone.
Procedure:
Weigh out 4.00 g of nutmeg powder directly into a 50 ml Erlenmeyer flask.
Add 25 ml of diethyl ether and swirl periodically for 15 minutes.
(Do this in the fume hood)
Label a 50 ml vacuum flask and weight it to 4 places.
Support the labeled 50 ml vacuum flask using a ring stand and clamp.
Place a sintered funnel with a vacuum adaptor on the labeled flask.
Filter the solution by pouring the nutmeg/diethyl ether mix onto the sintered funnel.
Wash the Erlenmeyer flask with1–2 ml of diethyl ether and add it to the residue on the sintered funnel. Do this 3 times.
Evaporate the solvent using the airline in the fume ... Show more content on Helpwriting.net ...
Determine the percent recovery from recrystallization
Pure product / crude product x 100
0.94 g / 2.3 g x 100 = 40.9 ~ 41%
2.If the melting point of the purified trimyristin was done before it was completely dry, what would be the effect on the melting point and why?
If it wasn't dry and we took the melting point, we would want to know that it would still have an impurity, thus having a lower melting point
3.If the crude trimyristin were a white solid, would you have used norite? Explain.
We wouldn't have used norite because it is only used for colored impurities.
4.Assume the amount of trimyristin in nutmeg is 20% by weight. What would be the expected amount to be recovered from the 5.00 g of nutmeg?
Calculate your percent recovery using the 'expected recovery' amount.
1.00 g / 5.00 x 100 = 20 %
5.Why was acetone a good solvent to recrystallize the trimyristin? What were the disadvantages?
Acetone is a good solvent because it yields a pure compound, thus making trimyristin soluble hot, and insoluble cold. The disadvantages are that
acetone has a low boiling point and the solubility makes no difference in the compound.
Conclusion

All in all, I was able to dissolve the nutmeg and extract trimyristin. Upon doing the calculation, 41% of trimyristin was

Lab Report On Ascorbic Acid
Introduction
Vitamin C (ascorbic acid) is an essential nutrient used for the creation of certain biological compounds and is naturally found in citrus fruits. 1
Ascorbic acid has a chemical formula of CВ¬В¬6H8O6 and reacts with Iodine to cause the reaction:2 C6H8O6(aq) + I2(aq) –> C6H6O6aq)
+2IВ¬–(aq) + 2H+
To determine the amount of vitamin C an amount of KIO3 solution with a known concentration had it's iodine "freed" with the chemicals KI and
H2S04, this allowed the iodine to react with the dissolved vitamin C tablet. This was then titrated against a primary standard of sodium thiosulfate at a
concentration of 0.01102*10–5В¬В¬M. These chemicals cause the following reactions3:
KIO3(aq) + 5KI(aq) +3H2SOВ¬4(aq) –> 3I2(aq) + 3K2SO4(aq) + 3H2O(l)
2Na2S2O3(aq) + I2(aq) –> 2NaI(aq) + Na2S4O6(aq)
Since the volume of KIO3 solution and so is the molarity we can determine the amount of KIO3 solution that was freed. We can then compare that to
the amount of primary standard used to determine the amount of Ascorbic acid in the solution.
Procedure
The procedure given in the First YearChemistry Lab Manual for Experiment G4 was followed with the modifications below.
Instead of using a 500mL volumetric flask a 1L volumetric flask was used. This made calculations that required Liters (L) easier as the numbers could
be carried without doing any math. This also made the experiment more accurate. Even though the absolute uncertainty increased so did the volume of
the container, this meant that

Lab Report Chemistry Lab
MATERIALS
Erlenmeyer flask (125 mL)
Agarose (0.75g)
Scoopula
Weigh boat
Digital scale
Graduated cylinder (50 mL)
Pieces of aluminum foil
Vials of DNA samples (14): o lambda Hind III/ Eco RI (4) o mutated (2) o wild type (2) o child #2 (2) o child #1 (2) o No DNA (2)
Masking tape
Stirring rod
Mitton–like gloves
Hot plate
Well–forming comb
1Г—TAE Buffer (50mL)
Power Supply (150V)
Gel Electrophoresis Chamber
Gel Tray
Pipets (6)
Latex gloves
Permanent marker
Metric Ruler
Clock or stopwatch
PROCEDURE
1.Use a weigh boat and scoopula to measure out 0.75 g of agarose onto a digital scale. Make sure to tare the digital scale before weighing the powder.
Pour the powder into a 125 mL Erlenmeyer flask. ... Show more content on Helpwriting.net ...
Firstly, if the well–forming comb was not situated in the proper position, wells could have formed improperly. DNA bands would appear faint or

there would be none at all. If the student were to plunge different DNA samples into the improperly formed wells, an insufficient concentration of
DNA would be loaded into the gel, thus resulting in an unclear visualization of the DNA fragment positions. Low concentrations of DNA inserted
into each well would result because of the little volume of DNA in the well width. Secondly, strayed DNA fragment visualizations may also be a
result of more or less agarose powder. If there is more agarose, then high negative DNA molecules will not get as far to the other side of the
positive end of the gel than the gel with less agarose powder added into the 1.5% Agarose solution. Tiny sugar molecules of the agarose solution
act as obstacles to the DNA molecules that transport to the positive end of the gel. Lastly, if the gel runs too long or not enough by electric
currents, the gel model will be different from the ideal model. If the gel runs too long, DNA molecules or bands will reach the positive end of the
gel and run and disappear into the buffer. If the gel runs too little, DNA molecules or bands will clump or not get far to the positive end of the gel as
they should because the electric currents are the modes that move the DNA molecules. Hence, the three possible errors

The Acidity Levels Of Organic Tomatoes And Commercially...
Introduction
We decided to do a project concerning the acidity in organic tomatoes and commercially grown tomatoes. Originally, we wanted to use home grown
tomatoes compared to commercially grown tomatoes, but unfortunately the weather is not conducive to grow tomatoes in a home garden during this
time of the year. We choose this experiment because we wanted to determine if there is a significant difference in theacid of the tomatoes. In addition,
in determining the acidity level of the two groups and comparing them could help individuals determine which type of tomato to purchase when
canning foods or if someone is concerned about underlying health issues. We hoped to determine one group of tomatoes to have a much lower acidity
level ... Show more content on Helpwriting.net ...
In addition, for a titration to be successful it must turn the faint pink color with one single drop being added. Finally, measure the final reading of the
buret after finishing the titration, and note the reading.
Calculate the molarity of the base from the volume of titrant and mass of oxalic acid. Then, titrate more samples until the molarity of the calculations
are within five percent. Neutralize the waste solution in the waste beaker to a pH between 6 and 8 with 0.5 HCl if too basic or 0.5 M NaOH if too
acidic. Measure the pH level with the pH meter to determine which should be done. Discard the solution in the sink when it has been neutralized. This
part of the experiment is performed to help hone in on titration skills, so the individual could collect precise measurements to calculate precise
calculations.
Data and Results of NaOH
Trial 1Trial 2Trial 3
Mass of Hв‚‚Cв‚‚Oв‚„0.192 grams0.193 grams0.190 grams
Moles of Hв‚‚Cв‚‚Oв‚„0.00150.00150.0015
Moles of NaOH0.0030 0.0030 0.0030
Initial Buret Reading1.2 mL1.2 mL3.44 mL
Final Buret Reading33.2 mL32.5 mL33.12 mL
Volume of NaOH32.0 mL31.3 mL29.68 mL
Molarity of NaOH0.0938 M0.0958 M0.1011 M

Sample Calculation
Procedure Part 2 First, put on safety equipment (goggles and gloves). Next, set up the buret stand, and place the buret on the stand. Next, obtain
approximately 250 mL of pure tomato juice in a 250

Dichlorometry Lab
To begin the experiment, 0.565g of the chemical mixture (Excedrin tablet) was weighted using an analytical balance; then, the mixture was placed
on a 20ml beaker. A vacuum filtration was set up using s Hirsch funnel and a 25ml filter flask. Then, 8ml of dichloromethane was added to the
mixture in the 20ml beaker. The reaction mixture was stirred a few times using a glass stirring rod. Next, the solution was filtered through a filter
paper placed in the glass funnel. The 20ml beaker was washed with dichloromethane to collect the solid left in the beaker. The filtered solution was
collected in the 25ml filter flask. Then, the filtered solution was transferred to a clean centrifuge tube and the solid compound was transferred to a
clean test... Show more content on Helpwriting.net ...
The solution was stirred with a boiling stick after a few drops, until the solution tests acidic with pH paper (red). Two more drops of hydrochloric
acid were added to the solution. The liquid was removed from the reaction tube using a Pasteur pipette. To recrystallize aspirin, 3ml of water was
added to the test tube, the mixture was heat until it was dissolved. Then, the solution was place in an ice bath to induce crystallization. Aspirin crystals
were collected via vacuum filtration with a Hirsch funnel. Then, aspirin crystals were weighted to calculate percent yield and saved to perform TLC

Business Level 3 Unit 9 M1
Task 1: M1
Vacuum Filtration:
Vacuum filtration is the method of separating a solid product from a liquid or solution mixture. The mixture is poured through a Buchner funnel
containing filter paper. The filter paper holds the solid particles and the liquid draws through the funnel into the flask below.
In order to carry out the vacuum filtration you must first prepare all the equipment required such as access to a fume cupboard, a Buchner funnel, tubing,
filter paper, cleaning solvent, disposable dropper, vacuum flask and your sample of aspirin.
Firstly set up the equipment as shown in the diagram opposite.
Next clamp the vacuum flask securely to a clamp and stand, attaching the Buchner funnel to the top with the use of a rubber funnel ... Show more
content on Helpwriting.net ...
Next prepare the third test tube with an accurate measurement of 5ml sodium carbonate once again labelling appropriately.
Then in the last test tube fill it up with 5ml of sodium sulphate. Then after that carefully pour the sodium carbonate solution into the test tube labelled
copper chloride solution examining the result and recording appropriately.
Next you need to carefully pour the sodium sulphate solution into the second test tube containing copper chloride again making a note of the reaction
that takes place. In order to get accurate results you must ensure that none of the solution is spilt if a spillage were to occur you must ensure you clean
it up appropriately and begin the process again.
Finally ensure that your results are accurate. You should have a light blue precipitate remaining when the sodium carbonate reacts with the copper
chloride and when sodium sulphate ionises with copper chloride no precipitate should have formed.

Benzophenone Lab Report
Benzophenone (1.00g, 0.0054 mole) was measured and added into a 100 mL round–bottom flask. Next, 95% of EtOH (15 mL) was measured and
placed in the round–bottom flask and a stir bar was added. The mixture was heated on a sand bath until the benzophenone dissolved completely. The
round–bottom flask was removed from the sand bath and it cooled for a few minutes. A preliminary TLC was conducted with 20% ethyl acetate
and 80% hexanes solution. Next, NaBH4 (0.100g) was measured and added to the solution when it cooled. Five minutes after adding NaBH4 a TLC
was conducted. The TLC was not pure and had two spots with Rf of 0.48 and 0.36. Another TLC was conducted after five minutes and there were
two spots with Rf of 0.49 and 0.39. Next, an ice bath was prepared by filling a small... Show more content on Helpwriting.net ...
Benzophenone was reduced with sodium borohydride to get benzhydrol. The carbonyl compound with sodium borohydride transferred a hydride ion
from metal to electropositive carbon of the carbonyl. After the addition of sodium borohydride, a comparative TLC was conducted and it showed that
there was impurity and the reaction was not completed. The reaction was monitored by conducting a TLC every 5 minutes. As the minutes went by the
spot at the top started to get smaller and eventually disappeared. After the final comparative TLC, the product was The IR spectra was different for the
two compounds. The starting material, benzophenone, had an alkene(=C–H) stretch at 3051.11 cm–1, ketone (О±, ОІ–Unsaturated) at 1641.75 cm–1,
and an alkane (–C–H) stretch at 1444.44 at cm–1. The product, benzyhdrol, had an alcohol (O–H) stretch at 3353.75 cm–1, alkene(C=C) stretch at
1642.04 cm–1, alkane stretch at 1443.57 cm–1. The product, benzhydrol, had a melting point of 65.6–66.2 ВєC, theoretical yield of 0.0054 mole, and
percent yield of 84

Essay about Determination of the Composition of Cobalt...
Determination of the Composition of Cobalt Oxalate Hydrate Experiment 12 Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312–D TA's: Russell
Dondero & Sylvester Mosley February 9, 2000 Purpose The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with
that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O. Procedure The powdered cobalt
oxalate hydrate was weighed to about 0.3 g and placed in a pre–weighed crucible. The crucible and the cobalt oxalate were then heated until the cobalt
oxalate decomposed into a stable, black solid, or Co3O4. Once the crucible was sufficiently... Show more content on Helpwriting.net ...
|trial one |trial two | |Mass of cobalt oxalate hydrate |.3012g |.3027g | |Mass of residue (Co3O4) |.1777g |.1752g | |Percent Co in Cobalt Oxalate
Hydrate |43.33% |42.509% | |Average percent |42.92% | | | | | |Standardization of KMnO4 Solution | | |Concentration of Standard Na2C2O4 |.1mol/L |
|Volume of Na2C2O4 dispensed |15.0mL | |Volume of KMnO4 required |34.3mL | |Molarity of KMnO4 solution |.0175 mol/L | | | | | |Determination
of Oxalate | | | |Mass of cobalt oxalate |.3091g |.3031g | |Volume of KMnO4 used |38.6mL |37.1mL | |Percent oxalate in cobalt

Solubility Equilibrium and the Effect of Temperature Essays
Introduction For this experiment, we are going to determine the effect of temperature on solubility, to be done in a chemical by dissolving a solute in a
definite amount of solution which is saturated. Specifically, the goal of this experiment is to prepare a saturated solution of Na2C2O4 in water at
different temperatures, determine the effect of temperature in solubility, and to apply Le Chatelier's Principle. We can do all this by simply titrating a
certain amount of standard KMnO4, and measuring how much KMnO4 was needed to help Na2C2O4 reach chemical equilibrium at certain
temperatures. In doing this, we will have fulfilled all the goals of our experiment, as well as being able to determine the Solubility of Na2C2O3 at
both 20 and ... Show more content on Helpwriting.net ...
I then added 50 ml of distilled to the test tubes A1, B1, C1 and D1, then titrated them with the potassium permanganate solution (making sure to add 15
ml 3M sulfuric acid in each), then recorded the amount it took for them to turn pink.
Data
A. Standardization of KMnO4 solution:
Sampleg Na2C2O4moles Na2C2O4 (x 10^–3)moles KMnO4 (x 10^–3)ml KMnO4 usedM KMnO4
#1.473.511.415.5.090
#2.503.731.516.093
Average M = .091
B. Solubility of Na2C2O4 at different temperatures: in M and g/ L.
Sample and temp (C):ml of KMnO4 titratedmoles KMnO4 (x 10^–4) moles NaC2O4 dissolved (x 10^–3)M (moles/L) Na2C2O4g Na2C2O4 dissolved
in sampleg / L Na2C2O4
A1 В– 35.04.551.14.228.15230.5
B1 В– 31.16.05.461.37.274.18336.6
C1 В– 458.88.012.00.400.26853.7
D1 – 809.58.652.16.432.29057.9
Solubility of Na2C2O4 in g / LExperimental Value in g / LHandbook Value in g / L
At 20 C3637
At 100 C7363.3
C. Relationship of K and ∆H

SampleAverage M of Na2C2O4K=[Na^+]^2[C2O4]ln KT K1 / T K (x 10^–3)
A1.228.047–3.052763.62
B1.274.082–2.50304.13.29
C1.400.256–1.363183.14
D1.432.322–1.133532.83
At 20 C.276.084–2.482933.41
At 100 C.472.421

Chem Lab Essay
Experiment #4A– A Separation and purification Scheme Amena Alkeswani, PHCC Dhanlal Murally, PHCC September 27, 2012 Abstract: There are
millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated,
and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre–designed procedure for every mixture.
So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing
their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the
components of the... Show more content on Helpwriting.net ...
9) Filter the ppt formed as result of step 7 from the newly acidic solution. Then wash the filtered ppt with distilled water. Allow the extracted
benzoic acid to dry. 10) Weigh the extracted benzoic acid and measure the MP. 11) Dry out the methylene chloride solution that contain the
benzoin and the dibromobenzene by the use of anhydrous sodium sulfate. 12) Pipet the remaining methylene chloride to a new beaker. Place the
flask in hot water bath, and boil the methylene chloride out, leaving the benzoin and the dibromobenzene . 15) to separate the benzoin and the
dibromobenzene, a crystallization should be performed 16) Heat some of the hexane to boiling and place the solid to be crystallized into an
Erlenmeyer flask. 17) Pour a small amount of the hot solvent into the flask containing the solid. 18) Swirl the flask to dissolve the solid. 19) Place
the flask on the steam bath to keep the solution warm. 20) If the solid is still not dissolved, add a tiny amount of hexane and swirl again. 21) After
all of the solid dissolves, move the flask from the hot plate and allow it cool to room temperature. After a while, crystals should appear in the flask.
22) place the flask in an ice bath to finish the crystallization. 23) Set up a vacuum filtration 24) Separate the formed crystals (benzoin) and allow them
to dry, then take the MP. 25) Optionally evaporate the mother liquor from pre

Biological Macromolecule Polyhydroxybutyrate ( Phb )
ABSTRACT
The important biological macromolecule polyhydroxybutyrate (PHB) producing Bacillus subtilis was isolated from the sewage sample and identified
by means of 16S rRNA analysis. The renewable nature and biodegradability of PHBs make them suitable materials to replace synthetic plastics in many
applications. Currently their production is expensive, but these plastics are only in their first stage of commercial development. In the present study the
physico–chemical parameters such as Time, Temperature and pH were optimized for increased production of PHB. It was found that maximum
production of PHB was observed at 48th hour (328Вµg/ml) of incubation time, temperature 370C (336Вµg/ml), pH 7.5 (362 Вµg/ml). The low cost
production media was developed using fruit peel extract and sugarcane industrial waste. The amount of PHB produced using low cost production
media in fruit peel (234Вµg/ml) and industrial waste (218Вµg/ml). The PHB was characterized using FTIR and NMR analysis.
Keywords: polyhydroxybutyrate, Bacillus subtilis, optimization, INTRODUCTION The human population has led to the accumulation of huge
amounts of non–degradable waste materials across our planet. The problem of environmental pollution was caused by indiscriminate dumping of plastic
waste has assumed global proportions. They are used in almost all industries, especially for packaging and they account for more than 50% of total
consumption, especially they are used for bottling and baling. They

Acid Concentration
Does the amount of active ingredient in different types of tablets decrease or increase per milligram after its expiration date? Overtime, the
concentration of acid in a low dose aspirin tablet increases, as the concentration of acid in a high dose aspirin tablet decreases. However, due to
various experimental errors, the claim is not a strong and compelling one. What is assumed to have happened is that both low dose aspirin tablets and
high dose aspirin tablets increase in concentration of acid as the expiration is surpassed.
Four different tablets (two new and two expired): Bayer High Dose 325 mg (exp unknown), Bayer High Dose 325 mg (exp 8/18), Bayer Low Dose 81
mg Enteric (exp 4/11), and Bayer Low Dose 81 mg Enteric (exp 8/18) undergo the ... Show more content on Helpwriting.net ...
Firstly, the Bayer High Dose 325 mg tablets used as an "old and expired tablet" is unidentified in expiration date, but the container seems to look very
old. This means that it is uncertain whether the tablets labeled as "old" are actually expired or not (Table 1, 2, and 3). Secondly, not all of the
powdered tablet is put into the beaker. Some remain on the papers while others fly out onto the table. Because not all contents are present during the
titration process, this could very well affect the calculations measuring the mass of acid per

Synthesis Of An Iron ( IIi ) -Oxalate Complex

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