Qualitative Analysis Lab

Qualitative Analysis Lab
CH 204 – Introduction to Chemical Practice Experiment #1 – Qualitative Analysis of Cations Anam
Zaki* Baylee Halliwell TA: Jiawei (Will) He February 16, 2016 RESULTS & DISCUSSION The
purpose of this experiment was to use qualitative analysis in order to identify two cation in a
solution. During the first part of the experiment, the identity of either silver or lead was revealed,
and during the second part, the identity of either calcium or barium was discovered. For the last part
of the experiment, many different cations were exposed when Cation Flame Tests were executed. A
wooden stick dipped into each solution and was held over a flame, and the color of the flame
revealed the cation that was in the solution. For the first part of ... Show more content on
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Silver: Formula Unit:[Ag(〖NH_3)〗_2 ]Cl_((aq))+2H〖NO_3〗_((aq))→AgCl_((s))+2NH_4
〖NO_3〗_((aq)) Total Ionic Equation:〖Ag^+〗_((aq))+〖〖〖2NO〗_3〗^–〗
_((aq))+〖2H^+〗_((aq) )+〖Cl^–〗_((aq))→AgCl_((s))+2N〖〖H_4〗^+〗_((aq))+2
〖〖NO_3〗^–〗_((aq)) Net Ionic Equation:〖Ag^+〗_((aq))+〖Cl^–〗_((aq))→AgCl_((s))
Calcium: Formula Unit: Ca(〖〖OH)〗_2〗_((aq) )+〖K_2 C_2 O_4〗_((aq) )→〖CaC_2 O_4〗
_((s) )+2KOH_((aq)) Total Ionic Equation: 〖Ca^(2+)〗_((aq))+O〖H^–〗_((aq) )+〖K^+〗
_((aq) )+〖〖C_2 O_4〗^(2–)〗_((aq))→〖CaC_2 O_4〗_((s))+2〖K^+〗_((aq))+2〖OH^–〗
_((aq)) Net Ionic Equation: C〖a^(2+)〗_((aq))+〖〖C_2 O_4〗^(2–)〗_((aq))→C〖aC_2 O_4〗
_((s)) REFERENCES Drug Testing in a Drug Court Environment: Common Issues to Address.
https://www.ncjrs.gov/pdffiles1/ojp/181103.pdf (accessed Feb. 14, 2016). Dogancay, D. Flame Tests
Performed Safely: A Safe and Effective Alternative to the Traditional Flame Test. Sci Teach [Online]
2005, 72,
... Get more on HelpWriting.net ...

Chemistry : Chemical Equations For The Reaction Between...
Most of the reactions took time to settle down to form a precipitate as seen in Diagram (1) which
shows the before and after of magnesium hydroxide. Discussion: Chemical Equations for the
reaction between cations and anions Na2CO3 + Mg(NO3)2 –> MgCO3(s) + 2NaNO3 Na2CO3(aq)
+ Ca(NO3)2(aq) –––> CaCO3(s) + 2NaNO3(aq) Sr(NO3)2(aq) + Na2CO3(aq) ===> SrCO3(s) +
2NaNO3(aq) Ba(NO3)2 (aq) + Na2CO3 (aq) ==> 2NaNO3 (aq) + BaCO3 (s) Chromates Calcium
nitrate Ba(NO3)2 + Na2CrO4 ––> 2 NaNO3 + BaCrO4 Barium nitrate Ba(NO3)2 (aq) + Na2CrO4
(aq) –––> BaCrO4 (s) + 2 NaNO3 (aq) Ba(2+)(aq) + 2NO3(1–)(aq) + 2Na(1+)(aq) + CrO4(2–)(aq)
–––> BaCrO4(s) + 2Na(1+)(aq) + 2NO2(1–)(aq) Hydroxide Mg(NO3)2 (aq) + NaOH(aq) →
Mg(OH)2(s) + 2NaNO3(aq) Ca(NO3)2+2Na–OH ––––––––––––>2NaNO3+Ca(OH)2 NaOH(aq) +
Sr(NO3)2(aq) –––> NaNO3(aq) + Sr(OH)2(s) Ba(NO3)2 + 2NaOH ====> Ba(OH)2 ppt +
2Na(NO3) Sulphate Mg(NO3)2 + Na2SO4 – MgSO4 + Na2NO3 Ca(NO3)2 (aq) + Na2SO4 (aq) ⇒
2NaNO3 (aq) + CaSO4 (s) Sr(NO3)2 (aq) + Na2SO4 (aq) → SrSO4 (s) + 2NaNO3 (aq) Na₂SO₄ +
Ba(NO₃)₂ –––> BaSO₄ + 2NaNO₃ Fluoride 2NaF + Mg(NO3)2 MgF2 + 2NaNO3 2NaF +
Ca(NO3)2 –> 2NaNO3 + CaF2 2NaF + Sr(NO3)2 –> SrF2 + NaNO3 2NaF + Ba(NO3)2 –> BaF2 +
NaNO3 Phosphate 3Mg(NO3)2(aq)+ 2Na3PO4(aq)––> Mg3(PO4)2 + 6NaNO3 2Na3PO4 +
3Ca(NO3)2–––>6NaNO3 + Ca3(PO4)2 Sr(NO3)2 (aq) + Na2SO4 (aq) → SrSO4 (s) + 2NaNO3
(aq) Na3PO4 + Ba(NO3)2 –> Ba3(PO4)2 + NaNO3 The aim of this experiment was achieved. The
hypothesis was tested and supported as Group II metal

Thin Layer Chromatography
Chromatography techniques are one of the most useful methods available for the separation or
isolation of organic compound from a mixture. The most common used chromatographic technique
includes column chromatography, thin –layer chromatography (TLC), etc. The purpose of this lab
exercise is using the gel filtration chromatography to separate different proteins from a mixture.
Collecting elutes (run off), and calibrating a curve to show how the column separates molecules by
molecular weight, and identify the molecular weight of the proteins. The sample mixture used in this
lab contained Blue Dextran that has a size of 2x106 Da, and has blue in color. Cytochrome C has a
size of 13,000 Da, pink in color. Potassium Chromate has a size of 192 ... Show more content on
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It is very important not to let the bed run dry during any part of the experiment because the pockets
of air in the bed will cause uneven flow of molecules through the column. Next, 13 clean, dry
cuvettes were collected and labeled 0 to 12. 1mL of water was measured by the P–1000 cuvette and
was transferred into the cuvette that labeled 0 in order to measure the amount of fraction that we
will collect. The sample mixture that included Blue Dextran, Cytochrome of was obtained and was
measured 250 μL by using the P–1000 pipette. Then, the 250 μL was carefully transferred into the
column that already packed. Add the mixture by placing your pipette against the wall of the column
so as not to disturb the bed. The mixture was allowed to enter the bed, close to the bottom the bed
(about 1 cm) by opening the stop cock . Then, about 15 mL of buffer was added into the column.
3mL of buffer added slowly each time to prevent the overflow and avoid disturb the bed. 1 mL
fractions were collected into each cuvette until there is no color present in the last fraction. 1 mL of
fraction was measured by keep the #0 cuvette contained water next to the cuvette that you want to
measure. After, collecting the fraction, the fraction was analyzed and recored the color and the
intensity. Each fraction was given the number based on the scale 0–5 based their color. The bigger
number the darker color they have and more intense. All the waste was discarded to appropriate
waste

Equilibrium Reactions and Le Chatelier's Principle
Lab: 5
Experiment:13
Pre–Lab The purpose of this experiment is to observe an equilibrium reaction counteracting changes
to it's system all in accordance to Le Chatelier's principle. An equilibrium reaction can be pushed
toward products or reactant based on changes in temperature or concentration. The reversibility of
reaction will also be looked at.
Pre–Lab questions
1. The concentrations of products and concentrations of reactants remain constant but both reactions
are still going on, just at the same rate.
2. Le Chatelier's principle when an equilibrium has been established in a system and is altered, the
systems will counteract the change.
3. a) it will go to the left b) to the left c) to ... Show more content on Helpwriting.net ...
If the equilibrium lies to the right, the solution is basic and will be yellow. The first solution turns
pink because the HCl is a strong acid and methyl orange is pink in acidic solutions. The
equilibriums shift to the left side showing an increase in the amount of acid in the solution that is
why the color changes to pink. The concentration of the solution then turns yellow because NaOH is
a base and turns yellow in a basic solution. The equilibrium is shifted to the right when the NaOH is
added.
| [pic] |[pic] |
| colourless (Acid) | pink (Base) |
Phenolphthalein is a weak acid and does not fully dissociate ergo it creates an equilibrium. When
the HCl is added, the equilibrium is to the left, The concentration of the anions is too low for the
pink color to be observed. However, the NaOH is a strong base and makes the solution's equilibrium
shift to the right. The concentration of the anion becomes sufficient for the pink color to be
observed. 4. Both test tubes appear red with the acetic acid with the methyl orange. This indicates
that the equilibrium lies toward the acid. CH3COOH(aq) (( H+(aq) + CH3COO–(aq) Red yellow 5.
Both test tubes changed from orange to yellow. This shift indicates 6. NaCH3COOH(aq) ( Na+(aq)
+ CH3COO– (aq)
Part 3:

Solubility Lab
Solubility Lab Report The purpose of this lab was to demonstrate the solubility of compounds
created through reactions between certain dissolved substances. The solubility or insolubility of
these compounds creates a visual demonstration of solubility rules. To obtain the data, the molar
mass of each compound was calculated, and divided by 100 to determine the mass (in grams)
needed. The compounds used in the lab include KNO3, Na2CO3, NH4Cl, NaOH, Pb(NO3)2,
K2CrO4, AgNO3, CoCl2, Ba(NO3)2, CuSO4, and NaI. Filter paper was placed on a scale and tared,
and the correct amount of salt was measured using a scoopula. The salts were then poured into
beakers and combined with 200mL of water to create solutions. A table was created to record the
results of each combination of substances. ... Show more content on Helpwriting.net ...
Compounds containing ammonium ions (NH4+) are also soluble, as are ions from the Alkali metal
family (such as K+ and Na+). The tendency of reactions with the AgNO3 solution to produce white
or milky precipitates leads to the conclusion that compounds containing silver ions (Ag+) are
insoluble, with the exception of AgNO3. Hydroxide (OH–) compounds also seem to be insoluble
unless they contain an Alkali metal or ammonium, as reactions which produce an Alkali hydroxide
(or NH4OH) did not produce precipitates. Similarly, salts containing carbonate (CO3–2) seem to be
insoluble unless they contain an Alkali metal or ammonium. Chromate salts seem to be highly
insoluble unless they contain potassium or ammonium, as nearly every combination that included
K2CrO4 produced a precipitate. Compounds containing halogen ions such as chloride (Cl–) and
iodide (I–) are also generally soluble. Finally, compounds containing sulfate (SO4–2) are soluble
with a few exceptions, as Ag2SO4, PbSO4, and BaSO4 were all

Lab 3 : Le Chatelier's Experiment
Lab 3: Le Chatelier's Principle
Khadijah Maraheel
Location: My apartment
October 1st–3rd, 2017
Course: Chem112
Abstract:
The purpose of this experiment was to determine the effect of a change on a system at an
equilibrium. I will learn how temperature and pressure affects a chemical reaction. During this
experiment, I will observe the physicals changes when the solutions are mixed and determine the
shift of the equilibrium. I think the only reaction I will have will be color change, when the different
solutions are added together. Experiment: For this experiment, I added two chemicals K2CrO4 and
HCl together which created an orange color. Then I added NaOH to revert the reaction, which
changed the color of the solution back to yellow. I repeated the same procedure but didn't add the
NaOH the second time but added the solution to cold water then hot water for three minutes and
observed the reaction. I did the same thing for K4Fe(CN)6 and Fe(NO3)3 except when I mixed
them together it produced a dark blue with dark specks solution. I then added NaOH to revert back
to the original solution but I got a yellow color with brown specks instead.
Exercise 1: Equilibrium of Chromate and Dichromate
Data Table 1. Chromate–Dichromate.
Color of Chromate
Color of Dichromate
Number of drops of NaOH to shift chemical system
Yellow
orange
14
Data Table 2. Endothermic and Exothermic Shifts.
Reaction at Room Temperature
Reaction in Cold Water Bath

Silver Chromate Lab Report
This experiment was performed to observe the formation of silver chromate from a reaction between
silver nitrate and potassium chromate. In this double displacement reaction, the cations and anions
of the two reactants swapped and produced silver chromate and potassium chromate. An indication
of a reaction occurring between the silver nitrate and potassium chromate was the production of a
red solid from the yellow potassium chromate and the clear silver nitrate. Potassium nitrate has its
uses in applications such as fertilizers and food preservation while the other product of this reaction,
silver chromate, has little application in the real world. Introduction: The reaction between silver
nitrate and potassium chromate was a double displacement ... Show more content on
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0.1 grams of potassium chromate was then weighed out on the balance and dropped into the test
tube containing silver nitrate by the scoop. The reaction that occurred was observed and recorded.
Analysis: Trial 1 Observations: In the first trial, the previously yellow potassium chromate turned
red, indicating the presence of silver chromate. The silver chromate has settled in the silver nitrate
that was not used in the reaction. In the second trial, a majority of the silver nitrate was used in the
reaction and the products had not separated from each other. In the third trial, there was an excess of
silver nitrate and the silver chromate settled at the bottom much quicker than the previous two trials.
Trial 2 Observations: In the first trial, the previously yellow potassium chromate turned red,
indicating the presence of silver chromate. The silver chromate has settled in the silver nitrate that
was not used in the reaction. In the second trial, a majority of the silver nitrate was used in the
reaction and the products had not separated from each other. In the third trial, there was an excess of
silver nitrate and the silver chromate settled at the bottom much quicker than the previous two

Advantages Of Ion Implantation
1.1 Ion Implantation
Ion implantation is a materials engineering operation where ions of a material are accelerated in an
electric field and impacted into a solid. Ion implantation can also be referred to as a technique used
to deposit precise quantities of n–type and p–type dopants or impurities into a semiconductor at a
low temperature. Ion implantation alters the physical, chemical, electronic properties of a material
by forcibly impacting different types of ions into the material.
In ion implantation, dopant atoms are volatilized, ionized, accelerated, separated by the mass–to–
charge ratios and directed at a target. The atoms enter the crystal lattice of the material and collide
with the existing atoms. These atoms lose energy and finally ... Show more content on
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This is performed to achieve a graded interface or strengthening adhesion between layers of
materials that are incapable of attaining homogeneity.
Fig. 1 Ion Implanter 2.1 Laser Surface Treatment
Laser Surface Treatment is a technique which is used to enhance the property and repair damaged
parts of work pieces. The process involves hardening, cladding and alloying with high processing
speed and slight thermal effect on the fundamental substrate due to the accurate control of the heat
input and addition of material.
2.2 Principle of Laser Surface Treatment
Laser surface treatment works based on the principle of interaction between a beam of coherent
light which has a high power density and the desired surface within a specified atmosphere. Light is
generated in a resonator and directed at the surface of the sample. During the movement of the laser
beam over the work piece, a track pattern is created at the surface. Based on the desired process and
the geometry of the work piece, the system can be automated or designed to be controlled by robots.
Fig. 2 Laser beam treatment
2.3 Types of Laser surface treatment

Flame Test Lab Report Essay
In Part A of the experiment, the Unknown Substance #4 was found to contain Silver. Since no
precipitate was formed in Step 6 of the experiment, it was confirmed that there was no presence of
lead. Step 8 verified that the unknown solution contained Silver, with the formation of the white
AgCl precipitate. Silver was reasonable since it was confirmed that it was not Lead. Part B of the
experiment resulted in the identification of Barium. The presence of Barium was confirmed in Step
13, with the formation of the white BaSO4 precipitates in the orange solution. The unknown
solution was further tested to avoid a false positive confirmation of Calcium in Step 14. No
precipitate was formed so the solution in the 1M K2C2O4 so the Barium was once again verified.
Barium was reasonable since it had been ... Show more content on Helpwriting.net ...
After a metal salt is added to a hot flame, it shifts from the excited state to its ground state,
displaying a discrete spectrum of light. For example, Barium Chloride will emit a yellow color,
whereas Lithium Chloride emits a dark red color. However, the cation flame test is limited in that if
multiple cations are present, the results can be altered. The result of an impure solution can cause
the mixing of emitted wavelengths and colors. Alternatively, one cation can potentially conceal the
identity of the others.3 If this experiment were to have been repeated, micropipettes would be used
instead of the standard pipettes to increase the accuracy when withdrawing fluids. This would
substantially decrease the degree of errors due to incorrect measurements. Additionally, the
centrifuges would be replaced with new machines since the previous centrifuges caused a few test
tubes to break, even though the solutions had been evenly balanced by weight. More caution may
also be needed when balancing the centrifuges to prevent future

Chromium Essay
Chromium, the seventh most abundant element on earth is a transition metal from group VI–B .It is
found in nature as the bound form constituting approximately 0.1 – 0.3 mg.g–1 of the earth's crust.
The name of the element is derived from the Greek word "chroma" meaning color, because many of
its compounds are intensely colored. Cr is able to exist in several oxidation states, of which the
trivalent Cr (III) and hexavalent Cr (VI) species are the most stable and abundant forms (Zayed &
Terry et al., 2003).
The most stable form of chromium is its trivalent oxidation state which is primarily found
geologically as chromite (FeCr2O4) (Cervantes et al., 2001). Cr (III) is naturally occurring, whereas
Cr (VI) is of anthropogenic origin. This ... Show more content on Helpwriting.net ...
The deficiency of chromium has been implicated in impaired insulin action, which can cause
glucose intolerance, elevated glucose blood levels, diabetes, elevated cholesterol levels, obesity and
heart diseases, as well as other conditions not yet documented. Chromium is considered the cofactor
for all the actions of the hormone insulin, primarily the regulation of carbohydrate, protein and fat
metabolism. Signs of chromium deficiency are widespread; they tend to be associated with aging,
and are consistent with the progressive decline in body and organ content of chromium from birth
onward. Chromium deficiency impairs glucose utilization and disturbs protein and lipid metabolism
The biological effect of chromium is highly dependent on its oxidation state. Cr(VI) is highly toxic
and has been shown to be a mutagen and carcinogen, whereas Cr(III) is considered to be relatively
innocuous, probably due to the inability of Cr(III) to penetrate cells (Cervantes et al., 2001; Codd et
al., 2001).Chromate alone does not react with DNA in vitro, however, in the presence of reductants
a wide variety of DNA lesions, including Cr–DNA adducts, DNA–DNA crosslinks, DNA–protein
crosslinks and oxidative damage occurs (Codd et al., 2001).
Under normal physiological conditions, Cr6+ reacts spontaneously with the intracellular reductants
(e.g. ascorbate and glutathione) to generate the short–lived intermediates Cr5+ and/or Cr4+ free
radicals and the end–product Cr3+

Krypton Research Paper
Krypton, (symbol being Kr), is a very interesting element. It was discovered May 30, 1898 by Sir
William Ramsay and Morris M. Travers, who were Scottish and English chemists. Krypton was
named from the Greek word 'kryptos', which means hidden. It was found when the chemists were
studying liquefied air. It is about 0.0001% of the earth atmosphere. It can also be found in some
photographic flashes, some fluorescent light bulbs, and can be combined with other gases to make
signs with a greenish–yellow glow.
Every element is special because none are ever the same. Even an atoms isotope is different.
Krypton's atomic number is 36. Its atomic mass is 83.798 units. The number of protons in an
element, which is also the atomic number, is 36. It also ... Show more content on Helpwriting.net ...
It is found in gas form and is pure. It can bond with Fluorine to form Krypton Difluoride and
Krypton Tetrafluoride depending on the number of Fluorine atoms. It can also bond with chlorine
(Krypton Tetrachloride), Bromine, (Krypton Hexabromine), carbon and oxygen, (Krypton
Dichromate and Krypton Chromate depending on number of carbon and oxygen atoms), and just
oxygen, (Krypton Dioxide). Krypton is purified by passing it over hot titanium metal. A balanced
equation showing the purification of krypton is shown below:
Krypton Tetrachloride to Krypton
KrCl4 Kr + Cl4
All you have to do is separate Krypton from Fluoride and boom you got pure Krypton.
As said before, Krypton is used in some types of photographic flashes, some fluorescent bulbs, and
its mixtures are used in signs to give them a greenish–yellow glow. It was also once used in
measurements and is used in lasers for lab use.
Krypton is found in an extremely small amount of our earth's atmosphere. It is also used in a lot of
lights. If this element was not available my life and everyone else's would be different. We would
have no lights and God knows what will happen to our atmosphere. What if it's a crucial element for
us? If it was taken away, we'd be

Back Titration Lab Report
Abstract The concentration of ethanol in vodka was determined by back titration. A known amount
of excess potassium chromate was added to the vodka sample to convert ethanol into acetic acid by
oxidation. The amount of leftover chromate was determined by titration with iron (II) solution,
prepared from dissolution of ferrous ammonium sulfate. Using the amount of chromate added to the
vodka solution, the amount of chromate reacted was determined and used to find the amount of
ethanol in the sample. A potentiometer in the mV mode was used to create first and second
derivative curves for determining end points. The concentration of ethanol determined was 39.91%,
with standard deviation of 0.13%. The percent error was 0.22%, with the true concentration being
40.00%.
Introduction The consumption of alcoholic beverages, which has increased, has been presenting
several health complications in recent years. The center for disease control explained that the act of
drinking in order to become intoxicated has become more popular recently, and that this has led to
increases in alcohol poisoning, high blood pressure, stroke, liver disease, and neurological damage,
as well as both intentional and unintentional injuries [1]. Although alcoholic beverages contain
many different ingredients, the most significant is ethanol, as it is most commonly responsible for
the health problems mentioned above. This study's primary focus was to identify the concentration
of ethanol in an unknown

Dynamic Equilibrium and Le Chatelier’s Principle
Experiment No. 2: Dynamic Equilibrium and Le Chatelier's Principle December 1, 2011 Final
Formal Results Le Chatelier's Principle states that "when a stress is applied to a chemical system at
equilibrium, the equilibrium shifts in a direction that reduces the effect of stress" (Gross, Abenojar,
and Tan 23). Moreover, it helps us "predict the direction of the shift of the equilibrium" (Silberberg
745). Silberberg also stated that there are three kinds of disturbances – concentration, pressure, and
temperature – that can be applied to a system at equilibrium. However, only concentration and
temperature were observed in this experiment. Part 1: Cobalt Complexes Table 1 shows the color
change of the cobalt chloride solutions ... Show more content on Helpwriting.net ...
Mixing the colors red and blue produced the magenta–colored solution. The reaction above is
classified as endothermic while its reverse is exothermic. Increasing the temperature caused the
equilibrium to shift to the right resulting to a darker color while decreasing the temperature causes
the equilibrium to shift to the left resulting to a lighter color. Conclusions Le Chatelier's Principle
states that "when a stress is applied to a chemical system at equilibrium, the equilibrium shifts in a
direction that reduces the effect of stress" (Gross, Abenojar, and Tan 23). The principle was seen in
this experiment; as a stress – in this case concentration and temperature – is applied to the system, a
shift in the equilibrium was observed. The principle also helped in determining the direction of the
shift of the equilibrium. Increasing the reactants or decreasing the products causes the equilibrium to
shift to the right and vice versa (Silberberg 746). On the other hand, increasing the temperature
favors the endothermic direction while decreasing the temperature favors the exothermic direction
(Silberberg 750). Answers to Questions 1. How does one know when a reaction is at equilibrium? A
reaction is at equilibrium when the rates of the forward and the reverse reactions are equal (Ladon).
Reactants react to form products and

Duquenois Test Lab Report
As expected, the marijuana bubbled after HCl was added, signifying the release of CO2 (g). The
LCD glowed fluorescent under the UV light, as hallucinogens tend to show up as such. Another
technique that could be used to detect the presence of marijuana is the Duquenois test, in which 0.5
mL acetaldehyde, 1.0 g vanillin, and 50 mL ethanol are added to a sample and shaken. Extracting
this with chloroform will result in a purple or dark–blue color if marijuana is present. The unknown
contained silver, as both the unknown and silver solutions turned red and formed red precipitates
with the addition of potassium chromate. With the addition of Dithizone, both the unknown and
silver formed colloidal solutions with gray particles, so the unknown was likely silver. Discussion
Conclusion ... Show more content on Helpwriting.net ...
In doing so, we found that the unknown must contain silver ions, which formed a red precipitate
when potassium chromate was added. Both also formed a colloid with gray particles when
Dithizone was added. Lessons learned Our examination of marijuana and LSD reaffirmed the
information from the reading regarding their characteristics. The calcium carbonate crystals at the
base of marijuana leaf hairs reacted the HCl to produce CO2 (g), as most carbonates will form CO2
(g) when acids are added. The glowing LSD confirmed that hallucinogens have a tendency to glow
under ultraviolet light. Part II demonstrated the solubility rules and ion colors, as seen by AgCl and
PbCl, which both precipitated in our experiment. Sources of

Cation and Amnion Lab Essay
Name: Lisa Brewer iLab, Week # 2 CATIONS AND ANION LAB Introduction The purpose of this
week's lab is to learn to demonstrate a double–replacement reaction of ionic compounds. To
accomplish this, two ionic compounds will be mixed together and the product will precipitate out of
solution. In this procedure, the product must be precipitated out of the solution and then weighed.
For this lab, lead (II) nitrate (Pb(NO3)2) and potassium chromate (K2CrO4) will be reacted together
to demonstrate double replacement reaction between 2 ionic compounds. This was shown when
chromate replaced the nitrate and formed lead (II) chromate, and when the nitrate replaced the
chromate and formed potassium nitrate, which is shown in the ... Show more content on
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This indicates a reaction occurred and precipitate has formed and settled on the bottom of the
beaker. Set up the Erlenmeyer flask with a Buchner funnel. Select equipment from toolbar, then
from the dropdown menu, select Erlenmeyer flask–250mL. Right click the Erlenmeyer flask, choose
Buchner funnel. The Buchner funnel will be added to your Erlenmeyer flask. Select the 100mL
beaker and right click on Pour/Decant. The flask will turn on its side so that you can move the
beaker above the Buchner funnel. The solution will pour into the funnel when positioned correctly.
Note: When the solution has been filtered, a white area will appear on the bottom of the flask. Right
click the flask. Select Buchner funnel. Message window appears with question. Select place solid
into 50mL Test tube. Click OK. Note: a test tube will appear with a small amount of precipitate on
the bottom. To measure the weight of the precipitate, right click the test tube. Select show weight.
The weight of the precipitate will appear below the test tube. Record this information in the
Observations and Results section of the lab report, including the weight and appearance of the
precipitate. Observations and Results The appearance of the precipitate was shown several ways
during the experiment. In the 100mL beaker, after both chemicals were added, it was shown as a
dotted solution. It was then shown as a solid and a white color in

Sunday On La Grande Jatte Analysis
Imagine a painting comprised of thousands of tiny dots that have been strategically placed in a
pattern to form an image.The pioneer of pointillism and Neo–impressionism Georges–Pierre Seurat
sparked a new art movement and painting technique which was associated with creating the
appearance of solid figures using points of pure color grouped together. His creation of this art style
was inspired by his desire to abandon Impressionism. Seurat's most famous paintings of the 19th
century is the art piece made by Frenchman Georges Seurat called A Sunday Afternoon on La
Grande Jatte which uses the pointillism approach. It was painted between 1885–1886. The technique
he chose took much longer to produce, which is why it took him more than two years ... Show more
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From the figures in the painting, you can see sunbathers, soldiers, men in top hats, women with
parasols, dogs, and a monkey. According to an article, it states that "a monkey in French (and
female) is known as "singesse," denoting a prostitute. The smartly dressed woman is fishing – but
for what" ("Seurat's Grande Jatte", n.d.). I found this interesting because when I first saw this
painting, I first assumed it was just a regular painting of wealthy citizens relaxing and did not
suspect anything of the monkey strangely being present. The women on the right is holding a leash
to the monkey which many critics suspect that Seurat is trying to say through symbolism that this
woman is a prostitute who is out for a stroll with her client and that she is "fishing" for more. On the
left of the photo, you see a woman dressed in orange fishing by the water, which seems innocent.
According to an online dictionary, the French word for fish is 'pêcher', which some believe is a plan
on word as the French word for sin is 'pécher' (Dave, "The Psychology of Geometry"). References
to prostitution used the words 'pêche' (fishing) and 'péché' (sin) a lot in French cartoons. The artist
may be hinting that they are both prostitutes and demonstrates the art piece's satirical nature. Not
only are they suspect prostitutes, but they may have been proletarian women that have become
superficially bourgeois through prostitution. Seurat adds another perspective to the comparison of
the proletariat and the bourgeoisie, hinting the superficiality and immorality behind the high class

Transition Metals: Chromium
Chromium has an atomic number of 24, and is considered to be a transition metal.
It has an atomic mass of 51.996 amu, a melting point of 1907 degrees Celsius (2180 K, 3465
degrees Fahrenheit), and a boiling point of 2671 degrees Celsius (2944 K, 4840 degrees Fahrenheit).
This element is the first element within group 6. The ways in which interactions with light occur
along its surface allow for it to be considered lustrous. In addition, it is a silvery metallic that is hard
yet brittle. Its crystalline structure consists of a body–centered cube. Its density is 7.19 g/cm3 at 20
degrees Celsius. Its electron configuration is 2–8–13–1. Its spdf configuration is 1s^2 2s^2 2p^6
3s^2 3p^6 3d^2 4s^2. It has electrons located in 4 energy levels. The most common ions chromium
forms are Cr2+, Cr3+, and Cr6+. Louis Nicolas Vauquelin, French scientist, obtained samples of
crocoite ore in 1797. He discovered that he could isolate metallic chromium by heating its oxide in a
charcoal oven, allowing for him to become the discoverer of the element. Vauuquelin was also able
to identify remnants of chromium in gemstones, such as emerald or ruby. Moreover, he was able to
produce chromium trioxide by amalgamating crocoite and hydrochloric acid. During the 1800s,
chromium was used as a constituent piece of paints and in tanning salts. Chromium is also known
for its luster when polished. It is used in plumbing fixtures, furniture parts and many other items.
Initially, crocoite from

Groundwater Contamination Research Paper
When there is an addition of undesired substances from human activities in the groundwater, it can
cause groundwater contamination. There are many industrial operations that cause contamination in
ground water, due to the large quantities of chemicals used. Chlorinated hydrocarbons, which are
used in cleaning products and solutions containing chromium, which are used in metal plating, lead
to the groundwater contamination. These industrial wastes are dumped in storage tanks and they
leak, thus causing contamination. There is greater awareness of the issues and hazards of the
dumping of chemical waste and there are laws restricting the dumping of this waste. Since many
individuals rely on groundwater for drinking water, many of them are drinking contaminated water.
Due to this, there are many health risks including, hepatitis, poisoning and cancer when exposed to
polluted water. As well, the wildlife can be harmed from the contaminated ground water. A good
disposal method of ground waste consists of a chemical treatment that is able to convert the
hazardous waste into environmentally safe materials. A highly toxic chemical, trichloroethylene,
becomes non–toxic when the chlorine atoms are converted to chloride anions. As well, when
chromium–containing waste has highly toxic chromate anions are converted into Chromium (III)
ion, ... Show more content on Helpwriting.net ...
In the Colorado River in the American Southwest, a solid rocket fuel, ammonium perchlorate, had
waste when it is being manufactures and that in causing contamination in drinking water and is also
causing contamination in irrigation (water supply to land and crops). This contamination is causing
a lot of health problems because the contaminant is being found in vegetables as well. By using
microorganisms, perchlorate is being removed from water, since a lot of bacteria need perchlorate to
survive and they leave behind harmless chloride

Lab Report On Silver Nitrate
Faculty of pharmacy
Analytical Chemistry Department
Assignment Topic: Silver Nitrate
Course Title: Analytical Chemistry 2
Course Code: PC223
Lab Group: D
Prepared By: Ahd Mohamed Abdelmoniem Fahmi–175063
Due Date: 23–10–2017
Introduction about Silver Nitrate:
Silver nitrate is an inorganic compound with chemical formula AgNO3. It's colorless or white
crystalline solid which is less sensitive to light than the halides and a highly water soluble
crystalline. It was once called ... Show more content on Helpwriting.net ...
Decomposition: When heated to decomposition, emits toxic fumes of nitrogen oxides. Decompose
at 444° C, into metallic silver, nitrogen, oxygen and nitrogen oxides. Auto–Ignition: Not flammable
Light sensitive : Stability On exposure to air or light in the presence of organic matter, silver nitrate
becomes grey or greyish–black, and in the presence of traces of nitric acid, silver nitrate is stable to
350°C.
Solubility: Greater than or equal to 100 mg/mL at 61° F.
122 G SOL IN 100 CC WATER at 0°C.
952 G SOL IN 100 CC WATER at 190°C.
*Soluble in ether, glycerol.
*In water: highly soluble. Safety: Danger DOTInformation: DOT Class 5.1: Oxidizer
Pharmaceutical uses of silver

Santiago Ramon Y Cajal Neurology
1. Describe the neuron doctrine.
A theory proposed by Santiago Ramon y Cajal that the nervous system is made up of a different
type of cell, which transmits signals within this system called neurons. Cajal also added to the
theory that neuritis communicate through contact and aren't continuous.
2. Describe the contributions of Santiago Ramón y Cajal and Camillo Golgi to the field of
Neuroscience.
Camillo Golgi came up with the idea of silver staining, which uses silver chromate solution on brain
tissue. Through this staining process it showed more details about the neuron than the Nissl stain
could, like how the neuron had two distinct parts. Using Golgi's method Santiago Ramon y Cajal
was able to discover that the neuron was in fact the cellular

How To Write A Lab Report Using Qualitative Analysis Of...
The goal of this experiment was to correctly identify two different cations in unknown
solutions using qualitative analysis techniques. 1 Silver (Ag + ) and lead (Pb 2+ ) created a solution
of
metal nitrate salts which remained unknown until it was identified at the end of part A. Part B of
this experiment had a similar scenario to part A except the metals were switched and replaced with
either barium (Ba 2+ ) or calcium (Ca 2+ ). Part C consisted of a series of cation flame tests using
metal
chloride solutions, which resulted in a variety of colored flames. The color with which each cation
burned was observed and recorded. Throughout part A and B, a centrifuge was used to separate
solids and liquids that were in the solution. The centrifuge was able to do this ... Show more content
on Helpwriting.net ...
Keeping a centrifuged balanced was important as it could cause severe problems to the
equipment and substances inside. To balance a centrifuge, it was important to note that if one test
tube was placed inside, then another test tube with an equal amount of substance would be placed
directly opposite of the first test tube. By doing this, the weight inside of the centrifuge was
distributed equally and did not cause damage due to the high speeds.
The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)
to the unknown solution in order to completely precipitate the cations in part A. 2 A compound
between the unknown cation and chlorine (Cl – ) was also formed from the addition of HCl. HCl
was

also used to neutralize any base that may have been present.
The unknown sample was then heated in boiling water in step 5. The reason for heating the
sample was to allow for the lead chloride, if present, to completely dissociate into its ions of Pb 2+
and Cl – . If Ag + was present instead, then the solution would have consisted of silver chloride

Chemical Reactions Lab Report
I was hired to be a new chemistry teacher at the Forest Grove High School. When I got there, there
was chemicals on a shelf but some chemicals did not have labels. The important concept in this lab
was to help teach you how to identify chemicals based on other chemical reactions. There were six
chemicals that did not have labels so we had to make a hypothesis and then test the chemicals. After
testing the chemicals we had to write down the reactions on a data table saying if they were soluble
or not and what color the reaction is. Safety methods were to wear goggles and to wash your hands
often. Our hypothesis was A–Hg(NO3)2, B–NH4OH,C–K2CrO4, D–AgNO3, E–FeCl3, and F–
HgCl2. The chemicals that were the most soluble ... Show more content on Helpwriting.net ...
We made our predictions on which ones are which. We knew that one of the chemicals had a terrible
smell that resembled that of NH4OH, so that one was easy to predict. Then we tested the chemicals
to the ones on our data chart. We tested the chemical reactions that had unique colors. We tested
mystery element B with potassium chromate which made a neon yellow color, and that was the
same as Mercury(II) Chloride. That left us with the last possible chemical which was Hg(NO3)2 and
element F. In conclusion we ended up solving the mysteries of the mystery elements. The results
were that mystery element A was Ammonium Hydroxide, B was Mercury(II) Chloride, C was
Potassium Chromate, D was Silver Nitrate, E was Iron (III) Chloride, and F was Mercury(II)
Nitrate. Possible errors in the lab could have been chemical mixtures, data collection, cleanliness of
hands and clear chart, and possible data crossing. Our hypothesis was mostly correct but some parts
were incorrect. The parts of a hypothesis that were incorrect or the predictions of all the clear
liquids. What I had learned from this lab is how to predict and find out what chemicals are based
upon data and testing. This could be used in other parts of science because you are using your data
to predict other things. I would enjoy trying this experiment again with more mystery chemicals to
try and

Analysis Of Erin Brockovich By Director Steven Soderbergh
Taking a shower, washing your car, living life, all require one common element, water. Roughly
seventy percent of the surface of Earth is liquid, that's a lot of H2O. With such an abundance of this
natural resource why do so many not have access to a reliably clean source? Industrialization was
the problem for the residents of Hinkley, California as portrayed by director Steven Soderbergh's
2000 drama titled Erin Brockovich. A movie that made the public aware of a life threating substance
found throughout the world. Erin Brockovich is based on the community of Hinkley, California a
town located in the Mojave Desert. Where more than 600 residents were destructively affected by
groundwater that was polluted with Chromium VI (CrVI) also known as hexavalent chromium.
Three miles southeast of Hinkley, is the site of Hinkley Compressor Station 3, owned by the Pacific
Gas and Electric Company (PG&E). The compressor is used to compress natural gas as it is
transported through pipelines running from Texas to California. The California Water Science
Center reports that during the 1950s and 1960s the compressors cooling water was treated with Cr
VI to prevent corrosion of the compressor station. That cooling water was then released into unlined
ponds subsequently releasing contaminates into the soil and groundwater (U.S. Geological Survey
2016). Chromium is not a new finding. Its original discovery was made during the 1700s when
Johann Gottlob Lehmann acquired a mineral that had

Research Paper On Chromium
Chromium is a transition metal located in Group 6 of the periodic table and is steel grey in its pure
form. It is the 21st most abundant element in the earths crust. It has many compounds that are
colored, the most important compounds is the chromates of sodium and potassium; the dichromates;
and potassium and ammonium chrome alums. Chromium was discovered by Louis–Nicholas
Vauquelin in 1797. Vauquelin discovered that he could obtain metallic chromium by heating
chromium oxide in a charcoal oven. Chromium can not be found as a free element in nature, it is
found in the form of ores. Today, chromium can be obtained by heating the mineral chromite, which
is the main ore of chromium, from the elements silicon or aluminum, or by the electrolysis

Observations Of Chemical Reactions Lab Report
Kalah Bailey October10th 2015 Chem 109 Pre–Lab 6 Title: Observations of Chemical Reactions. In
this lab, students will recognize and record the chemical reaction results of seven different anions
and one cation. This experiment also focuses on the reaction of salt solutions and what happens
when two different solutions mix. Procedure: Carbonate (CO32–) – First, solid calcium carbonate
(CaCO3) is added to a test tube in a small amount. Next, 15 to 20 drops of 6M HCl are placed in the
tube. The result is then recorded. – 15 to 20 drops of 1M Na2CO3 are poured in a separate test tube.
Then 15 to 20 drops of 6M HCl are slowly added to the tube and the outcome is recorded. Sulfate
(SO42–) –Second, in a test tube 15 to 20 drops of 0.1 Na2SO4 are added. 5 drops of 0.5M BaCl2
are placed in the tube and the solution is stirred. The result is recorded. ... Show more content on
Helpwriting.net ...
Next, 1to 2 drops of 6M HNO3 and 5 drops of 0.1M AgNO3 are added and the solution is stirred.
The observation is recorded. – In the same tube, 6M NH3 is transferred drop after drop and is stirred
until a change happens. The reaction is then recorded. Iodide (I–) –Fourth, 15 to 20 drops of 0.1M
KI are moved into a test tube. A small amount of AgNO3 is added and the result is recorded. – In the
same tube, 20 drops of 6M NH3 is placed drop after drop and is stirred. The observation is recorded.
Acetate (C2H3O2) –Fifth, 15 to 20 drops of 1M NaC2H3O2 are added to a test tube followed by15
to 20 drops of 3M H2SO4. The solution is stirred and any odor is distinguished. Then, the outcome
is

The Effects Of Chemical Treatments On The Life Of The Timber
For centuries wood has been utilised by many great civilisations. With its natural form, it is
vulnerable to decay and degradation over time. Wood preservation has become more and more
important over the years because of the efforts to grow timber more rapidly and convert it more
economically have likely reduced the durability of the end product (Ridout, 2000).
When placed in the ground, untreated Radiata Pine sapwood will completely fail from decay within
2–3 years. This of course is depending on its cross–sectional dimensions. In above ground situations
however, the average life varies a lot, dependant on exposure, but poses a serious issue that many in
the past have noted. On the contrary, the development of chemical treatments greatly increased the
life of the timber. The expected service life of CCA (Copper Chromate Arsenic) treated sapwood is
20–50 years, depending on end–use and exposure conditions. Manufacturers who supply the timber,
guarantee CCA–treated wood from insect attack and fungal decay for 50 years when prepared,
treated and used in accordance with New Zealand standards. (Read, 2003). Other major treatments
have been developed but none have compared to CCA treated timbers worldwide sales and success.
Pre–treatment is not a new concept, and has been practiced for centuries, is used to prevent rot and
insects for sapwood. A majority of pre–treatment experimentation was adapted by problems in the
Navy, and various experiments were carried out with the likes

Understanding Of Basic Solubility Principles And...
The purpose of this experiment was to apply the understanding of basic solubility principles and
precipitation reactions to identify two unknown cations in a given solution. The first two processes
involved adding various acids and basis to the unknown solution to observe different precipitation
reactions. The unknown solution contained either silver or lead and either barium or calcium. For
unknown solution one, adding a sample of hydrochloric acid to the unknown solution started the
experiment. This was imperative because it triggered a precipitation reaction, creating PbCl2 or
AgCl. HCl was an ideal acid that was used because it was soluble to Calcium or Barium but atleast
partially insoluble to Ag and Pb, allowing for the Calcium or Barium to have remained in solution,
become isolated in a new test tube, and set aside for later use.1 The chloride ions are much more
attractive to the silver and lead ions compared to the calcium or barium, which allowed some to
precipitate while others to have remained in solution.2
After the initial decanter, deionized water was added to the precipitate and the tube was placed in
boiling water. This is an essential step, because this allows for the dissolution of any PbCl that
might have precipitated. Since PbCl is slightly insoluble, if there was Pb in the unknown solution,
the heating process would have caused it to become mostly soluble in the water. The addition of
heat as a source of energy was enough to break the attractive forces

Evolution Of Gas Lab Report
Evolution of gas–When a gas is formed it is evidence that a chemical reaction has occurred. In this
reaction HCl(aq) and solid NaHCO3 were converted to NaCl, water, and CO2(g). We can see the
bubbles in the aqueous solution. (–– removed HTML ––)
NaHCO3(s)+HCl(aq)→NaCl(aq)+H2O(l)+CO2(g)
Temperature change–The burning of methane produces heat and that is evidence that a chemical
reaction has occurred. When bonds are formed, energy can be released. We are actually feeling the
formation of new bonds when we feel heat from a fire.
Refinery flare – burning of dangerous gases in the oilfield
CH4(g)+2O(2)→CO2(g)+H2O(l)
Image © Shutterstock, Inc.
The formation of a solid is also evidence that a reaction has happened. Lead (II) chromate is ...
Show more content on Helpwriting.net ...
For example, you would say hydrogen and oxygen yield water. When chemical equations are
written, all atoms are balanced with a number before the compound called a stoichiometric
coefficient. These coefficients indicate the number of moles of reactants or product that is needed or
produced for that particular reaction. It is nature's recipe for that unique reaction. If we write our
example reaction it looks like this:
H2(g)
+
O2(g)
→
H2O(l) (NOT BALANCED)
2.02 g 32.00 g 18.02 g
Assuming we have 1 mol of each, we have 34.02 g on the reactants side and 18.02 g of product.
During a chemical reaction mass must be conserved. We add stoichiometric coefficients in front of
molecules to balance the number of atoms on both sides of the reaction. In doing so, the masses on
both sides of the reaction arrow are balanced as well. As always, the number "1" is implied.
2H2(g)
+

O2(g)
→
H2O(l)
4.04 g 32.00 g 36.04 g + + → +
4 mol H atoms total = 4.04 g 2 mol O atoms = 32.00 g 2 mol O atoms + 4 mol H atoms = 36.04 g
total mass of all

Potassium Chromate Lab Report
5. The addition of 3ml of 0.1mol L–1 potassium dichromate; K2CrO4 as our indicator. Safety
Procedures Silver Nitrate – AgNO3 Storage: Silver Nitrate must be stored in a dark and tightly
closed container which is completely wrapped in tin foil, as it deteriorates in presences of UV light.
It should be stored in cool, dry and well–ventilated areas away from all reducer, combustible
material, ignition sources and incompatible substances as it strong oxidizer. It should also be stored
away from corrosive areas and light. Safety  Silver nitrate is toxic so it should never be poured
into a sink.  Immediate medical attention is required if silver nitrate is split on skin or eyes. The
area on which the chemical is split must be washed with plenty ... Show more content on
Helpwriting.net ...
The spillage should be vacuumed or swept into a disposable container that can contain silver nitrate.
No combustible materials should be used to clean a spillage e.g. paper towels. Potassium Chromate
– K2CrO4 Storage: Potassium chromate must be stored in a closed container in a cool, well
ventilated place away from heat, ignition sources, combustible material, reducing agents and
incombustible substances. Safety  Potassium Chromate is toxic so it should never be poured into a
sink.  Immediate medical attention is required if potassium chromate is split on skin or eyes. The
area on which the chemical is split must be washed with plenty of cold water for 15 minutes. If it
split on clothing e.g. lab coat, it must be immediately removed.  If any spillage occurs, inform the
teacher in charge of the lab. The spill must be swept up into a sealed container and be disposed.
Once the spill is cleaned, the site must be washed and ventilated. No combustible materials should
be used to clean the spill. Ethanoic Acid – CH3COOH Storage: It must be stored in a tightly closed
container in a cool, well–ventilated area away from heat, ignition sources and oxidizing agents as it
a flammable substance.

Effects Of Chromium On Plant Growth Promoting Bacteria
SEMINAR AND TERM PAPER
ON
Enhancing phytoremediation of chromium–stressed soils through plant–growth–promoting bacteria
Under the guidance of:
Dr. Pravindra Kumar Associate proffesor
Department Of Biotechnology
Indian Institute of Technology Roorkee
Submitted by: Ilu Kumari
M.Sc. II yr
Enrollment no: – 14610008
Department Of Biotechnology Indian Institute Of Technology Roorkee
CHAPTER–08
Enhancing phytoremediation of chromium –stressed soils through plant–growth–promoting bacteria
Ilu Kumari Department of Biotechnology,IIT ROORKEE,ROORKEE
Abstract
Chromium which is a chemical element ,a metal,is toxic pollutant .Nowdays these are found to be
present in soils due to many human activities.It affects plant system and microorganisms that are
present in soil as well.Phytoremediation has emerged as a process to minimize or eliminate
chromium from chromium stressed soils,but this process takes long time.So when plant growth
promoting bacteria( PGPB) is used with this process as bioinoculant then it results into increased
plant growth and higher chromium reducing effects.PGPB via root architecture modification
increases chromium uptake,secretes metal

Pigment Lab
Introduction Pigments have a rich and complex history that connects both chemistry and art into one
science. In this experiment there were four different pigments being created: barium white, chrome
yellow, synthetic malachite, and Prussian blue. Barium white, also known as Barite, is an excellent
pigment to paint with because "barium sulfate is particularly inert to UV light and so does not
darken over time" (Emsley, 2014). Therefore, the pigment can survive for long periods of time
without fading. Chrome yellow was discovered in 1816 by Nicolas Louis Vauquelin (Douma, 2008).
Vauquelin also "found that he could make bright yellow and rich orange versions of lead chromate,
both of which he proposed as potential pigments" (Douma, 2008). The ... Show more content on
Helpwriting.net ...
The chemical reaction produced was Na2SO4(aq) + BaCl2(aq)  BaSO4(s) +2NaCl(aq) with
barium sulfate being the precipitate. Similarly, when scraping off the chrome yellow, ZnSO4(aq) +
Na2CrO4(aq)  ZnCrO4(s) + Na2SO4(aq), there was less pigment than was expected. However,
the copper carbonate made an exceptional amount of pigment, both the first week and the second.
The reaction to make copper carbonate is written, CuSO4(aq) + 2NaHCO3(aq)  CuCO3(s) +
Na2SO4(aq) + H2O(l) + CO2(g). Lastly, the final amount of Prussian blue, 4FeCl3(aq) +
3K4Fe(CN)6(aq)  Fe4(Fe(CN)6)3(s) + 12KCl(aq), was very little; however, the amount was
enough to incorporate shadows into the painting. By using all but the chrome yellow, a snowy
landscape was painted as seen in Figure

Aqueous 6.0 Molar Nitric Acid
Unknown 8543, a blue solution, was obtained and filled a quarter of a clean test tube. Three drops of
3.0 molar aqueous sodium chloride were added, causing a white solid to precipitate out of the aqua
solution. The test tube was centrifuged at power level one for approximately one minute. The
solution was decanted and saved for later. The solid was washed and suspended in a few drops of
deionized water and boiled for twenty minutes. The solid did not dissolve in water after this, giving
it the identity of solid silver chloride. To confirm the presence of the silver cation, a few drops of
aqueous 15.0 molar ammonia were added, creating a blue solution that must have been the complex
ion Ag(NH3)2+. Then, aqueous 6.0 molar nitric acid was added, producing a white precipitate,
silver chloride. This confirmed that the silver cation was present. To the solution that was set aside
earlier, five drops of aqueous 1.0 molar sodium sulfate was added, producing a white precipitate
from the aqua colored solution. The test tube was centrifuged for about one minute to separate the
solid from the solution, which was saved for later in a clean test tube. The possible cation in the
solid was ... Show more content on Helpwriting.net ...
Aqueous 3.0 molar ammonia was added, turning the solution a dark blue and forming a blue
precipitate. The test tube was centrifuged for one minute to separate the solid from the liquid. The
solid was saved and the liquid was placed into a clean test tube. To the solution, five drops of
aqueous 6.0 molar nitric acid were added, as well as four drops of thioacetamide solution, turning
the solution light green and producing a gelatinous precipitate. The test tube was then boiled for
approximately four minutes. This caused a black solid to precipitate out, indicating that copper was
the cation present. To confirm this, aqueous potassium iodide was added. This produced a dark
drown precipitate, confirming copper as the cation

Potassium Chromate Lab
The results obtained were consistent with the lab manual and the unknown sample aligned well with
the instructions that were given. The unknown sample was labeled "3" which was then combined
with HCl and centrifuged, decanted, combined with more HCl, centrifuged, and decanted again. The
precipitate formed from the two latter steps was then boiled and then combined with acetic acid and
Potassium Chromate to check for the presence of Pb2+. Upon mixing the precipitate with acetic acid
and Potassium Chromate, a bright yellow solution was formed with no apparent precipitate. This
bright yellow solution indicated that our unknown for part A contained Lead Chromate. In part, B
the liquid that was decanted in step 3 was to be tested for the presence of either the presence of
Barium or Calcium. The solution was mixed with Ammonium hydroxide and then it was tested to
make sure the solution was basic. Ammonium carbonate was then added and the solution was
heated, cooled, centrifuged, and the liquid was discarded. The precipitated was washed with water
and centrifuged. Acetic acid was mixed with the precipitated and dissolved until it was not cloudy.
Ammonium hydroxide was mixed with the unknown liquid. Potassium Chromate was then added
and a yellow precipitate was formed. The mixture was centrifuged and an orange liquid was formed
and then decanted. The remaining precipitate was then checked for the presence of barium by
adding HCl to dissolve it and was then ... Show more content on Helpwriting.net ...
The HCl itself helped to separate the Lead ions from the Calcium ions. This is why a precipitate was
formed for use in Part A and the liquid was saved for Part B. This worked due to differing KSP's as
one compound was more soluble rather than the other and thus the Lead, which was extremely
insoluble with a low KSP formed a precipitate with the addition of HCl since

Alkaline Earth Cation Lab
Introduction:
The purpose of this experiment is to establish the most efficient way to identify an unknown
alkaline earth cation and an unknown halide anion based on observations of various precipitation
and redox reactions. These observations are dependant on whether or not a precipitant formed or
there was a color change. Both of these indicate a reaction has taken place. The alkaline earth metals
are barium, beryllium, calcium, magnesium, radium, and strontium. And the halogens are fluorine,
chlorine, bromine, iodine, and astatine.
Experimental Procedure:
This experiment is broken up into two parts. The first part involves Alkaline Earth Elements. First
one drop of 1 M Na2CO3 is added to one drop of each alkaline earth solutions, 1 M

Lab Report Essay
When Kate and I showed up to set up our new classroom before the new school year, and we
discover the people before left a group of chemicals unlabelled. So to not waste supplies, we as
experienced chemists must determine their identities so we can use them. My partner, Kate and I
must identify a set of unknown chemicals with the knowledge we acquire by testing a set of known
solutions and seeing if they form precipitation reactions, if yes what color do they turn. We will
known if combining the solutions creates a reaction if one of the products is in a solid state. To
determine the identities, we must conduct an experiment. Before doing anything, we will put our
safety goggles and make sure there is no food and drink in the testing area. Then we will add drop of
a known solution and another known solution to see if a reaction occurs. We will repeat this action
and collect a database, then we will compare the results to the data of the unknown substances. With
both sets of data we will be able to make an educated ... Show more content on Helpwriting.net ...
First of all, solution A has a awful smell that Ammonium Hydroxide also has. Also both Ammonium
Hydroxide and solution A are clear solutions. Finally, they react to the known substances similarly.
When we mixed solution A with Copper II Sulfate a blue precipitate formed, which was what
happened we mixed Copper II Sulfate with Ammonium Hydroxide. When we mixed Iron III
Chloride with Ammonium Hydroxide and solution A separating a precipitate that was foggy clearish
formed. Also when mixed with Magnesium Sulfate both Ammonium Hydroxide and solution A do
not react, therefore mixing Magnesium Sulfate with those compounds doesn't cause a double
displacement reaction. Of course testing solution A and Ammonium Hydroxide with more chemicals
side by side would give us more confidence in our answer, but Kate and I are highly confident in
our answer

Newton And Seurat Research Paper
The world that we live in is constantly innovating new ideas and methods to benefit the lives of
many. It is a fascinating opportunity to reflect on all the inventions that have been made throughout
each of our lifetimes. Two very important individuals that shaped the world we live in today is Sir
Isaac Newton and Georges Pierre Seurat.
Sir Isaac Newton was an English mathematician and physicist. There is a theory that Newton
discovered gravity when he saw a falling apple. Supposedly, when he was observing the apple he
was also thinking about the forces of nature. Newton realized that some force must be acting on
falling objects like apples because otherwise they would not start moving from rest. Newton also
realized that the moon would "fly" ... Show more content on Helpwriting.net ...
For instance, when you stand on something soft, the object caves in or is pushed down. This is the
reaction of one's force on the soft object, and the soft object's reaction to one standing on it.Seurat
painted the 'La Grande Jatte' in three distinct stages. In the first stage, which was started in 1884,
Seurat mixed his paints from several individual pigments and was still using dull earth pigments
such as ochre or burnt sienna. In the second stage, during 1885 and 1886, Seurat dispensed with the
earth pigments and also limited the number of individual pigments in his paints. This change in
Seurat's palette was due to his application of the advanced color theories of his time. His intention
was to paint small dots or strokes of pure color that would then mix on the retina of the beholder to
achieve the desired color impression instead of the usual practice of mixing individual
pigments.Seurat's palette consisted of the usual pigments of his time such as cobalt blue, emerald
green and vermilion. Additionally, Seurat used then new pigment zinc yellow (zinc chromate),
predominantly for yellow highlights in the sunlit grass in the middle of the painting but also in
mixtures with orange and blue pigments. In the century and

Chatthooche Research Paper
The Chattahoochee is no longer an undisturbed river, but now all that is seen is man harvesting the
river or using the river in some way. Lake Lanier is one of the deepest of the dams created on the
Chattahoochee. Back in 1950 the US Corp of Engineers had three purposes in mind for the lake. The
first was to prevent flooding, second to proving a drinking water supply for the growing Atlanta
Metro area, and the third use was for power. Lake Lanier was at the center of the Water Wars. All
three states could not come to an agreement and be civil about how much power each would have
over the river. Materials & Methods The materials that were used to carry out the experiments on
the water samples were ten testing kits. We ran 10 tests on all ... Show more content on
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The buffer can filter out the stuff we put in our lawns, stop the silt that washes off places where we
dig and contain pollutants from lawns and roads. These pollutants have another way to get in to the
Chattahoochee, they flow virtually unchecked into the river from hundreds of miles of creeks that
thread through the water shed. Silt is sent down stream because of nearby construction. The greatest
danger to the creeks and to the water shed is land disturbing activities that lead to erosion, whether it
is tearing out plants and trees along the banks or lack of fence systems to hold dirt. Local
governments over seen by the state authority boards are responsible for enforcing state laws on
erosion control. But when faced with the pressure and desire to increase tax, few local governments
stand in the way of development. Even the latest growing counties have at most a few people to
enforce the law. Donald Mitchell, chief soil and erosion inspector in Fulton Count, compares his job
to "dropping a bucket of golf balls on a driveway and having to pick 'em up before they hit the
street." His job is part cop and part educator. He needs to make sure everyone is educated on the
issue so that people know what to do. Erosion into the creeks that feed the Chattahoochee is even
more severe a problem than direct run–off into the river, as

Hazardous Chemistry Research Paper
Sophia Zoll
January 22, 2017
Hazardous Chemical Rough Draft
Chemistry 7th INTRO
In 1954, Hinkley, California was a sleepy little town located in the Mojave Desert. People went
about their normal, daily lives without ever suspecting that they were in danger of chemical
poisoning. Little did they know that natural gas compressor station was slowly leaking hexavalent
chromium into the groundwater. Over the course of ten years, hexavalent chromium steadily spread
over the town of Hinkley, unbeknownst to the citizens. The chemical, originally intended to prevent
rust in water towers, was causing health issues in the unsuspecting citizens of Hinkley. For ten
whole years, the leakage of hexavalent chromium was affecting the health and environment ... Show
more content on Helpwriting.net ...
The chromium [affected] an area of groundwater at least eight miles long and two miles wide"
(California EPA, 2016). Over the course of ten years, the residents of Hinkley were living above this
polluted and contaminated groundwater. Later, "in the 1990s, hundreds of Hinkley residents claimed
illnesses and other damages stemming from the contaminated water" (Zimmerman, 2013).
Hexavalent chromium is a more toxic and dangerous form of the element chromium. Hexavalent
chromium is both an allergen and a carcinogen, depending on individual reactions. Exposure to this
chemical can cause allergic reactions on the skin, and lung cancer and respiratory issues can be
effects of breathing in or consuming hexavalent chromium. Other sublethal effects include irritation
or damage to the skin, nose, eyes, or throat if hexavalent chromium present in a large amount or a
high concentration. In the case of Hinkley, hexavalent chromium was concentrated enough that it
became a health and environmental

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