Essay On Ice Packs An Endothermic Reaction

Essay on Ice Packs an Endothermic Reaction
* .
Introduction
Endothermic reactions are accompanied by the absorption of heat. The dissolving of ammonium nitrate in water is an example of an endothermic
reaction. The solution resulting from this mixture is colder than either the ammonium nitrate or the water. This is the simple explanation of what
happens in an instant ice pack. The more detailed information will be discussed in the following paragraphs.
Cold Packs
Most cold packs come with a fabric cover made to absorb condensation and to protect the skin from contacting the surface of the cold pack. Cold packs
are used for injury or muscle relief. The cold pack contains two bags one containing water and the other containing ammonium chloride. Once the
ammonium chloride is ... Show more content on Helpwriting.net ...
This cooling reaction occurs instantaneously but lasts for about an hour. How does this reaction sustain itself for twenty minutes? This question will be
answered later in this explanation.
The type of cold pack presented here contains ammonium nitrate, which is a white crystalline substance. When these crystals react with water they split
into positive ammonium ions and negative nitrate ions. Due to the energy expended by the water in order to dissolve these crystals, the water becomes
colder.
Chemical Reaction
Ammonium nitrate (NH4NO3), is classified as a salt. The salt family of chemicals contains ions, which are particles with electrical charges. Due to
the fact that opposite polarity ions attract each other, they form a solid crystal that is called salt. This when seen by the naked eye seem like a simple
reaction. Bu, in reality this occurs in two different steps and each step a change of energy takes place.
The first step is the separation of the solid crystals back into separate ions, a positive ammonium ion and a negative nitrate ion. The break these ionic
bonds requires a lot of energy which means heat must be taken from the surrounding water. The second step the water molecules, which are H2O, are
attracted to the ions and attach themselves to the ions. The second step actually causes heat to be produced to the surrounding liquid mixture. .Even
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The Kinetocs Experiment of Iodide Ions and Persulphate Ions.
The catalytic effect of D–block ions and the kinetics of reactions iodine clock reaction: By Stephen Parsons 6K2 Centre number: 61813 Candidate
number: 8270 Table of Contents My aim and my reaction:3 Rate of reaction:4 Activation enthalpy:5 Collision theory:6 The effect of temperature on
reaction rate:7 The effect of concentration on reaction rate:7 The effect of a catalyst on reaction rate:8 D–block elements:9 The effect of extra kinetic
energy (from stirring etc.):10 Where do we use D–block ion catalysts?10 Arrhenius equation:12 Orders of reaction:10 Oxidation states of D–block
ions:13 Electronic configuration and transition metals:13 Experiment:13 Method:14 Risk assessment:15 How to make my standard... Show more
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The temperature affects most reactions and increases there rates unless the reaction uses an enzyme that only is effective up to or down to a certain
temperature. This change has this effect because it increases collision rate and speed so more collisions with the correct reaction energy occur so
more successful collisions occur increasing the reaction rate. The pressure is an important factor in gas reactions because the gas concentration is
proportional to pressure. The use of a catalyst affect reaction rate by lowering the reaction enthalpy making the proportion of successful collisions
higher. Surface area of reactants is a key variable because a higher surface area provides a higher chance of 2 reactants colliding and producing a
successful reaction. Activation enthalpy: I just talked a lot about activation enthalpy I will now explain what is meant by this. Activation enthalpy is
the minimum amount of kinetic energy required by a pair of colliding particles for a reaction to occur. it is the amount of energy required for the
particles of the reactants to break the bonds holding them

A Comparison Between Sodium Thisulfate And Carbonic Acid
The sodium cation did not have an effect on pH. We tested sodium acetate, sodium carbonate, sodium bicarbonate, sodium bisulfate, sodium bisulfite,
sodium chloride, sodium citrate, sodium formate, sodium iodide, and sodium hydroxide. The pHs of these compounds ranged from 1.25 to 13.00,
which were sodium bisulfate and sodium hydroxide, respectively. Sodium bisulfite and sodium carbonate had average measured pHs of 4.24 and
11.13, respectively. Since this range is so wide, we can conclude that sodium had no direct effect on pH. As for the potassium cation, we tested
potassium acetate and potassium hydroxide. When comparing the pHs of these two compounds, potassium acetate had a measured pH of 7.31 and
potassium hydroxide had... Show more content on Helpwriting.net ...
For a pool to be usable to swim in, it must be at a certain pH. If a pool is too basic or too acidic, then this can cause some serious health issues to
that particular person. Most people monitor the pH to be at 7.5 to get the most effectiveness of sanitation. Another application where pH is important
is when studying the stomach. The human stomach contains gastric acid, which is used to break down food particles. This is beneficial with
digestion but can cause problems such as heartburn. Heartburn occurs when the gastric acid in one's stomach goes back up to the esophagus. This
can be counteracted however by using a basic substance such as Tums. The base will then make the solution in the esophagus neutral and relieve the
person of their heartburn. D) If all 23 compounds had the same concentration, we believe that Nitric Acid would have the lowest pH. For the highest
pH, we think it would be very close between Potassium Hydroxide and Sodium Hydroxide. We believe these compounds would be the highest and
lowest because of the fact that they are strong acids and bases. Strong acids and bases completely ionize when put into a solution in water, because of
the

Identifying Unknown Ionic Salts From Zinc Nitrate
Identifying Unknown Ionic Salts by Precipitation ––– Cindy
Aim: identify three unknown ionic salts from zinc nitrate, barium nitrate, lead nitrate, sodium chloride, sodium carbonate and magnesium chloride by
precipitation.
Equipment:
6 small test tubes
distilled water
measuring cylinder
3 unknown ionic salts (No.7, 8, 9)
rack
silver nitrate
sodium hydroxide
calcium nitrate
sodium chloride
copper sulphates Method:
1.Pick three unknown ionic salts (NO. 7, 8 and 9)
2.Use the measuring cylinder to get 1.5ml water and pour it into a test tube
3.Use a spatula to remove 3 scoops of the ionic salts powder into the test tube and dissolve them in 1.5 ml water respectively.
4.Put 2 drops of silver nitrate in each of the ... Show more content on Helpwriting.net ...
NO. 7NO. 8NO. 9
Silver nitratePPT
Table 2: Test for unknown solid 7
Table 3: Test for unknown solid 8 and 9 NO. 7
Sodium hydroxide
Calcium nitratePPT

PPT = Precipitation NO. 8N0. 9
Sodium chloride
Copper sulphatesPPT Table 4: Name of solid 7, 8 and 9
Number of the ionic solidNo. 7No. 8No. 9
Name of the solidSodium carbonateZinc nitrateBarium nitrate
Dissociation equations of the ionic solids:
1.Na2CO3 (aq) + aq 2Na+(aq) + CO32–(aq)
2.Zn(NO3)2(aq) + aq Zn2+(aq) + 2NO3–(aq)
3.Ba(NO3)2 (aq) + aq Ba2+(aq) + 2NO3–(aq)
Precipitation equation:
1.Na2CO3 (aq) + 2AgNO3 (aq) NaNO3 (aq) + Ag2CO3 (s)
2.Na2CO3(aq) +Ca(NO3)2(aq) 2NaNO3(aq)+ CaCO3(s)
3.Ba(NO3)2(aq) + CuSO4 (aq) Cu(NO3)2 (aq) + BaSO4 (s)
4.Ba(NO3)2(aq) + CuSO4(aq) Cu(NO3)2(aq)+ BaSO4 (s)
5.MgCl2(aq) + 2Na2CO3(aq) 2NaCl(aq) + MgCO3 (s)
6.MgCl2(aq)+ 2NaOH(aq) 2NaCl(aq) + Mg(OH)2 (s)
7.Pb(NO3)2(aq)+ 2NaOH(aq) 2NaNO3(aq)+Pb(OH)2 (s)
8.Pb(NO3)2(aq) + CuSO4(aq) Cu(NO3)2(aq)+ PbSO4 (s)
9.2NaCl(aq)+ Pb(NO3)2(aq) 2NaNO3(aq) + PbCl2 (s)
10.NaCl(aq) + AgNO3(aq) NaNO3(aq) + AgCl (s)
11.Zn(NO3)2(aq) +Na2CO3(aq) 2NaNO3(aq)+ ZnCO3 (s)
12.Zn(NO3)2(aq) +2NaOH(aq) 2NaNO3(aq) + Zn(OH)2 (s)
Discussion:
In the method, the first chemical that is used to identify the solids is silver nitrate

The Effect Of Hydration Of Copper Chloride Hydrates
Purpose Hydrates are inorganic salts that lose water when heated and undergo a color change. The loss of water makes the hydrate anhydrous.
Copper chloride hydrate is what will be used in the lab to show what happens when a hydrate is heated which can lead to a better understanding of
hydrates as a whole and their reactions that can be observed to discover things about the environment they're in. After the removal of water from the
copper chloride hydrate, the solid ,when reacted with aluminum and filtered, produces elemental copper. Through the understanding of the process
used to achieve this, the experiment can be recreated for another hydrate to isolate a different element. By determining the amount of water and copper
in the ... Show more content on Helpwriting.net ...
The molecular formula is the actual amount of atoms of in each molecule but is not used in this lab. Empirical formulas can be found by converting the
grams of each substance within a compound to moles using their molar mass then dividing each value by the smallest value calculated. That results in
the molar ratios which are multiplied so that they are all whole numbers. Those numbers can be plugged into the formula as subscripts to obtain the
empirical formula which is the simplest form of the formula. The empirical formula of copper chloride hydrate will be found by completing experiment
and using the masses of the reactants and products. The mass of chlorine is not measured during the experiment but can be found through the masses of
water and copper that are measured in the experiment. By adding the masses of water and copper together the mass of chlorine can be determined and
used in finding the mole ratios which can then lead to the formation of the empirical formula. The empirical formula of the hydrous compound will be
found and is different than the anhydrous formula. The anhydrous version won't contain water. How the empirical formula is written is also important.
The compound in the experiment contains water and instead of distributing the mole ratio of water to each subscript, the number comes before it. This
is because the empirical formula is the smallest

Determining The Chemical Formula For A Hydrated Compound...
Introduction:
This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal
structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxClyzH2O, and aim is to determine
chemical formula of this compound.
Law of definite proportion, sometimes called Proust's law, states that a compound always has exactly the same proportion of elements by mass. This
means that contents of a compound does not depend on its source or its method of preparation.
John Dalton wrote the modern atomic theory, a fundamental component of that is, the mole ratios of elements in a compound will be small whole
numbers. ... Show more content on Helpwriting.net ...
Used stirring rods to completely remove copper from that wire. And then completed the removal of copper using 5 drops of 6M HCl, adding it onto
copper. There will produced copper in a solution. Connected Buchner flask to the vacuum line and place filter paper in it to completely washed off
the copper. Then, add 95% ethanol to copper and leave it for 1 min and turned section back for 5 mins. Measured mass of clean, dry watch glass.
Transfer copper to watch glass and dry it under heat lamp for 20 mins, allowed it to cool to room temperature and then accurately determine its mass.
Results:
Data table:
Included below is the measured mass of materials.
Mass of crucible (g) 9.1003
Mass of crucible and hydrated sample (g)
10.108
Mass of hydrated sample (g)
1.0217
Mass of crucible and dehydrated sample (g)
9.8870
Mass of dehydrated sample (g)
0.7867
Mass of water evolved (g)
0.2350

Mass of empty watch glass (g)
1.8904
Mass of watch glass and copper (g)
2.2850
Mass of copper (g)
0.3946
Figured out all the mass listed in the table from which: Mole of water: .2350g divide by 18.016 g/mol = .013 mol. Mole of copper: .3946g divide by
63.55 g/mol = .00621 mol.
Mole of chlorine : 1.0217g – .221g – .3946 g = .4061 g of chlorine .4061g divide by 35.45 g/mol = .01146 mol.
Mole Ratios :
Mole of water : Mole of copper = .013/.00621 = 2.09
Mole of Chlorine : Mole of copper = .4061/.00621=1.8
So,

Essay about Ionic Reactions
Ionic Reactions
Abstract
This experiment is designed to study the nature of ionic reactions, and write net ionic equations for precipitation reactions, as well as to identify
spectator ions, perception reactions and solubility of different compounds.
Experiment and Observations
In this experiment I was using a 96–well plate to add two drops of the following solutions into seven wells in rows A through E: cobalt (II) nitrate,
copper (II) nitrate, iron (III) nitrate, barium nitrate, and nickel (II) nitrate. Afterward, two drops of each of sodium phosphate, sodium iodide, sodium
sulfate, sodium chloride, sodium bicarbonate, sodium carbonate and sodium hydroxide were added to the five vertical wells under columns ... Show
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This was expected because the solubility rules stated that these were all insoluble substances. I was careful to add exactly two drops of each into each
well, as to keep my experimental error to a minimum.
Questions:
A. Compare your results with the solubility rules and/or solubility table in your chemistry text.
B. Do your results agree with your expectations from the solubility rules/table? Yes, my results did agree with my expectations from the basic solubility
rules.
C. Which anions generally form precipitates? What are exceptions? Most hydroxides, sulfides, carbonates and phosphates form precipitates. Alkali
metals, barium, silver nitrate, silver nitrite and silver perchlorate are some exceptions.
D. Which anions generally do not form precipitates? What are the exceptions? All nitrate salts, alkali metals, ammonium salts, sulfates, acetates, and
halides do not form precipitates. Calcium sulfate, strontium sulfate, barium sulfate, lead (II) ions, silver halide, lead (II) halide and mercury (I) ions
are some exceptions.
E. Which cations generally do not form precipitates? All cations in groups 1 and 2 of the periodic table generally do not form precipitates. http:/

/chemistry.about.com/od/lectureclassnotes/a/Qualitative–Analysis.htm F. Select 10 reactions that produce a precipitate, color change, or gas and write
balanced chemical equation and a net ionic equation for

Resistance Of Movement Of The Cell
If a cell is to perform its functions it must maintain a steady state in the midst of an ever changing environment. This steadiness is maintained by the
regulation of movement of materials into and out of the cell. To achieve this control, cells are bounded by a delicate membrane that differentiates
between different substances, slowing down the movement of some while allowing others to pass through. The membrane is said to be differentially
permeable since not all substances penetrate equally well. Selective permeability is a characteristic of healthy, intact cells. When a cell is seriously
damaged, the membrane becomes permeable to virtually to everything and substances can move freely in and out of the cell. (Marieb 2013) Movement
of... Show more content on Helpwriting.net ...
(Marieb 2013) Osmosis, is a special kind of diffusion, is defined as the diffusion of water through a semi–permeable membrane from a higher
concentration to that of a lower concentration. The concentration of water is inversely related to the concentration of solutes. If the water can diffuse
across the membrane, both water and solutes will move down their concentration gradients through the membrane. (Marieb 2012) There are three terms
used to describe the concentrations of solute particles of different solutions: Hypotonic– When compared to another solution of different concentration,
the solution contains the lower concentration of solute particles. Water moves across a semi–permeable membrane out of a hypotonic solution.
Hypertonic– When compared to another solution of different concentration, the solution that contains the higher concentration of solute particles.
Water moves across a semi–permeable membrane into a hypertonic solution. Isotonic–Having the same concentration of solute particles as another
solution. There is no net flow of water across the membrane. In animal cells, the movement of water is affected by the relative solute concentration of
the plasma membrane. As water moves out of the cell, the cell shrink and if water moves into the cell, the cell swells and may even burst.
PURPOSE: The objective of this experiment is to

Lab Report
Lab Report 1
пЃ¶Introduction: Proper chemical formulas entitle many challenges such as the Law of Multiple proportions that states that there may be more than
one plausible mole ratio for the elements in that compound. However if we determine the mass of each element in the compound we will be able to
get the true chemical formula.
In this experiment, we used the law of definite proportions to find the chemical formula for a hydrated compound containing copper, chlorine, and water
molecules locked in the crystal structure of the solid compound of Copper Chloride Hydrate. First we will gently heat a sample of the compound to
drive off the water of hydration. By measuring the mass of the sample before and after heating we can determine ... Show more content on
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It can cause painful burns if it comes in contact with the skin.
11.Use a glass stirring rod to scrape off as much copper as possible from the Al wire. Slide the wire up the wall of the beaker and out of the solution
with the glass stirrer and rinse off any remaining copper with distilled water. If any of the copper refuses to wash off the aluminum wire, wash it with
one or two drops of 6 M HCl solution. Put the Al wire aside.
12.Collect and wash the copper produced in the reaction.
A)Set up a BГјchner funnel for vacuum filtration.
B)Obtain a piece of filter paper. Measure and record its mass, and then place the filter paper on the funnel. Start the vacuum filtration.
C)Use small amounts of distilled water to wash all of the copper onto the filter paper on the BГјchner funnel. Use the glass stirring rod to break up the
larger pieces of copper.
D)Wash the copper twice more with small amounts of distilled water.
13.Turn off the suction on the vacuum filtration apparatus. Add 10 mL of 95% ethanol to the copper on the filter paper and let it sit for about 1
minute. Turn the suction back on and let the vacuum filtration run for about five minutes.
14.Measure and record the mass of a clean, dry watch glass. Transfer the copper to the watch glass. Make sure that you have scraped all of the copper
onto the watch glass.
15.Dry the watch glass of copper under a heat lamp or in a drying oven for five minutes. When the watch glass is

Clo2 Residual Testing Method
CHLORINE DIOXIDE AND CHLORITE
105
7. ANALYTICAL METHODS
The purpose of this chapter is to describe the analytical methods that are available for detecting, measuring, and/or monitoring chlorine dioxide and
chlorite, its metabolites, and other biomarkers of exposure and effect to chlorine dioxide and chlorite. The intent is not to provide an exhaustive list of
analytical methods. Rather, the intention is to identify well–established methods that are used as the standard methods of analysis. Many of the
analytical methods used for environmental samples are the methods approved by federal agencies and organizations such as EPA and the National
Institute for Occupational Safety and Health (NIOSH). Other methods presented in this chapter ... Show more content on Helpwriting.net ...
The absorbance is proportional to the concentration of the chlorine dioxide in water. Indicators used for this technique include
N,N–diethyl–p–phenylenediamine, chlorophenol red, and methylene blue (APHA 1998; Fletcher and Hemming 1985; Quentel et al. 1994; Sweetin et
al. 1996). For example, chlorophenol red selectively reacts with chlorine dioxide at pH 7 with a detection limit of 0.12 mg/L. The interferences from
chlorine may be reduced by the addition of oxalic acid, sodium cyclamate, or thioacetamide (Sweetin et al. 1996). APHA Method 4500–CLO2–B,
iodometric titration analysis, measures the concentration of chlorine dioxide in water by titration with iodide, which is reduced to form iodine. Iodine
is then measured colorimetrically when a blue color forms from the production of a starch–iodine complex. The detection limit for this method is 20
Вµg/L (APHA 1998).
CHLORINE DIOXIDE AND CHLORITE 7. ANALYTICAL METHODS
107
Table 7–1. Analytical Methods for Determining Chlorine Dioxide and Chlorite in Environmental Samples
Sample matrix Preparation method
Air Workplace air None.
Analytical method

Toxic gas vapor detector tube
Sample Percent detection limit recovery Reference
0.05 ppm No data EPA 1997 BjГ¶rkholm et al. 1990; Hekmat et al. 1994 (OSHA Method 202) Hoehn et al. 2000 (EPA Method 300.0) Pfaff and
Brockhoff 1990 No data APHA 1998 (Method 4500CLO2–D)
Diffusion of air into potasIon chromatosium iodide solution at pH 7. graphy (of chlorite ion

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

The First Utilized Schiff Bases 3a K Towards Mild Steel
3. Results and discussion 3.1. Identification of inhibitors In the view of the aforementioned remarked values of inhibition efficiency of this class of
organic inhibitors, this paper aims to study the concerned function of the first utilized Schiff bases 3a–k towards mild steel in 0.5 M H2SO4 solution.
N–aryl– (Sb_a–g), N–heteryl– (Sb_h–j)–, and the Schiff base Sb_k have been obtained condensation of N–aminophthalimide (S) with the
corresponding aromatic aldehydes 2a–e, heterylaldehydes 2f–j and isatine 2k, respectively. This study takes into account the beneficial role that could
be played by the p–electrons of the heterocyclic aldehyde or ketone N– and O– atoms present in the heterocyclic aldehyde and ketone moieties. The
name of products and symbols were listed in Table 2. The melting point, yield, time of reaction and IR spectra of products were listed in Table 3.
Spectral study has been used to characterize the structure of the novel synthesized Schiff bases (Sb_f–k) which to our knowledge have not been
previously reported as shown in Table 4. The structure of the Schiff bases Sb_a–e was confirmed by identity of melting point and spectral data in the
literature 25–27. The infrared spectra all the products Sb_a–k revealed that no coupling bonds in the 3 Mm region that refers to the absence of the
amino –NH2 functionality of compound S instead a sharp absorption band appears on the region of 1604–1688 cm–1. Characteristic to the imino
–c=N– group, indicating that compound

Analyzing The Properties Of Different Objects
Cole Powlison December 15, 2014 Mr. Gattis Pre–AP Chemistry–5 Discovering the Properties of Different Objects' Matters and Densities Group
Members: Cole Powlison and Cade Andrews Due Date: December 17, 2014 Purpose: The purpose of this lab is to explore the properties of both
density and matter in an object. Materials: One Triple Beam Balance Sodium Chloride Sucrose One Aluminum ball (tin foil) One Spoon Procedures:
1.A spoonful of sodium chloride was placed on the balance, then measured, then written down. 2.A spoonful of sucrose was placed on the balance,
then measured, then written down. 3.The aluminum ball was placed onto the balance, then measured, then written down also. 4.The molar mass, the
number of moles in the sample, and the number of representative particles in the sample were also recorded. 5.The mass, molar mass, moles (in 100
mL), and the representative particles (in 100 mL) of water, hydrogen peroxide, and rubbing alcohol were also recorded given the volume and density.
Data/Results: Sodium ChlorideSucroseAluminum Mass of Sample (g)4.38 grams6.92 grams1.28 grams Molar Mass (g/mol)58 g/mol342 g/mol27 g
/mol Moles of sample0.076 moles0.02 moles0.047 moles Number of representative particles in sample4.6 x 1022 NaCl Particles1.2 x 1022 Sucrose
Particles2.8 x 1022 Aluminum Particles WaterHydrogen PeroxideRubbing Alcohol Chemical FormulaH2OH2O2C3H8O Density (g/mol)1.00 g
/mol1.46 g/mol0.785 g/mol Volume (g/mol)100 mL100

Chemistry Concepts That Are Present During The Process Of...
Introduction
Rust, also known as iron (II) oxide, occurs when iron is exposed to oxygen and moisture for a long period of time. This reaction is called oxidation.
Oxidation can occur on old cars, iron, exhaust and even the burning of fossil fuels. When wood, natural gas, or coal burns, the oxygen in the air
combines with the carbon and hydrogen in the fuel to produce water and the oxides of carbon.(Prentice Hall Chemistry The Study of Matter p.599.) Rust
may seem like an average everyday phenomenon, however many things we cannot see take place as the rust begins to form. Many everyday exposures
such as water or hot temperature can cause rust to form. The purpose of this paper is to relate chemistry concepts that are present during the ... Show
Despite its destructive characteristics it can be stopped by acids or bases that will dissolve the rust off, but if you leave any bare iron outside exposed
to heat and water rust will occur without doubt. After the rusting process has occurred iron can either lose its magnetic ability or weaken it. ("Rate of
Rust Formation", van.physics.illinois)
SC2 Molar mass of Rust and indicators of chemical properties.
The molar mass of rust is 159.69 g*molв€’1 . The chemical formula is Fe2O3. Chemical properties in rust are indicated by the change of color,
smell, and production of a solid. Rust as a solid can appear on many household items such as cars, bikes, and tools. Basically, anything left outside can
get rained on, and the rain will leave the item wet, and overtime rust will appear. Rust has a brown–red–orange color. Rust has a smell similar to blood.
4Fe+3O2+6H20 в†’ 4Fe(OH)3 is the formula for the rusting of iron. So basically, do not leave items that you care for outside where they can get
rained on because the rust will ruin it.
SC3. Chemical bonds and the movement of electrons
Fe2O3 is an ionic bond due to the reaction between a metal, Iron, and a nonmetal, Oxygen. Based on the atomic radius

Initial Ph Test Lab Report
Upon completion of each spot test, as well as initial pH tests, the results were then recorded. It was known that the 10 solutions consisted of 1 M
hydrochloric acid, 1 M nitric acid, 3 M acetic acid, 1 M sodium hydroxide, 0.1 M silver nitrate, 0.1 M sodium chloride, 0.1 M zinc chloride, 0.1 M
aluminum nitrate, 3 M ammonium hydroxide and 0.1 M lead nitrate, however their corresponding number was unknown. The first identified unknown
was 98, acetic acid, given its highly prevalent scent, in addition to it not forming a precipitate with any substance due to the solubility rules. Given that
two bases were present on the initial pH test, one being strong (93) and one being weak (91), it was then concluded that they were the strong base
NaOH and the weak base NH4OH, respectively. Once identified, the precipitates formed by these two bases were then taken into account. Given that
both bases reacted with the weak acid, 99, yet it drastically different manners (white and copper), it was then researched to see what would react with
these bases to form a copper colored precipitate, resulting in AgNO3. Given that this was only one reaction, 99 as AgNO3 was not a fully supported
result yet; further reactions would have to be considered. Next, the chemical reactions were written out to determine ... Show more content on
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By applying the general solubility rules listed below, the precipitate or lack of were then able to be analyzed to determine each substances identity after
mixing on a spot plate. Given that specific compounds react differently when mixed with another substance, the precipitate, pH, and chemical equation
of the reaction itself was utilized in determining the substance. Procedures such as the one conducted in this experiment are especially useful in
determining which chemical is which, if it is unable to be deduced through pH, smell, or

Iodoethane Lab Report
Anas Hanini CHM 211L Professor: Bruce Bondurant 10/09/2017 Introduction The objective of this experiment was to carry out the alkylation of
sodium saccharin with iodoethane and to analyze the product mixture to determine the structure of the major product. In this reaction, the leaving
group is the iodide ion. The nucleophile in sodium saccharine is either the oxygen atom or the nitrogen atom. The sodium saccharin acts as an ambient
nucleophile which means it can attack from two or more places which can result in multiple products (Lehman). In order to determine the identity and
composition of the product formed in the reaction, proton nuclear magnetic resonance (1H NMR) spectrometry is used. Proton NMR is a powerful
instrumental method that... Show more content on Helpwriting.net ...
This melting point range is closer to N–ethylsaccharin than O–etyhlsaccharin. The signals on the proton NMR correspond to the CH2 (methylene)
protons in the –OCH2CH3 and –NCH2CH3 groups. In O–ethylsaccharin the CH2 protons are more deshielded by the more electronegative O giving a
larger chemical shift of 4.7 ppm. The larger chemical shift of O–ethyldsccharin's methyl group is derived from the protons of the methyl group having
less electron density than N–ethylsaccharin's methyl group. In N–ethylsaccharin the CH2 protons are less deshielded by the less electronegative N
giving a smaller chemical shift of 3.9 ppm. Around 8 ppm H NMR give the benzene peak. The peak for N–ethylsaccharin integrates a ratio number of
4 while the peak for O–ethylsaacharine integrates to 1. The Keq value was calculated to be 6.2x10^–5. This means that if our reaction was in complete
equilibrium the O–ethylsaacharin product would not even show up because it would be a 1:10,000 ratio. Based on our NMR data and observed
melting point, it can be concluded that N–ethylsaccharin is the major product that was formed in this

Water Is The Most Important Substance On Earth
Water is the most important substance on earth, all plants, animals and humans must have water to survive. Chemically, water is a compound made
of two hydrogens covalently bonded to the single oxygen atom, which forms the chemical/ molecular formula 0. In nature, water appears in all three
common states of matter and takes many different forms on Earth: water vapour and clouds in the sky, seawater and icebergs in the polar ocean and
glaciers and rivers in the mountains. Water is tasteless, does not have an odour and is liquid at standard temperature. Water's colour has a very slight
blue hue, although it appears colourless in small quantities and blue in large quantities. Water owes its blueness to the selective absorption in the red
part of its visible spectrum. The absorbed protons endorse transitions to high overtone and amalgamated states of the nuclear motions of the molecule;
to highly eager vibrations. To make this clearer, some of the light, hitting the surface of the ocean, is reflected back directly but most of it infiltrates
the water surface interacting with its molecules. The water molecules can vibrate in three different modes when light hits it. The red, orange, yellow
and green wavelengths of light are absorbed so that the remaining light we see is composed of the shorter wavelength; blues and violets. This is the
main reason why the colour of water is blue. To current knowledge water is the only example in nature in which colour comes from vibrational

Investigating the Kinetics of the Reaction Between Iodide...
PLANNING
Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions
By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate
ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions, then the concentration of
Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking place. From these results, I hope to draw conclusions
as to the effects of these changes to the environment of the reaction on the rate and also determine the order of the reaction and the activation enthalpy.
Background information ... Show more content on Helpwriting.net ...
In terms of log to the base 10 this is:
log k = log A В–Ea/ 2.303 RT
Reaction between Iodine ions and peroxodisulphate ions
S2O82–(aq) + 2I–(aq)  2SO42–(aq) + I2(aq)
In order to make the reaction clearer, during my experiment I will add starch and a small known amount of sodium thiosulphate (to act as a queching
agent). The thiosulphate ions turn iodine back to iodine ions:
2S2O32–(aq) + I2(aq)  S4O62–(aq) + 2I–(aq)
Which means that no starch–iodine colour will appear until all the thiosulphate has been used up. The amount of time taken for this occur (and the
reaction to suddenly turn blue) is the same amount of time for the reaction to produce the equvilant amount of Iodine.
Apparatus

(For making up solutions) weighing boats scales Beaker (150cm3)
3 Volumetric flasks (250cm3)
Distilled water
Glass rod
(for concentraion and temperature change experiments)
4 thermometers (0–110ВєC)
A large number of boiling tubes (roughly 50 depending on repeats)
5 Burettes with funnels for filling
5 Clamp stands (for burrettes)
Stopwatch
(for temperature change only)
Two large beakers (400cm3)
Chemicals
Freshly made starch solution
Pottasium Iodide (made to solution with conc. 1.00 mol dm–3)
Pottasium peroxodisulphate (made to solution with conc.

Review Paper On ' Shreyas Shah '
Review Paper on Microfluidics Shreyas Shah San Diego State University San Diego, CA, USA smsvapi@gmail.com Dr.Samuel Kassegne San Diego
State University San Diego, CA, USA kassegne@mail.sdsu.edu Abstract–Accurate and high throughput cell sorting enabling technology in molecular
and cellular biology, biotechnology and medicine. We classify these technologies as either active or passive. Active systems generally use external
fields (e.g., acoustic, electric, magnetic, and optical) to impose forces to displace cells for sorting, whereas passive systems use inertial forces, filters,
and adhesion mechanisms to purify cell populations. Cell sorting on microchips provides numerous advantages over conventional methods by reducing
the size of... Show more content on Helpwriting.net ...
Meanwhile, the growing interest in theranostics and personalized medicine, in which treatments are tailored to the prognoses of patients, is further
driving the demand for rapid and high performance cell sorting. This review will survey recent developments in microchip cell sorting by organizing
each technology into one of three principal categories based on its primary cell recognition modality: (i) fluorescent label–based, (ii) bead–based, and
(iii) label–free cell sorting. Within each category, several subsections are provided to further categorize each technology by the physical principles
governing the sorting process. We emphasize more recent technologies, especially those that integrate multiple functions on the same device toward a
fully integrated point–of–use device. II. FLUORESCENT LABEL–BASED CELL SORTING Fluorescent label–based cell sorting relies on fluorescent
probes or stains to identify cells by type. In traditional FACS, fluorescently–labeled cells organized in a laminar flow stream encounter a focused laser
beam that scatters into a detector. The fluorescent signal is then analyzed to assign each cell a type for discrete sorting, whereby in the case of FACS,
each cell is encapsulated into an aerosol droplet that is charged and

Gravimetric Analysis Of Copper Chloride Hydrate
Chemical formulas are central to chemistry; they describe, identify, and predict the properties of compounds. Chemical formulas can be found by a
process called gravimetric analysis in which components of a compound are isolated, their masses are found, and the mass differences recorded.
Gravimetric analysis can be helpful when finding the formula of an ionic hydrate, an ionic crystal bound to water molecules because it allows for the
mass of water to be found allowing for further separation of the remaining elements in the ionic compound. When water is removed from an ionic
hydrate, the ionic hydrate becomes an anhydrous ionic compound. Additionally, because of the Law of Definite Proportions, theratio of moles of water
released to ... Show more content on Helpwriting.net ...
The wire reacted with the solution to yield copper; any remaining aluminum was dissolved with a few drops of 6M HNO3. Following the isolation of
the copper, it was separated from the solution with a BГјchner funnel and flask. A piece of filter paper was weighed, and its mass was recorded. Then,
the filter paper was placed on the vacuum flask, which was turned on, and the copper solution was poured over it. The copper was also rinsed with
95% ethanol solution before being set on a paper towel to dry. Finally, one day after the previous step, the copper was weighed, and its mass recorded.
The recorded masses were then used to determine the mass of copper, chlorine, and water in the unknown copper chloride hydrate. The resulting masses
were used to find the formula of the unknown copper chloride hydrate according to CuxClynH2O.
Results
The mass of water in the unknown Copper Chloride Hydrate is 0.22g, as found by the difference in mass between the sample before and after
heating. The mass of copper is 0.29 grams, and the mass of chlorine is 0.49 grams. These values were found by isolating the copper then subtracting
the mass of the copper from the mass of the sample after heating to determine the mass of chlorine. The masses were converted into moles with the
general formula 1 mole/Molar Mass x mass of given element/compound. For example, the moles of copper were found by multiplying 0.29 grams by 1
mole/63.546 grams (Molar Mass of copper),

Qualitative Anion Tests Essay
Exercise 14: Qualitative Anion Tests PURPOSE: The purpose of this experiment is to identify some commonly occurring anions & to study some of the
reactions used for their identification. PROCEDURE: You must first determine to which of the three groups the various anions belong. Since no two
people observe the same event in exactly the same way it is important to also conduct specific confirmation tests on the known samples of each anion.
This information will help identify the anion present in the unknown solution. After determining to which group the unknown solution belongs the
specific confirmation test will enable you to conclusively identify which anion is present in the unknown solution. 1. Before beginning, set... Show
If the paper turns black (caused by PbS) this indicates the presence of sulfide. Thoroughly clean and dry the test tubes before beginning tests on
the next solution. Cleanup: Tightly cap the bottle of silver nitrate solution and put it in the Experiment 11 bag so it will be easy to find when you
need it for the next experiment. Flush any other remaining solutions down the drain with lots of water. Properly rinse all equipment used, then dry
and store for future use. OBSERVATIONS: | | |Data Table: Qualitative Anion Tests | | |Test Tube 1 |Test Tube 2 w/AgNO3 | |Test Tube 3 | |Name |w/HCl
| |w/HNO |Confirmation | | |NR |White ppt |Not dissolved |Gold color | |Bromide | | | | | | |Gas |White ppt |Dissolved

Metal Cations Lab Report
In this lab an unknown metal cation is identified by comparing chemical reactions of known metal cations with different ions to chemical reactions of
the unknown with those ions.Nine different metal cations are reacted with sulfate, iodide, carbonate, hydroxide, and ammoniaand observed. A
procedure is then planned using the original tests to identify the unknown metalcation. The nine different metal ions, aluminum, barium, cobalt, copper,
iron, magnesium, manganese, lead and zinc, were reacted with sulfate, iodide, carbonate, hydroxide, and ammonia. When reacted with sulfate
aluminum, cobalt, copper, iron, magnesium, manganese, and zinc all had no reaction. Barium and lead both formed white precipitates. When reacted
with iodide aluminum, barium, cobalt, magnesium, manganese, and zinc all had no reaction.... Show more content on Helpwriting.net ...
Aluminum had no reaction to the NH3 at all. When an excessamount of NH3 was added barium formed a white precipitate, cobalt formed a pink
precipitate,copper formed a bright blue precipitate, iron formed an red precipitate, magnesium had a whitesmooth precipitate, manganese had a tan
precipitate, and lead and zinc both turned clear.The unknown metal cation contains either zinc or lead. To discover which one is presentthe unknown is
tested with sulfate because only lead and barium react with the sulfate. Barium isnot an option in the unknown metal mixture, so if a reaction occurs it
is known that lead ispresent. In this case there is no reaction so zinc is present meaning that Zinc White is the presentpigment. Zinc white was
introduced in 1840. Next the unknown is tested for iron, copper, orcobalt. This is done by mixing the unknown

Investigating the Kinetics of the reaction between Iodide...
PLANNING
Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions
By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate
ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions, then the concentration of
Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking place. From these results, I hope to draw conclusions
as to the effects of these changes to the environment of the reaction on the rate and also determine the order of the reaction and the activation enthalpy.
Background information
The ... Show more content on Helpwriting.net ...
Effect of Temperature
A basic law of physical chemistry is that an increase in temperature causes an increase in the rate of any reaction. As the collision theory states, for a
reaction to take place the particles need to collide. If the temperature is increased, each particle has greater kinetic energy transferred from the heat
energy, and therefore is moving faster (the average speed of molecules is proportional to the square root of the absolute temperature.) The faster the
particles are moving, the more likely they are to collide and therefore the faster the reaction. Also, the more energy transferred to each particle due to
increased temperature the more likely it is to surmount the activation enthalpy and again the higher the number of effective collisions. As a general
rule, the rate of a reaction doubles for every increase of 10K in temperature.
The diagram below demonstrates the effect of temperature on the rate of a reaction. Despite the initial increase in the energy of particles of a lower
temperature, one can see that those at a higher temperature eventually surpass and lead to an overall higher amount of particles with energy higher than
the activation enthalpy and therefore a greater number of effective collisions.
The exact relationship between temperature and rate of reaction was first proposed by a Swedish chemist called Arrhenius in

Chemistry (Redox)
Experiment 1 : Redox Titration Using Sodium Thiosulphate
Abstract
This experiment is to determine the concentration of oxidizing solution using the iodine/ thiosulphate titration where the reducing solution is potassium
iodate solution and the oxidizing solution is sodium thiosulphate solution. Potassium iodate solution which is an oxidizing agent is added into an
excess solution of acidified potassium iodide. This reaction will release iodine. Potassium iodide is acidified with sulphuric acid and the iodine released
quickly titrated with sodium thiosulphate until it become light yellow. The iodine then detected with starch solution and it turn into dark blue solution
and titrated again with sodium thiosulphate until colourless. From ... Show more content on Helpwriting.net ...
B.Standardization of 0.1M sodium thiosulphate solution 1. A burette is filled with the 0.1M sodium thiosulphate solution to be standardized. There are
no air bubbles in the burette. 2. The initial reading of the burette is recorded in table 1.1. 3. 25–mL of standard potassium iodate solution prepared in
part A are pipetted into a 250–mL conical flask and a magnetic flea is added into conical flask. 4. 1 g of potassium iodide, KI, is weighed
approximately and it is placed in a 50–mL beaker. 5. 10.0 mL of 1.0M sulphuric acid solution are added and are swirled until all the KI dissolved. 6.
This solution is added to the conical flask containing the potassium iodate solution and it is immediately titrated with the sodium thiosulphate solution,
while it is stirred using a stirrer hot plate, until a ligth yellow solution is obtained. Then, the solution is diluted with distilled water until the total
volume is about 100 mL. Then, 1.0 mL of starch solution is added and the titration is continued until the blue colour disappears and the solution
become colourless. 7. The final reading of the burette is recorded in the table 1.1 . The procedures are repeated twice as the results is more accurate.
CALCULATIONS :
1. Complete chemical reaction equation for reaction between ; i. iodate and iodide

Naming A Chemical Compound : What Type Of Atoms You Are Using
Naming a Chemical Compound
To name a compound begin by deciding what type of atoms you are using. You should be able to clasify the pieces of the compound as
Metals with a known charge (Groups 1 and 2, Al+3 , Ag+ , Cd+2 , and Zn+2 )
Metals which can have more than one possible charge (most of the transition metals)
Nonmetals
Polyatomic ions (these always have a known charge)
All of the compounds you encounter will be one of two types:
1. Ionic Compounds (These are made by combining a metal with a nonmetal or a metal with a polyatomic anion, ionic compounds are held together by
the interaction of positive and negative charges)
These are made by combining a cation (an atom or polyatomic ion with a positive charge) with an anion (an atom or polyatomic with a negative charge.)
To name an ionic compound name the cation first and then the anion.
The Cation
A. If the cation has a single possible charge then simple list the metal or polyatomic ion.
This includes the metals of Group 1 (+1) and Group 2 ( +2)

Other common metals that have a single possible charge are Ag (+1), Al (+3), Zn (+2), and Cd (+2)
For example MgCl2. Mg is a metal who always forms a +2 cation Cl is a nonmetal, it's the anion This is magnesium chloride
Another example is NH4ClNH4+ is a polyatomic cation and is always +1 (ammonium) Cl is a nonmetal, it's the anion This is ammonium chloride
B. If the cation is a metal who can have different charges write down the

Factors Affecting Rate of a Reaction, Chemistry Design Lab
Chemistry Lab Report
(Design)
Factors affecting Rates of a Reaction (Kinetics)
KINETICS DESIGN LAB
Research Question:
Does the concentration of Potassium Iodide (KI) affect the rate of its reaction with hydrogen peroxide (H2O2) (of a fixed concentration)?
Introduction:
There are several factors that affect the rate of a reaction. Some of them being Pressure (if the reactants are Gases), Temperature, Presence of a
Catalyst, Surface Area of the reactant, and Concentration. According to the Collision Theory, during a reaction, particles collide with each other and
react if the geometry of the collision is correct. In this Experiment, we will investigate the effect of varying concentrations of Potassium Iodide on its
reaction with ... Show more content on Helpwriting.net ...
The Potassium Iodide particles will increase and the frequency of their collisions with Hydrogen Peroxide particles will also increase, causing them to
react quicker.
I hypothesize that as I increase the concentration of the Potassium Iodide Solution, the rate at which the blue–black starch complex covers the 'X'
marking on the tile, will also increase until a point where the rate will remain the same due to all the particles having already finished reacting.
1

Anion Analysis Lab
The Method to go about Cation/ Anion analysis is called Qualitative Analysis. With this method, one is able to determine if a Cation or Anion is
present in a substance. In 1834 Michael Faraday who was an English physicist and chemist introduced the word Anion and Cation to the world. The
name Cation means a positively charged ion and an anion meaning a negatively charged ion. Cations was given this name because it were observed
to be drawn to the cathode. Anion were given its name because it was also observed to be drawn to the anode in a galvanic device. When Cations and
Anions are combined they attract to one another to form an ionic compound such as a salt. The suffix on the words Anion and Cation is the word ion.
So what is an ion you ... Show more content on Helpwriting.net ...
A precipitate is formed when two soluble salts react in solution. The product is then one or more insoluble products. In a precipitate you can see a
solid that has separated from the aqueous solution. An example of a precipitate is when AgNO3 (Silver Nitrate) and NaCl (sodium Chloride) is
mixed. An insoluble compound is formed. In attempting to identify ions in a precipitate the dissolved substances must be removed. Next the mixture
of ions need to be mixed with a reagent that will assist in identifying the ions in which you are trying to identify. Commonly used compounds for
analysis of cations and anions are 6M HCl, 6M HNO3, 6M NaOH, and finally 6M

How The Molecules Is Capable Of Transporting Of The Cell...
Abstract The reasoning behind this experiment was to be able to specify which molecules are capable of transporting in and out of the cell through the
process of diffusion. Diffusion is the process where molecules move from a level of high concentration to low concentration and eventually stops once
the equilibrium is reached. This study was able to demonstrate that glucose, starch, and silver nitrate were all existing at different amounts. Results
began to show after around 40 minutes, but when we first started the experiment, no particles were present.
Introduction The technique in which molecules are able to move in and out of a cell is by the process of diffusion. Diffusion takes the molecules from a
high level of concentration to a low level of concentration. This method will be tested by taking different solutions, such as glucose, starch, and sodium
chloride, pouring them into a test tube, adding reagents to them, and analyzing which molecules are able transfer. Benedict's reagent will be added to
glucose, iodine to starch, and silver nitrate to sodium chloride. Glucose, starch, and sodium chloride will all be poured into the dialysis bag, which
will be noted as the cell, and will eventually be examined along with the extracellular fluid, which is the fluid outside of the bag, or around the cell.
The different directions that water is able to flow inside and outside of the cell includes hypertonic, isotonic, and hypotonic. Hypertonic solutions flow

Metals and Halogens Reactions
Metals and Halogens reactions
Elements such as fluorine, chlorine, bromine, iodine, and astatine belong to Group 7, Halogens. At room temperature, fluorine is a yellow gas,
chlorine is a pale green gas, bromine is a red liquid, and iodine is a purple solid. Astatine is a radioactive element, therefore it exists only in small
amounts. All the halogens exist in diatomic molecules. They have high ionization energies and are the most electronegative elements. Their electron
configuration ns2 np5 make them perfect elements in order to react with Group 1 and 2 metals since they want an electron which Group 1 and 2 are
willing to give. Therefore, out of all the main group elements, Halogens react vigorously with Group 1 and Group 2 metals. All ... Show more content
on Helpwriting.net ...
It was the triiodide ion that is mostly responsible for the orange–red–brown color since iodide was colourless and since iodine is not very soluble in
water. As the reaction was progressing, the coloured solution began to fade to orange, yellow and finally became colourless. As these colour changes
occur, the temperature of the solution was decreasing gradually until it has finally reached room temperature. This change in colour was due to two
factors. First, all of the solid and dissolved iodine had reacted with the zinc to produce iodide and zinc ions, both of which are colourless substances.
Secondly, the red–brown solution of triiodide ions also reacted with zinc metal to produce the colourless iodide ions.
In the other experiment three pieces of universal pH indicator were placed on a white spotting tile and drop of chlorine water, bromine water and iodine
water were transferred on each one of them. The colour of the pH indicators were observed and recorded as shown in the table 1.The halogen solution
were filled into the dimples of the spotting tile. They were put in columns and rows which had numbers (1, 2,3 and 4) and letters (A,B and C) in order
to differentiate each solutions. After

Calcium Chloride Lab Report
Based on the results of the test, the unknown substance was Calcium Chloride. Multiple tests were performed to determine the identity of the
substance. By comparing known positive results to the unknown substance, properties could be discovered about the substance. Most tests led to this
conclusion, however some tests did not follow the established properties of Calcium Chloride. Most of the physical properties of the unknown
substance were typical of Calcium Chloride. The unknown substance was crystals and odorless, just like Calcium Chloride1. However, the unknown
substance had a pH of 5 while Calcium Chloride has a pH of 92. This difference could be contributed to other substances in the solution. The solution
was made with tap... Show more content on Helpwriting.net ...
The unknown substance, when placed in the Bunsen flame, turned the flame a deep red. Therefore, the cation is Calcium4. Calcium burns red
because as the substance is heated up, the electrons get excited. As they fall back down to the normal state, they give off a wavelength. This can be
perceived as a color. The wavelength given off by burning Calcium corresponds to red wavelength in the visible light spectrum6. This test had to be
performed multiple times to confirm because the red flame is difficult to see. Also, the nichrome wire was used many times before this experiment.
There were other substances still on it and in order to prevent the tests from being incorrect, they had to be burned off. This is also what led to the test
being run multiple times to be sure that the unknown substance was the only substance

Describe What Happens When The Bunsen Burner
My first procedure that I completed was the filtration. When I mixed the lead (II) nitrate and the sodium iodide together, I got a bright yellow liquid
that turned out to be lead (II) iodide. I believe I did this part of the procedure correct because the color was not too pale and I did not use too much lead
(II) nitrate or sodium iodide. I used the correct amount to get the results that were listed on the laboratory, In procedure D, Glassworking, cutting the
glass came out great. I followed all safety procedures and it snapped perfectly. Although, I could have fire polished the cut glass a little bit more but
could not due to time constraints. A problem I could have had during this procedure is not having the Bunsen Burner flame too low where

The Formula Of Zinc And Hydrochloric Acid
In this lab, we balanced the equation xZn(s) + yHCl(aq) в†’ ZnxCly (s) + y/2H2(g) by the information obtained from the lab. When zinc and
hydrochloric acid are mixed together, the reaction took place in an evaporating dish that was accompanied by hydrogen gas. Then we measured out the
mass of zinc and chlorine in the reaction and calculated the empirical formula of zinc chloride which was ZnCl8. Based on the conservation of mass,
we balanced the equation and got Zn(s) + 8 HCl (aq) в†’ ZnCl8 (s) + 4 H2 (g). In the second part of the experiment, we obtained copper wire and
sulfur from the instructor. Then we measured out the mass of copper and added proper amount of sulfur to cover the copper wire. During the lab,
copper with sulfur was heated, and the reaction was carried out. We saw the blue flame occurred on the crucible. We determined the empirical formula
of copper sulfide, which was Cu2S. Then, the equation was balanced easily from the obtained data which was 2Cu + S = Cu2S.
Introduction:
The purpose of this lab is to become familiar with chemical formulas and how they 're obtained. Chemical formulas represent what are produced from a
chemical reaction. Compounds composed of molecules are called molecular compounds, which may or may not contain more than one type of atom.
Chemical formulas indicating actual numbers and types of atoms in a molecule are called molecular formulas, whereas chemical formulas that indicate
only the relative numbers of atoms of a type 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 Helpwriting.net ...
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

Of The Rate Of Reaction Of Peroxydisulfate Ion With Iodide...
The objective of this experiment is to be able to measure the rate of reaction of peroxydisulfate ion with iodide ion. Students will be allowed to
calculate the reaction order, partial order and rate constant of four different reaction solution. Furthermore, observe and record the time when the color
changes when KI solution (potassium iodide), starch solution, Na2S2O3 solution (sodium thoisulfate), KNO3 solution (Potassium nitrate) and EDTA
solution is mixed in an Erlenmeyer flask. Measuring a reaction rate is not only significant to this experiment or chemistry but also in real life. For
example, according to Roughton, F. J., & Forster, R. E. (1957), before an individual is diagnosed with difficulties breathing due to the low capacity of...
Show more content on Helpwriting.net ...
Each reaction would be carried out by mixing five different solutions four times separately and each reaction is consisted of KI solution, starch
solution, Na2S2O3 solution, KNO3 solution and EDTA solution. Theconcentration of each solution varies because the first reaction include 25.0ml
KI solution, 1.0ml starch solution, 1.0ml Na2S2O3 solution, 48.0ml KNO3, 1 drop EDTA solution and the total volume eqaul 75.0ml. The second
reaction include 25.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1 drop EDTA solution and total
volume equal 50.0ml. The third reaction include 50.0 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3 solution 23.0 mL KNO3 solution 1
drop EDTA solution and the total volume equal 75.0 mL and the fouth reaction include 12.5 mL KI solution 1.0 mL starch solution 1.0 mL Na2S2O3
solution 35.5 mL KNO3 solution 1 drop EDTA solution and total volume equal 50.0ml. After obtaining all of the solutions and seven different test
tubes of 1.0ml Na2S2O3 solution which should be pour into the Erlenmeyer flask whenever the color of the solution changes. To calculate the reaction
rate of each reaction the timer should start immediately when all of the solutions are mixed. Once all of the solutions have been mixed the students
should observe as well as record the time of the reaction when the color change to dark blue and one of

Effect Of Aa Content On The Swelling Ratio Of Hydrogel
Effect of AA content on the swelling ratio of hydrogel
Fig. 3b shows the effect of AA on the Q value of hydrogel. With increasing concentration of AA, the Q values of hydrogels increased and then
decreased. When AA amount was more than 7 g, the Q values of hydrogels decreased because when the concentration of AA was high, the collision
probability between monomers would increase, thus increasing the graft length of sulfonated cellulose, favoring the formation of a polymeric network
at higher Q values of hydrogels. HIGh AA concentrations would lead to self–polymerization and lower swelling ratio. The best ratio between
sulfonated cellulose and monomer was determined as 1:7.
3.5 The effect of KPS on the swelling ratio of hydrogel
Fig. 3c shows the effect of KPS on the Q value of hydrogel. The Q values of the hydrogels increased, followed by a decrease with increasing amount
of KPS. The maximum Q value was observed at 2% KPS, because polymerization was initiated by the free radicals generated from KPS under heat.
More initiators would produce more free radicals that can enhance grafting efficiency. Therefore, the hydrogel formation was enhanced and Q
increased. However, too much initiator would produce too many free radicals, thus increasing the collision probability between free radicals, eventually
terminating the reaction. The generated short graft chains would be difficult to form a 3D network, decreasing the Q value.
3.6 The effect of neutralization degree of AA on

Jci Holland Case
JCI Holland Facility Blood–Lead Level Problem Analysis February 14, 2014 Prepared For: Jamie Morris Toledo Facility EHS Manager Johnson
Controls Battery Division 10300 Eber Rd. Holland, OH 43528 Prepared By: Dennis Prater II Chief Executive Officer DenPrater EHS Services 1234
Safety Way. Toledo, OH 43614 1234 Safety Way Toledo, OH 43614 419
–765–4321 2015 JCI Holland Blood Lead Levels February 14, 2015 Johnson
Controls Battery Division 10300 Industrial St. Holland, OH 43528 Attention: Jamie Morris, EHS Manager JCI Holland Facility Blood–Lead Level
Problem Analysis Our company has completed our investigation into factors that may be leading to increased blood lead levels at your Holland
facility. Our company has spent four months... Show more content on Helpwriting.net ...
Nonexistent hoods and inadequate hoods should be replaced and installed immediately. The low on nonexistent fpm's produced by these hoods are in
violation of OSHA regulations. Putting garage doors on the equipment doors should be done after this. The free flow of lead from POS to other parts
of the plant is of great concern to everyone's health. Keeping the lead in the POS department would make it much easier to control. The installation of a
wind tunnel between POS and COS should be installed in the next couple years. A large sized capital improvement investment will be required for this
construction. Personal hygiene, facility sanitation practices, and employee dietary needs should be instituted immediately. These changes have very
little cost and do not require much labor downtime. Conclusion The blood–lead levels in the Holland, Ohio facility are the worst not only in the United
States, but the world as well. In order to lower these blood lead levels each changes and improvements must be made in all six categories outlined in
this report. The changes range from simple policy changes that at little or no cost, to engineering controls that will be fairly expensive. I look forward
to meeting with you and other plant leadership to discuss this study, and how to we should move forward with these recommendations to reduce blood
lead levels in the Holland, Ohio facility. Works

Identify And Distinguish Between Ions In The Halide Family...
Andrea Moreno
9 February 2016
Block A
Calculations:
There are no calculations.
Analysis/ Critical Thinking Questions:
1. Explain what information you found from each of the first three (or four) parts of this experiment. Make separate clear, concise and grammatically
correct statements for each part. Someone else should be able to take your answers and do the unknowns successfully. Only fluoride precipitates with
calcium ion, not with silver. All three of the others precipitate with silver: chloride is white at first, then turns gray, bromide is sort of ivory colored
and iodide is yellow. Silver chloride is soluble in ammonia and in sodium thiosulfate solution. Silver bromide dissolves in ammonia, if you stir it, but
only a little bit in ... Show more content on Helpwriting.net ...
(The problem/objective, materials, procedures and safety notes above are taken from "World of Chemistry" by John Little, 2013)
Hypothesis: If the solutions react with a particular halide ion, then it will be able to identify each halide as an unknown and subsequently identify two
halide ions mixed together in solution.
Hypothesis Supported or Not Supported: This hypothesis is supported.
Data to Support/ Not Support the Hypothesis:
The first unknown substance could be fluoride because the reaction it had with Ag+ was almost the same reaction.
The second unknown substance is bromide because both of them had the same reaction of turning darker yellow.
Error Analysis:
There is no error analysis.
Improvements:
There are no improvements.
Major Scientific Principle Discussion: The scientific principle that was supported by the lab was to conduct tests on solutions of the four halide ions.
The tests consisted of comparing the responses of each of the halide ions to each test and to identify two unknowns based on the results obtained using
known solutions of the anions. This activity relates to informations from the textbook and class discussions because of the anion analysis we are
learning. The outcome of this activity connects to what occurs in the world around us because we can learn to make observations. This lab was

important, because of the small size, students

The Swallow Man
The next lesson was, "Asking a stranger for something is the easiest way to ensure that he will not give it. Much better simply to show him a
friend with a need" (62). In order to get supplies, the Swallow Man would create stories that make strangers feel bad for him or to make it seem
like they have something in common. This is how their trust was gained. Only then would the Swallow Man mention anything they were looking
for. Using this method, the Swallow Man could get food and supplies that strangers had no need of anyway. Another lesson of the Swallow Man
was, "Regret is like golden jewelry: at the proper moment it may prove immeasurably valuable, but it is rarely wise to advertise its presence to
strangers" (93). If a person is seen having regrets, then they may be taken advantage of. That is why it is imperative that even if a person does have
regrets about their actions, they should not show that they do. Otherwise, the witness of the regret may see weakness and think that they can
overpower that person. A similar lesson is, "Transitions are periods of weakness" (160). This transition is similar to regret. If a person is seen as
being weak during transitions, they can be taken advantage of in the same way they can with regret. That is why the Swallow Man avoided both of
these situations whenever he could. A lesson used in the DwГіr was, "Carrying light in darkness is an invitation to be snuffed out. Learn to keep your
sight in the dark" (196). Seeing in the dark is

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