Kinetics of Iodide and Peroxodisulphate Reaction

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
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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 ...
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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

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

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 more content on
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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*mol−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 → 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

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
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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

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

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 more content on Helpwriting.net ...
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

The Formula Of Zinc And Hydrochloric Acid
In this lab, we balanced the equation xZn(s) + yHCl(aq) → 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)
→ 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

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, the ratio of moles of water released to ... Show more content on
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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 Büchner 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),

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 content on Helpwriting.net ...
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

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,

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 more content on Helpwriting.net ...
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

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 Chloride Sucrose
Aluminum Mass of Sample (g) 4.38 grams 6.92 grams 1.28 grams Molar Mass (g/mol) 58 g/mol
342 g/mol 27 g/mol Moles of sample 0.076 moles 0.02 moles 0.047 moles Number of representative
particles in sample 4.6 x 1022 NaCl Particles 1.2 x 1022 Sucrose Particles 2.8 x 1022 Aluminum
Particles Water Hydrogen Peroxide Rubbing Alcohol Chemical Formula H2O H2O2 C3H8O
Density (g/mol) 1.00 g/mol 1.46 g/mol 0.785 g/mol Volume (g/mol) 100 mL 100

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

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
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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. The concentration 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

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. 7 NO. 8 NO. 9
Silver nitrate PPT
Table 2: Test for unknown solid 7
Table 3: Test for unknown solid 8 and 9 NO. 7
Sodium hydroxide
Calcium nitrate PPT
PPT = Precipitation NO. 8 N0. 9
Sodium chloride
Copper sulphates PPT Table 4: Name of solid 7, 8 and 9
Number of the ionic solid No. 7 No. 8 No. 9
Name of the solid Sodium carbonate Zinc nitrate Barium 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 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 Dwór 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

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

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

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 µg/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 Björkholm 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

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

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

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 Helpwriting.net ...
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

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

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

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 NH4Cl NH4+ 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

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

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

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
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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

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

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

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

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 –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 (0–110ºC)
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.

Lab Report
Lab Report 1
 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 Helpwriting.net ...
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 Büchner 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
Büchner 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

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

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

Kinetics of Iodide and Peroxodisulphate Reaction

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Kinetics of Iodide and Peroxodisulphate Reaction