FTIR spectroscopy of SO2

FTIR spectroscopy of SO2 Abstract In this lab, the IR spectrum of SO2 gas was taken. The spectrum was then used to determine which peaks corresponded to the vibrational modes of SO2 ­. Once the modes had been determined, the experimental wavenumbers of the v1 and v3 modes and the overtones were used to determine the anharmonicity of the two different modes. While there was a difference between the two modes anharmonicity, overall there was not a significant difference. The modes and their corresponding wavenumbers were also used to calculate the force constants of SO2. The experimental data produced a force constant k1 with 3.112% error while the kÃŽ ´/l2 constant had a 2.963% error. Introductions IR spectroscopy is the detection of a transmittance or absorption intensity of change as a function of frequency1. In recent years, Fourier transform spectrometers replaced the traditional dispersive spectrometer because they are faster and more sensitive. They have made it possible to analyze many areas which were not possible with the dispersive spectrophotometer. The difference is the simultaneous examination of all frequencies. The three basic spectrometer components in a FT system are the radiation source, interferometer and detector. The radiation source in precision FTIR instruments is often water-cooled in give it more power and stability2. Figure 1. shows a diagram of the interferometer and the schematics of the spectrophotometer as a whole. The interferometer has the following three components: a moving mirror, fixed mirror, and a beamsplitter.. The beamsplitter is a semireflecting geranium thin film of small particles deposited on flat KBr substrate. Radiation from the broadband IR source is focused into the interferometer, and hits the beamsplitter. Once the beam hits the beam splitter, half of it is transmitted to the fixed mirror while the other half is transmitted to the moving mirror. The changing position of the moving mirror relative to the fixed one generates an interference pattern and causes the two beams to oscillate in and out of phase. When the beams are in phase, there is a constructive interference resulting in the maximum detector response. However, when the beam is out of phase, there is a deconstructive interference between the two beams. Once they have been reflected from both mirrors, they recombi ne at the beam splitter. The recombined beam passes through the sample and then focuses on the detector2. The intensity of the radiation hitting the detector will vary in a sinusoidal manner while the mirror is moving at constant velocity. The record of the interference signal is the interferogram and is a time domain spectrum. The detectors response changes versus time within the mirror scan are recorded. When a sample absorbs at a certain frequency, the amplitude of the sinusoidal wave reduces proportionally to the amount of sample in the beam. In an IR spectrophotometer, this process happens in three component frequencies, which creates a more complex interferogram2. To convert these interferogram recordings to the IR spectrum, a Fourier transformation is used. Small, precise intervals are used during the mirror scan. The rate of the sampling behavior is controlled by a monochromatic beam produced by a helium neon laser focused on a separate detector2. For this analysis, the mid IR spectrophotometer utilized a KBr beamsplitter and a mercury cadmium telluride (MCT) detector. MCT detectors are photon detector with a dependence on the quantum nature of radiation. They also exhibit very fast responses. They must be at a constant temperature of 77^(o)K, the temperature of liquid nitrogen. It is faster and more sensitive than the alternative detector, the deuterated triglycine sulfate (DTGS) 2, which was used for the far IR analysis. The cell used to hold the SO2 gas can be seen in Figure 2. A molecules energy can be split into three components: the electrons motion, the constituent atoms vibrations and the whole rotation of the molecule. While electronic transitions happen on a short timescale, rotational transitions happen on a longer time scale. When a molecule is placed in an electromagnetic field, such as light, energy from the light is transferred from the field to the molecule. This happens upon the satisfaction of Bohrs frequency condition: ΔE = hv When a molecule is excited from one state to another, the energy difference between the two states is absorbed by the molecule. When the molecule reverts back to the previous state, the change in energy which was absorbed upon excitation is then emitted1*. A molecule will be excited by photons which possess the appropriate energy3. Vibrational transitions are observed in the infrared (IR) spectra which are about the 103 ~ 104 cm-1 region. These transitions are caused by the vibration of the nuclei constituting the molecule. The rotational transitions occur at 1-103 cm-1 region, the microwave region, while the electronic transitions occur at 104-106 cm-1 region, the UV-visible region. As the vibrational quantum number v increases, the rotational intervals tend to decrease. The vibrational fine structure of electronic transitions can give insight to the structural and bonding information about molecules which are electronically excited1*. A system displaced from its equilibrium force will be restored due to a restoring force provided by the elasticity of the system. However, there is a property of inertia which causes the system to over correct for the displacement. The back and forth actions of elasticity and inertia cause the system to have oscillatory motion4. When the potential energy is graphed versus the internuclear separation, a perfect harmonic oscillator forms a parabola. The energy spacing in a harmonic oscillator does not change throughout the well of the parabola and is equal to hω where ω=km12 and the zero point energy is Eo= 12hω When a system is not a perfect harmonic oscillator, it is considered anharmonic. Anharmonicity forces the right side of the parabola to widen and asymptotically approach zero. The spaces between the permitted states are not evenly spaced as they were in the harmonic system5. The comparison of the two graphs can be seen if Figure 3. One of the possible ways to calculate xe, a term which shows the anharmonicity of a system is to graph ?G/? versus (?+1). This yields a graph with an equation as follows ΔGv=v+ 1xeve+ ve By dividing the xeve term by ve, the xe term is found. The larger this number, the more anharmonic the system is and vise versa5. Covalent bonds of molecules are not rigid as ball and stick models would suggest, but rather they can be compared to stiff springs which are capable of stretching and bending. More energy is required to stretch and compress a bond than it does to bend it. There is a direct relationship between the energy or frequency which characterizes the stretching vibration of a bond and the bond dissociation energy3. The major factors which are influencial in the stretching frequency of a covalent bond can be seen in the following equation: v = 12rck(m1+m2)m1+m2 where v is the frequency, k is the force constant, c is the speed of light, and m1 and m2 are the masses of the two atoms on each end of the bond. This equation corresponds to the rigidness of the oscillation. However, it should be noted that not all molecular vibrations are capable of being observed in the infrared region. In order to be seen in an IR spectrum, a vibration must cause a change in the dipole of a molecule. This change in charge distribution allows the molecule to absorb infrared light. There is a proportional relationship between the change in charge distribution and the absorption: the greater the change, the stronger the absorption3. All vibrating physical objects have a set of normal modes6. A normal mode can be defined as a simple harmonic oscillation which occurs about an area which is local and low in energy. The normal modes are determined by the systems structure R and its energy function V(R ). Any motion can be expressed as a superposition of normal modes when a pure harmonic V(R ) is being considered. However, the near minimum potential can still be approximated by a harmonic potential for an anharmonic V(R ). Also, small-amplitude motions can still be described by the sum of normal modes. This means that all systems behave harmonically at low temperatures7. For SO2, it is necessary to have nine Cartesian coordinates in order to determine the positions of all three nuclei. Therefore, the molecule is considered to have nine nuclear degrees of freedom. The first three are necessary to describe the position of the center of mass of the molecule. If these three degrees change, it represents the translational movement of the molecule in space. The next three degrees of freedom refer to the orientation of the molecule. These three degrees can be described as the angles of the molecule. If these three degrees change, then the molecule has rotated. The three remaining coordinates are those used to describe the relative positions of the three atoms. These are called vibrational coordinates8. To describe the vibrations of a bent trigonal molecule, it makes sense to use the valence coordinates. The valence coordinates consist of the two bond lengths and the bond angle. However, they do possess a drawback. If energy is put into a bond so that it stretches, to observe how the molecule reacts is difficult due to the energy put into the stretched bond quickly flowing into the vibrations of the other bond in the molecule. Because of this, it is said that the stretching of a single bond and other vibrational motions are coupled8. By varying the coordinates, which are the linear combinations of changes in the bond lengths and bond angles, a good uncoupled approximation can be made. These coordinates are called the normal coordinates. Motions which take place in these coordinates are appropriately called normal modes of vibration. The center of mass does not move in these coordinates8. A non symmetric molecule with N number of atoms will have 3N-6 normal modes. This means SO2 will have 3(3)-6 = 3 normal modes. The normal modes for SO2 can be seen in Figure 3. The symmetric stretch is labeled as v1, the bend is labeled v2, and the asymmetric stretch is labeled v3. When a molecule is exhibiting one of the vibrational modes, it travels the path indicated by the arrow, stops, and then returns back to its starting position8. It is possibly to express the three normal modes as a potential-energy function written in terms of bond stretching and angle bending as shown in the following equation: V = 12k1(R1-Re)2+ 12k1(R1-Re)2+ 12kb(ÃŽ ¸-ÃŽ ¸e)2 where R1 and R2 are the first and second bond length of S-O, Re is the equilibrium S-O bond length, ? is the bond angle of O-S-O, and ?e is the equilibrium value. The constants ks and kb ­ are for the stretching and bending respectively9 ­. Though the derivations are difficult, it was found that the following equations are derived from eq. (1) and are used to calculate both constants: 4r2v32 = 1+2momssin2ÃŽ ±k1mo 16r4v12v22 = 21+2momssin2k1moÃŽ ±kÃŽ ´l2 4r2v12+v22 = 1+2momscos2ÃŽ ±k1mo+2mo1+2momssin2ÃŽ ±kÃŽ ´l2 where v# is the wavenumber of that particular mode, 4?3 is expressed as 5. 8918E-5 in order to obtain units of Nm-1, mo is the mass of oxygen, ms is the mass of sulfur, ? is 59.75^(o), and k?/l2 is the same as the kb constant used in equation (6)10. Diatomic molecules possess only one vibrational coordinate which is quantized. This means that only specific results will be obtained for the value of the vibration. The quantum mechanical harmonic oscillator upon first approximation gives the allowed levels of a diatomic molecule. Polyatomic molecules are similar. Each normal mode has quantized energy, and can be approximated by the harmonic oscillator model when at low energy levels. The frequencies associated with bending tend to be lower than the frequencies associated with stretching10. It is possible to see normal modes via IR spectroscopy if they have a change in dipole in the molecule when it stretches or bends10. All of the normal modes in SO2 are IR active and therefore can all be seen in the IR spectrum at the fundamental frequency. It is possible to observe other weak bands in the spectrum which are a result of overtones. Overtones occur because anharmonicities. They usually happen at integer multiples of 2 or 3 of the fundamental frequencies and are caused by two modes being simultaneously excited10. These bands are located at frequencies which are approximately the sum or difference of the two modes which were excited and are weak10. Method About 1.5g of drierite was weighed out and placed in the barrel of a syringe and the plunger was inserted almost entirely into the barrel. A 3 cm piece of rubber tubing was attached to the tip of the syringe. A 1.5 g of sodium hydrogen sulfite was measured and placed in a vial cap that was small enough to fit into the syringe barrel. The filled vial cap was then into the syringe using a bent spatula to prevent the sodium hydrogen sulfite from spilling into the barrel. The plunger was pushed into the syringe as far as it would go. To ensure that none of the sodium hydrogen sulfite was spilled, the syringe was placed tip down in a beaker. The next step was placing 15 mL of 6 M HCl into a small beaker. All of the acid was then drawn into the syringe containing the vial cap very carefully as to not let any of the acid mix with the sodium hydrogen sulfite. The plastic lid was then screwed onto the syringe. Once the cap was secure on the tip, the syringe was shaken so that the acid and the sodium hydrogen sulfite mixed. As SO2 gas was being produced, the plunger on the syringe was pulled out simultaneously. The high pressure of the gas in the syringe caused the cap on the tip to leak so it was necessary to apply pressure to the tip to prevent it from spitting acid out. Once the reaction had stopped producing gas, the syringe was inverted so that the tip was pointing up and the liquid was at the bottom of the barrel. The cap was removed and the tip was connected to the other end of the rubber tubing attached to the syringe containing drierite. At this point the syringe containing drierite was above the syringe containing the SO2 gas. As the plunger in the bottom syringe was being pushed in, the plunger in the top syringe was being pulled out; making sure no liquid was pushed through the tubing and into the top syringe. The top syringe, now containing the SO2 gas, was capped and allowed to sit for five minutes in order for the drierite to dry the SO2 gas. The excess HCl in the reaction syringe was expelled into a waste beaker. 15 mL of NaOH was placed in a beaker and then drawn up into the syringe in order to destroy any remaining SO2. The NaOH was then also expelled into the waste beaker. After the syringe containing the gas had sat for five minutes, the IR gas cell was placed in the hood. The syringe containing the SO2 was then attached connected to the gas cell using another piece of rubber tubing. Both stopcocks on the gas cell were opened and the gas was pushed into the cell. Both stopcocks were then immediately closed to prevent any of the SO2 from leaking out. A spectrum in the range of 700-2500 cm-1 was obtained using an FTIR spectrophotometer. In order to get a good spectrum from the mid IR range, the cell was undiluted. However, to obtain a good spectrum in the far IR range, it was necessary to dilute the gas cell. Once the spectrum had been obtained, the gas cell was placed inside a fume hood. Both stopcocks were opened up and a syringe was used to flush air through the gas cell. The gas cell was then placed in a vacuum sealed dessicator with the stopcocks open in order to dry out any moisture that may have entered the cell during the experiment. Results The IR spectra of SO2 can be seen in Figure 5. By looking at what wavenumbers the peaks appeared at, it could be concluded which peak corresponded to each vibrational mode of SO2. The bending of a molecule happens at lower wavenumbers, so it was concluded that graph in the top right corner corresponds to the ?2 vibration. It was known from literature that the stretches occur somewhere between 1000 and 1500 cm-1 so the graph in the bottom right must correspond to the overtones of SO2s ?3 and ?1 modes. It is known that asymmetric stretches always correspond to higher wavenumbers. So it was concluded that the next two peaks on the spectrum were ?1 and ?3 respectively. The actual experimental wavelengths of each mode can be seen it Table 1. There are two overtones present, one from the ?1 mode and another from the ?3 mode. The lower frequency overtone corresponds to the lower-frequency mode. Thus the lowest overtone is that of ?1 while the second seen overtone comes from the ?2 mode. Using the experimental wavenumbers for each mode, both constants could be found using eq. (7) first to solve for k1. This values was calculated to be 1000.858 Nm-1. The litereature value is 1033 Nm-1 and the percent error in the experimental value was 3.112% The calculated value of k1 was then used in eq. (8) to find the k?/l3 constant. The second constant was calculated to be 78.60 Nm-1. Literature value for this constant is 81 Nm-1 and the percent error in the experimental calculation was 2.963%. To evaluate the effectiveness of this method for finding the constants, both sides of eq. (9) were solved for. The left side equaled 93.77 Nm-1 while the right side equaled 95.54 Nm-1. The percent difference between these two values is 1.85%. In order to determine the harmonicity of each of the modes of vibration, the ve and vexe values were calculated. This was done by graphing ?G/v versus (v + 1) in Microsoft Excel. The ?G corresponds to the wavenumber of the overtone seen on the IR spectrum. ?G was then divided by v. The overtones corresponded to v=2 while the normal mode bands corresponded to ?=1. Graphs for both the ?1 mode and ?2 mode can be seen in Figure 6. Excel was then used to fit a trend line and produce a y = mx + b equation for the data. The slope of the equation was vexe and the intercept was ve. To determine the anharmonicity of the two modes, it was necessary to solve for xe. This was done using eq (4). The calculated values for xe in the ?1 mode was 1.0612 and for the ?3 mode was 0.07891. This means that the ?1 mode is more anharmonic than the ?3 mode. Conclusion For this lab, SO2 ­ was prepared and then studied via FTIR spectroscopy. The three modes of SO2 were identified on the IR spectra obtained. It was determined that the lowest energy of bending correlated to the lowest frequency peak. The second highest frequency peak was determined to be ?1 since the symmetric stretch is lower in energy than the asymmetric stretch (?3) which is the third highest frequency peak. The wavelengths determined from the IR spectra were used to calculate the constants k1 and k?/l3. It was determined from the numbers crunched from eq. (6) that the used method of determining the constants was an accurate method. Also, the anharmonicity of the modes ?1 and ?2 were calculated and compared. The graph of ?G/vversus (v + 1) produce an equation of y = mx + b which provided the values of xeve and v ­e. These values were then used to find xe, which described the anharmonicity of each mode. The ?1 mode was found to be more anharmonic due to its greater xe value whil e the ?3 was found to be more harmonic. Refrences What is Infrared Spectroscopy?. (n.d.). Mount Holyoke College, South Hadley, Massachusetts. Retrieved December 11, 2009, from http://www.mtholyoke.edu/~mlyount/MySites/ForensicSpectroscopy/WhatIsIR.html Nakamoto, Kazuo.Infrared and Raman Spectra of Inorganic and Coordination Compounds. Sixth Edition ed. Hoboken, NJ: Wiley Sons, Inc., 2009. Print. Hsu, S. (n.d.). Infrared Spectroscopy. prenhall.com. Retrieved December 6, 2009, from www.prenhall.com/settle/chapters/ch15.pdf Chem.msu.edu. (n.d.). Nature of Vibrational Spectroscopy. Retrieved November 30, 2009, from 2http://www.cem.msu.edu/~reusch/VirtualText/Spectrpy/InfraRed/irspec1.htm#ir1 The Simple Harmonic Oscillator. (n.d.). PAWS Personal Accessible Web Space Kettering University. Retrieved December 12, 2009, from http://paws.kettering.edu/~drussell/Demos/SHO/mass.html Atkins, P., Friedman, R., Paula, J. D. (2008). Rotational and Vibrational Spectra. Quanta, Matter and Change: A Molecular Appraoch to Physical Change (pp. 315-318). New York: W. H. Freeman. Normal mode Wikipedia, the free encyclopedia. (n.d.). Wikipedia, the free encyclopedia. Retrieved December 11, 2009, from http://en.wikipedia.org/wiki/Normal_mode Normal Mode (Harmonic) Analysis. (n.d.). Center for Molecular Modeling. Retrieved December 11, 2009, from http://cmm.cit.nih.gov/intro_simulation/node26.html Vibrational Spectroscopy. (n.d.). med.upenn.edu. Retrieved December 10, 2009, from www.med.upenn.edu/bmbgrad/Faculty/Master_List/Vanderkooi/course_notes/8.vibrational.pdf Sulfer Dioxide Vibration. (n.d.). d.umn.edu. Retrieved November 30, 2009, from www.d.umn.edu/~psiders/courses/chem4644/labinstructions/SO2spartan.pdf Infrared Spectroscopy of SO2. (n.d.). Spectroscopy and Structure Chem 4591. Retrieved November 30, 2009, from 3http://www.colorado.edu/chemistry/chem4581_91/SO2.pdf

Health Care” Right or Privilege” Essay

There has been an active debate about health care reform among many Americans in the United States. Some the recent concerns and questions involving a right to health care are access, fairness, efficiency, cost, choice, value, and quality. Health Care† Right or Privilege† Health care in the United States is provided by many separate legal entities. Health care facilities are largely owned and operated by the private sector. Health insurance is now primarily provided by the government in the public sector, with 60-65% of healthcare provision and spending coming from programs such as Medicare, Medicaid, TRICARE, the Children’s Health Insurance Program, and the Veterans Health Administration (â€Å"Health care in the United States.,† 2011). In the United States, ownership of the health care system is mainly in private hands, though federal, state, county, and city governments also own certain facilities. The non-profit hospitals share of total hospital capacity has remained relatively stable (about 70%) for decades. There are also privately owned for-profit hospitals as well as government hospitals in some locations, mainly owned by county and city governments. There is no nationwide system of government-owned medical facilities open to the general public but there are local government-owned medical facilities open to the general public. The federal Department of Defense operates field hospitals as well as permanent hospitals (the Military Health System), to provide military-funded care to active military personnel. The federal Veterans Health Administration operates VA hospitals open only to veterans, though veterans who seek medical care for conditions they did not receive while serving in the military are charged for services(â€Å"Health care in the United States.,† 2011). Hospitals provide some outpatient care in their emergency rooms and specialty clinics, but primarily exist to provide inpatient care. Hospital emergency departments and urgent care centers are sources of sporadic problem-focused care. Surgery centers are examples of specialty clinics. Hospice services for the terminally ill who are expected to live six months or less are most commonly subsidized by charities and government. Prenatal, family planning, and â€Å"dysplasia† clinics are government-funded obstetric and gynecologic specialty clinics respectively, and are usually staffed by nurse practitioners (â€Å"Health care in the United States.,† 2011). Over 45 million Americans are uninsured or underinsured. Those living in poverty exhibit the worst health status. Employment, education, income, and race are important factors in a person’s ability to acquire healthcare access. Having established that there are people lacking healthcare access due to multi-factorial etiologies, the question arises as to whether the intervention necessary to assist them in obtaining such access should be considered a privilege, or a right(â€Å"Health care in the United States.,† 2011). An active debate about health care reform in the United States concerns questions of a right to health care, access, fairness, efficiency, cost, choice, value, and quality. Some have argued that the system does not deliver equivalent value for the money spent. The USA pays twice as much yet lags behind other wealthy nations in such measures as infant mortality and life expectancy, though the relation between these statistics to the system itself is debated. Currently, the USA has a higher infant mortality rate than most of the world’s industrialized nations and life expectancy is ranked 42nd in the world. (â€Å"Health care in the United States.,† 2011) The Patient Protection and Affordable Care Act (PPACA) is a United States federal statute signed into law by President Barack Obama on March 23, 2010. The law (along with the Health Care and Education Reconciliation Act of 2010) is the principal health care reform legislative action of the 111th United States Congress (à ¢â‚¬Å"Patient Protection and Affordable Care Act,† 2011). A majority of the states, and numerous organizations and individual persons, have filed actions in federal court challenging the constitutionality of PPACA. As of September 2011, federal appellate courts are almost evenly divided on the constitutional issues raised in this litigation; at the district court level, three judges upheld the constitutionality of PPACA and three declared it unconstitutional, in part. PPACA includes numerous provisions to take effect over several years beginning in 2010(â€Å"Patient Protection and Affordable Care Act,† 2011). Perhaps the biggest disappointment of our legislative and executive branches of government in the creation of â€Å"Obama Care† is that they lacked vision and a concrete understanding of the bigger picture when crafting and ‘pushing’ this new agenda. With a broad brush assessment, we can see that the architects of â€Å"Obama Care† failed in addressing the following two areas: Bridging Safety loophole s that needlessly lead to over 100,000 medical-related deaths and hundreds of thousands more in injuries in American medical institutions each year. Propagating the misperception that a one-tiered, national health system plan, with greater centralized control, can work somehow ‘better’. One of the provisions I disagree with is the shared responsibility requirement, commonly called an individual mandate, it requires that nearly all persons not covered by Medicaid, Medicare, or other insurance programs purchase and comply with an approved insurance policy or pay a penalty. The only people exempt from the mandate are individuals of recognized religious sects or those individuals able to obtain a waiver from the Internal Revenue Service in cases of financial hardship(â€Å"Patient Protection and Affordable Care Act,† 2011) . The Act’s provisions are intended to be funded by a variety of taxes and offsets. Major sources of new revenue include a much-broadened Medicare tax on incomes over $200,000 and $250,000, for individual and joint filers respectively, an annual fee on insurance providers, and a 40% tax o n â€Å"Cadillac† insurance policies. There are also taxes on pharmaceuticals, high-cost diagnostic equipment, and a federal sales tax on indoor tanning services. Total new tax revenue from the Act will amount to $409.2 billion over the next 10 years. $78 billion will be realized before the end of fiscal 2014(â€Å"Patient Protection and Affordable Care Act,† 2011). I have two problems with what many Americans now refer to as â€Å"Obama Care†, one I am no fan of paying higher taxes. Any economist will tell you that raising taxes does not stimulate economic growth and without economic growth people will continue to spend less, businesses will not hire new employees or expand, and the unemployment rate will continue to rise. Also an increased unemployment rate means more people in need of government assistance, along with more Americans unable to afford health care. So in short our government is going to raise taxes to give all Americans health care which will in effect cause more Americans to become unemplo yed and lose there health care and become subject to a penalty. Sounds like the democratic version of utopia is nothing more than a double edge sword doomed for failure. The concept of utopia is an unrealistic dream; for each person’s vision of utopia is different. The other problem I have with Obama’s centralized health care plan is that we are letting government dictate what we as American have to purchase or be subject to a fine if we do not comply. Our constitution states each person has the right to pursue happiness, it does not say the government should or could guarantee it, just that you have to right to pursue it. Some people suggest making healthcare mandatory is the same as having to purchase automobile insurance, the only problem with this type of thinking is that you do not have to drive or own a car. If you choose not to, no one fines you for it. I view health care as a right in respect that I have the right to purchase health care or to choose not too. I believe all Americans have the right to choice and should not be fined or penalized if they choose to exercise that right. Too many people today view our government as a separate entity and believe that it owes them something. We as Americans are in fact the government, for we are a government of the people for the people. References Health care in the United States. (2011). In . Retrieved October 24, 2011, from http://en.wikipedia.org/w/index.php?title=Health_care_in_the_United_States&oldid=456210485 Patient Protection and Affordable Care Act. (2011). In . Retrieved October 24, 2011, from http://en.wikipedia.org/w/index.php?title=Patient_Protection_and_Affordable_Care_Act&oldid=456759152

Lab 3 Determinates of Water Hardness

Determination of Water Hardness Using a Titrator Heather Crall Chemistry 1 SMT- 271044 10/17/2012 Abstract From seeing all of my results and conclusion I now see that I didn’t understand this lab very well and that its not easy when others try to help. Since I have hard water it tells me that my water flows over and through rocks and minerals, like limestone. Purpose The purpose of this lab is to become familiar with the concept of water hardness. We learn that hard water contains high levels of dissolved minerals that are in the form of metallic ions.Most of Ohio which is the state I live in either has moderately hard water or hard water. For as my town the city is moderate and the country is hard. Procedure 1) Put safety things on 2) Place the stopcock in the closed position on the end of the titrator and fill with 10 mL of EDTA solution. 3) Put a crumpled up paper towel under the titrator and allow a few drops of the solution to fall into the towel. This way it fills the ti p of the titrator then close and throw the towel away. Then place the 100 mL beaker under the setup. 4) Use the graduated cylinder to measure exactly 10 mL of tap water from your sink. ) Pour the tap water into the beaker then add 5 drops of pH 10 buffer solution. Swirl carefully the mixture in the beaker. 6) Read the volume of EDTA in the titrator and record the initial volume. Then slowly open the stopcock and add 1 drop at a time while swirling the mixture.7) Once the solution turns a pale blue-gray color turn the stopcock off then record the final volume in the titrator. 8) Repeat steps 4-7 and fill in Table 1. 9) Pour the rest of the contents down the drain Data Data Table 1: EDTA titration volume| | Initial EDTA Volume (mL)| Final EDTA Volume (mL)| Total Volume of EDTA Used (mL)| Trial 1| 9 mL| 7. mL| 1. 6 mL| Trial 2| 8 mL| 6. 6 mL| 1. 4 mL| Trial 3| 7mL| 5. 2 mL| 1. 8 mL| Average Volume of EDTA Used (mL): 1. 6 mL | Data Table 2: Water Hardness| Average Volume of EDTA Used (m L)| Concentration Ca^2+ ions per Liter of Water (mol/L)| Water Hardness (ppm CaCO3)| 1. 6 mL| 0. 015 mol/L| 1,500. 9 ppm CaCO3| Results A) Based on the analysis of your local water, would you classify its hardness as soft, moderate, hard, or very hard? Explain your answer. My water is moderately hard even though it’s the city we still have plumbing problems due to our soil and the minerals in our town.The country all has hard water so the deal with rust and bigger clogs than the city. B) Approximately how much calcium would you ingest by drinking eight 8-oz glasses of your local water? HINT: 1 oz(fluid ounces) =29. 57 mL 8oz= 236. 56 236. 56*8= 1,892. 48 mL Conclusion In conclusion it seems as though my results have come to show that I have very hard water when looking at the last graph but to have it say 1,500 tells me that my results is potentially incorrect. From what I understand it shows that the calcium carbonate is very high in my town.

The Fight For Equal Marriage - 1292 Words

The fight for equal marriage rights has been one of great length. Although this topic only brought to attention of the Supreme Court in 2015, gay marriage has long been a topic of interest in American society. Prior to 2015, gay marriage was only acknowledged and legal in select states, not nationwide. This caused great distress and heartache. One case in particular, the case that was brought to the supreme court, is very representative of such dejection. The subjects of such case are James Obergefell and John Arthur of Ohio. In 2013, the two were legally married in Maryland. Shortly after, however, Mr. Arthur grew terminally ill, and eventually passed away. Due to Ohio state laws, the state refused to put â€Å"married† on Mr. Arthur’s death†¦show more content†¦Hodges 40-41). Based off of these cases, there has clearly been great perplexion as to how homosexuality should be viewed and treated. Which leads to the controversy of gay marriage, and Obergefell v. Hodges. Obergefell v. Hodges was the Supreme Court case of 2015, which ultimately granted equal marriage rights to same-sex couples. Obergefell was arguing in favor of equal marriage rights, while Hodges had an opposing argument. This case was brought to the Supreme Court after the state of Ohio refused to put a married status on the death certificate of James Obergefell’s late husband in 2013. Theodore Wymyslo, James Obergefell’s defendant in the original Ohio case, appealed the ruling against Obergefell, which led to the case being pushed to higher courts throughout 2014, eventually reaching the Supreme Court in 2015 (LGBT Rights on the Docket). In the Obergefell v. Hodges case, Obergefell’s side discussed topics such as the expansion of marriage and gay rights, the due process clause of the Fourteenth Amendment, and the undeniable rights associated with marriage in their argument. Hodges’ side, however, had much weaker arguments, such as same-sex marriages will ruin the reputation of marriage, and religious views are conflicting of the premise of same-sex marriage. Taking a more extensive look into both sides of this case proves to be very interesting and thought provoking. Oberefell’s first argument was that marriage hasShow MoreRelatedThe Fight For Equal Rights For Same Sex Marriages Across The United States1393 Words   |  6 PagesThe Fight for Equal Rights for Same-Sex Marriages across the United States Having one loving parent is good. Having two loving parents is great. Having a mother and a father is traditional. Having two mothers or two fathers is wrong. This is what we are told to believe but as we learn from our past and grow as a society, we start to look for positive change in which our values are challenged and the truth becomes clear. 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