OUTLINING PROCESSES IMPLEMENTED ‐ SIX SIGMA PROJECTS S‐HTM‐TECH SUPPORT OF HCL TECHNOLOGIES HCL Outlining processes implemented through the following Six Sigma projects for IS‐HTM‐ Tech Support of HCL Technologies IS‐HTM‐Tech Support project: BEA‐WLS‐Support Six Sigma projects • • • Improving Org Learning Compliance Reducing Resolution time Streamlining Leave Management System An overview of BEA‐WLS‐Support BEA Systems‚ Inc. is a world leader in enterprise infrastructure software. Customers
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| Hydrochloric acid Sulphuric acid Stomach juice Lemons Vinegar Apples Oranges Grapes Sour milk White bread Fresh milk | 0.1 0.3 1-3 2.3 2.9 3.1 3.5 4 4.4 5.5 6.5 | Human saliva Distilled water Blood plasma Eggs Seawater Borax Milk of
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obtained 2. 10 drops of 0.3M lead nitrate solution was placed to TT 1 3. 10 drops of 0.5M silver nitrate solution was placed to TT 2 4. 10 drops of 0.5 mercurous nitrate solution was placed to TT 3 5. One drop of cold. 6N HCl solution was added to each TT. When precipitate forms‚ the HCl solution was continue to add in each TT drop by drop until no precipitate was form 6. The precipitate was settled down and the supernatant liquid was decant 7. The precipitate in the TT was added with 10 drops of distilled
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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Well #/Question: | Chemicals: | Reaction: | A-1/A | NaHCO3 andHCL - CO2 | Substance bubbled‚ releasing Carbon Dioxide | A-2/B | HCl andBromthymol Blue | Substance turned a yellowish-orange color |
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EXPERIMENT NO. 5 COMMON ION EFFECT Lopez‚ Pauline G. HIJ-2‚ Group No. 5‚ Ms. Jervee M. Punzalan Ramales‚ Ayane Mark Q. September 15‚ 2014 I. ABSTRACT The common ion effect involves how the solubility of a salt changes when some ion that is common to both added substance and the salt in question is introduced. The presence of a common ion hinders the ionization of a weak acid or a weak base hence this is known as the common ion effect. Simply put‚ the effect
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enthalpies for each step equals the enthalpy change for the overall reaction. For example‚ the three chemical equations used throughout the experiment were: Equation 1: NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) Equation 2: NH4Cl(aq) + NaOH(aq) NH3(aq) +NaCl(aq) + H2O(l) Equation 3: NH3(aq) + HCl(aq) NH4Cl(aq) Resulting in Equation 1 plus Equation 2(reversed) will equal Equation 3. In this case‚ Hess’s Law gave the ΔH for Equation 3. Calorimetry is the science of measuring heat‚ and is
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Medicine Dropper Calibration: 1 mL = 16 drops Table 1. Cobalt Complexes Solution Color Change # of drops mL CoCl2 in EtOH + H2O red-violet 5 0.31 + 12 M HCl blue 9 0.56 CoCl2 in H2O + 0.5 M NaCl light red 18 1.12 + 0.5 M HCl light red 20 1.25 + 1 M HCl light red 20 1.25 + 6 M HCl reddish pink 25 1.56 + 12 M HCl reddish pink 23 1.44 The equilibrium equation for this reaction is Co(H2O)62+ + 4 Cl- CoCl42- + 6 H2O [4] pink blue Addition of water
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temperature can affect Reaction Rate. Hypothesis: I predict that the higher the temperature‚ the higher the Reaction Rate will be. Therefore I predict that the Reaction rate of the 40˚ C heated Lime Stones and HCL acid will be higher than the 35˚ C heated Lime Stones and HCL acid. I predict this because I know that when the temperature is raised‚ particles move faster and collide more frequently. Therefore if temperature is raised‚ the Reaction rate will increase. The increase in temperature
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Abstract This laboratory involved utilizing equipment to dilute a sugar water solution. It also created solutions containing varying levels of concentrations and densities. Equations were used to figure the molecular weight of the sugar‚ and the number of moles of sugar in the volumetric flask. There was also an equation to figure the Molarity‚ as well. As a result of the experiment‚ I now have a better understanding of the density of a concentration‚ and what Molarity is . Observations Data
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