Experiment 2 – Identification of Inorganic Solids Jesse Galina CHM 101 Lab Monday October 1‚ 2012 Unknown Solid – 2 Identifying my cation was rather easy because of the color of the powder when it was first given to me. It was pinkish/slight red when solid and when it was grounded up even further. This observation ruled out every cation except for some hydrated Co (II) salts. After being dissolved in water‚ the solution turned pink which agrees with the statement that the cation was Co
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Water Testing Lab Conclusion In this lab‚ chemical tests were used to check for the presence of calcium‚ chloride‚ and sulfate ions in water samples. To do this‚ the testers started with five samples: a reference‚ a sample of only the chemical being tested for‚ a control‚ distilled water‚ two home water samples‚ and a school water sample. To test for the ions in the water‚ a chemical that would react with the ion and create a precipitate was added. If the precipitate was not easily visible‚ a
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solution. Mix. Record color change. B. Calcium oxalate equilibrium Put 5 mL of .1 M calcium chloride and 5 mL of .1 M sodium oxalate into 6 inch test tube. Mix by stoppering and inverting. Equilibrium is established by formation of white precipitate. Add concentrated HCl. Shake after each drop. Record any changes. C. Cobalt chloride equilibrium Heat 2 mL of saturated aqueous solution of cobalt chloride to boiling in a 6 inch test tube. Record the color before heating. Now place tube in ice water
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INDEX CONTENTS NO. 01 02 03 04 05 06 07 08 09 10 11 12 13 RESEARCH METHODOLOGY INTRODUCTION TO THE SALT INDUSTRY EDIBLE IODISED SALT PEST ANALYSIS OF INDUSTRY FIVE FORCES ANALYSIS OF INDUSTRY COMPETITIVE ANALYSIS PROMOTIONAL CAMPAIGN IN EDIBLE SALT INDUSTRY NIRMA INDUSTRIES LIMITED SWOT ANALYSIS OF NIRMA SHUDH SALT DATTA ANALYSIS HYPOTHESIS FINDINGS SUGGESTIONS & RECOMMONDATIONS BIBLIOGRAPHY APPENDIX LIST OF THE GRAPHS PAGE NO. 03 08 15 19 22 25 29 31 41 43 67 73 77 X Y A LIST OF THE GRAPHS
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Experiment 5: Shifting Equilibrium A solution is in equilibrium when the rate of forward reaction and the rate of reverse reaction are equal. This equilibrium may be disturbed when the concentration of the reactants‚ the concentration of the products or the temperature is changed. If the process involves gases‚ a change in pressure can also affect the position of equilibrium. The concept behind this is Le Chatelier ’s Principle which states that when a system is disturbed through application
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part 1 ‚ we observed the shift in equilibria of two aqueous solutions of Copper and Ammonia then Nickel and Ammonia. In part 2‚ we focused on cobalt ions in the presence of chloride ions as well as the precipitation of silver nitrate and sodium carbonate. In the last part of the experiment we utilized a solution of Cobalt chloride and compared the color at room temperature and then again in a container of boiling water. Physical Data: No physical Data was applicable to the experiment. Chemical Equations:
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Analysis of drilling fluids is essential to their performance. In this laboratory exercise the aim is to test three drilling fluid samples for; density and rheological properties‚ Fluid loss‚ chemical analysis i.e. testing pH‚ alkalinity‚ testing for chloride ions‚ calcium carbonate‚ calcium‚ bentonite; also determining the amount of solids present in the samples as well as volumes of oil‚ water and solids contained in the sample‚ and to test for contaminates such as NaCl and KCl. These tests helps us
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of the chloride ion on its rate of diffusion in agar means it will diffuse faster because it is more concentrated. We graphed the diffusion of chloride ions rather than sodium ions because while the sodium ions do diffuse in to the agar the chloride ions from the NaCl will combine with silver ions‚ from AgNO3 and create a white precipitate. The white precipitate allows us to measure the the white band through the agar at different points and determine the rate of diffusion of the chloride ions.
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Name: __________________________________ Teacher: ________________________________ DO NOT OPEN THE EXAMINATION PAPER UNTIL YOU ARE TOLD BY THE SUPERVISOR TO BEGIN Chemistry 2202 FINAL EXAMINATION June 2010 Value: 100% General Instructions This examination consists of two parts. Both parts are contained in this booklet and further general instructions are provided on appropriate pages. Part I – Multiple Choice (40%) Select the letter of the correct response from those provided. EITHER
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Introduction The purpose of this lab was to explore the properties of an unknown compound. An unknown was given and a cation flame test and anion test was performed to determine the identity of the compound. Once the identity was determined‚ the properties were explored. Experimental To determine the cation of the compound‚ a cation flame test was performed. A bunsen burner was lit until a medium blue flame was burning. The given unknown was scooped onto a nichrome wire loop. The wire was held
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