disassociation of Sodium Chloride: NaCl(aq)Na+ (aq)+ Cl-(aq) c. Aqueous Formic Acid—HCOOH‚ formic acid‚ is a weak electrolyte. This is due to its covalent bonds‚ but when added to water the acid releases some of ions that allow for little conductivity. The chemical reaction of the disassociation of Formic Acid: HCOOH(aq) H+(aq) + COOH-(aq) d. Glacial Formic Acid—Despite being a liquid‚ glacial formic acid is a covalent compound in pure form; it cannot ionize and become an electrolyte until
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Mixing of two solutions. 55 Class IX EXPERIMENT No: 9 AIM: To study the external features of root‚ stem‚ leaf and flower of monocot and dicot plants. Material Required : Plants of Hibiscus/Peturnia/rose/pea and grass/maize/bamboo/lily or‚ any other ornamental herb with flower and fruits‚ simple or dissecting microscope‚ hand lens‚ slide‚ coverslip and razor /blade. Procedure : 1. 2. 3. Observe the differences in the external features of stem‚ leaf‚ root‚ flowers and seeds. To study the leaf‚ see
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digestion of carbohydrates‚ proteins‚ and lipids (Digestion BioKit). Although test tube three contained this solution‚ we predicted that there wouldn’t be a reaction due to the fact that it was being boiled. The number‚ type‚ and arrangement of the amino acids determine the shape of the protein which directly controls the protein’s function. The shape and function of a protein can be altered by a process known as denaturing. Too high a temperature or change of pH can cause the denaturing to take place. If
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Corrosion during acidization job - Acid corrosion (causes and mechanism) Remedial steps to reduce corrosion - Use of Arcasolve™ in Acidizing Processes - Use of corrosion inhibitors References INTRODUCTION Acid treatments have been applied to wells in oil and gas bearing rock formations for many years. Acidizing is probably the most widely used work-over and stimulation practice in the oil industry. By dissolving acid soluble components within underground rock
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completed. In this experiment‚ solutions will be prepared‚ reacted‚ and then “disrupted” by adding compounds to the mix. Procedure: Part 1: Obtain 5 ml of saturated NaCl solution in each of two test tubes. Add 10 drops of concentrated 11.7 M hydrochloric acid to one test tube. Same for the other test tube using 1 M instead. Observe for 2 minutes. Part 2: Mix 2 ml of .01 M FeCl3 and 2 ml of .1 M KSCN solutions in a test tube. Dilute this by pouring it into a beaker and adding 100 ml of deionized
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Coffee spoons 1 Rubber bands 2 Beaker‚ 50 mL‚ plastic 1 Magnifier‚ dual 1 Pencil‚ marking 1 Thermometer-in-cardboard-tube 1 Well-Plate-24 In the Experiment Bag: LeChatelier’s Principle 1 E.D.T.A.‚ .15 M (Na2EDTA) - 2 mL in‚ Pipet 1 Hydrochloric Acid‚ 6 M - 2 mL in Pipet 1 Magnesium Chloride‚ 2 M - 3 mL in Pipet 1 Phenolphthalein Solution‚ 1% - 0.5 mL in Pipet 2 Pipet‚ Empty Short Stem 1 Sodium Bisulfate Crystals - 0.5 g in Vial 1 Sodium Bisulfate‚ 0.1 M - 4 mL in Pipet 1 Sodium Hydroxide
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INTRODUCTION For this experiment we studied an oxidation-reduction reaction of magnesium and hydrochloric acid solution. We compared the experimental measured amount of a product and the amount predicted by the theoretical calculation of a balanced equation: Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) PROCEDURE First we obtained a strip of pre-cut magnesium ribbon‚ cleaned it with steel wool to remove any signs of oxidation from the strip (which would alter our results)‚ and then weighed it (individual
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Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature from the final temperature
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CHEM 1411 – General Chemistry I Practice Problems‚ Chapters 1–3 Chapter 1 – Chemistry: The Study of Change 1. Element‚ compound‚ homogeneous mixture (solution)‚ or heterogeneous mixture: a) orange juice b) brass c) 0.9% saline (NaCl) solution d) garden soil e) room air f) methane gas g) sodium metal h) N2 gas i) Cu(NO3)2 crystals (freshly-squeezed) 2. Define (some of these terms are found in Chapters 2 and 3): a) c) e) g) i) k) m) o) 3. b) d) f) h) j) l) n) compound physical change
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test tube. b. Add 8 drops of hydrochloric acid to the anion solution. Note the appearance of the solution plus any evolution of gas and odors of gas. 5. Second test tube: a. Put 8 drops of the anion solution in a second test tube. b. Add 3 drops of silver nitrate solution. c. Note the colors of any precipitates formed. d. Write a net ionic equation for any reaction that produces a precipitate. e. Acidify the test tube by adding a few drops of nitric acid. f. Mix well and note if the
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