the factors which affect its lytic activity. The assay method reported by Smolelis and Hartsell (1949) has been found to be accurate and highly adaptable to the study of this enzyme. This report concenms its application to the effect of pH‚ salts‚ ions‚ temperature‚ and manner of preparation of the cell suspension‚ on the activity of lysozyme. MATERIALS AND METHODS Preparation of the cell suspension. To expedite the testing of lytic activity by lysozyme ’and to reduce the possibility of daily
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CHEMISTRY 1184 Laboratory Manual for GENERAL CHEMISTRY I Jim Carroll Roger Hoburg Dana Richter-Egger August 2006 University of Nebraska at Omaha i Table of Contents Table of Contents ......................................................................................................................................... i Chem1184 SYLLABUS............................................................................................................................... ii Preliminary
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present. To access the degree of the alkyl halide formed (1° or 2° halide) and to determine whether Markovnikov’s addition occurred‚ two qualitative tests can be used: (a) reaction with alcoholic silver nitrate solution and (b) reaction with sodium iodide in acetone. For the silver nitrate test‚ one drop of alkyl halide is added to 2 mL of 0.1 M solution of silver nitrate in
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The Causes and Effects of Radiation A Research Paper Presented to Mr. Ronel Ramos Alcasarin St. Catherine Academy In Partial Fulfillment Of the Requirements for ENGLISH IV By: Hazel Dianne S. Cagalawan March 2013 The Research Paper attaches hereto‚ entitled The Cause and Effects of Radiation Prepared and Submitted by: Hazel Dianne S. Cagalawan In Partial fulfillment Of the Requirements in ENGLISH IV is hereby accepted: Mr. Ronel Ramos Alcasarin
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rule‚ reactivity increases as you move down a group in the periodic table. This means in regards to solubility that the more you farther you move down the group the more insoluble the element is when combined with hydroxides‚ chlorides‚ bromides‚ iodides‚ sulfates‚ carbonates‚ and oxalates. My results were consistent with this theory in that the mixtures went from no reaction to forming a precipitate or from forming a light precipitate to a heavy one as the elements moved down the periodic
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Chemical equilibrium is said to be dynamic because‚ at equilibrium‚ there are reactions continually occurring. The rate of the forward reaction equals the rate of the reverse reaction. Equilibrium Constants At equilibrium as much hydrogen iodide is being decomposed as is formed and so the concentrations of all three substances remains constant. Kc is the equilibrium constant in terms of molar concentration. This is known as the Equilibrium Law. The equilibrium constant shows the position
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in water‚ the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions‚ write balanced equations‚ and to write net ionic equations for precipitation reactions. A detailed view of the results can be found in the table below. Cations used: Barium‚ Copper‚ Iron‚ Sodium‚ Cobalt‚ Nickel Anions used: Nitrate‚ Carbonate‚ Chloride‚ Hydroxide‚ Sulfate‚ Bicarbonate‚ Iodide‚ Phosphate
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light (put in a dark place) will not decompose. Theory: Equipment: * 4 x petri dishes * 1 x glass stirring rod * 0.1 mol/L silver nitrate in a dropper bottle * 0.1 mol/L Sodium chloride in a dropper bottle * 0.1 mol/L Sodium iodide in a dropper bottle Method: 1. Ensure you are wearing safety glasses 2. Take the petri dishes and label then 1‚ 2‚ 3‚ and 4. 3. Add 20 drops of silver nitrate solution to each petri dish. 4. Add 20 drops of sodium chloride to petri
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which of the two will reacted with potassium iodide inside the breaker‚ as the latter passed from the beaker into the tube‚ the glucose/starch solution’s change of color showed that the potassium iodide was small enough that it able to pass through from the solution and into the bag. After the Benedict test‚ glucose from the bag was also founded small enough that it can exit from the bag and into and solution. In the end‚ glucose and potassium iodide was the only two that is capable to move freely
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CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION MULTIPLE CHOICE QUESTIONS 4.1 Which of the following compounds is a strong electrolyte? E A. H2O B. O2 C. H2SO4 D. C6H12O6 (glucose) E. CH3COOH (acetic acid) Answer: C 4.2 Which of the following compounds is a strong electrolyte? E A. H2O B. N2 C. KOH D. C2H6O (ethanol) E. CH3COOH (acetic acid) Answer: C 4.3 Which of the following compounds is a weak electrolyte? E A. HCl B. CH3COOH (acetic acid)
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