EXPERIMENT NO. 6 DETERMINATION OF THE MOLAR VOLUME OF A GAS AND THE UNIVERSAL GAS CONSTANT Salve‚ Ryan Angelo TAB3‚ Group 6‚ Mr. John Kevin Paulo Biadomang Tabor‚ Frances Hermilyn March 8‚ 2013 ------------------------------------------------- I. Abstract This experiment is working with the ideal gas law‚ which is the summation of Boyle’s Law‚ where pressure is inversely proportional to volume‚ Charles’ Law‚ where the volume is directly proportional to temperature and Avogadro’s Law‚ where
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Synthesis of Salicylic Acid and Potentiometric Determination of its Purity and Dissociation Constant ------------------------------------------------- Abstract The purpose of the study is to synthesize salicylic acid from the ester‚ methyl salicylate‚ and determine the acid’s dissociation constant and purity. The ester was converted to salicylic acid by base hydrolysis. The products were refluxed and recrystallized‚ to ensure maximum purity‚ and filtered‚ dried‚ and weighed. The melting point
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EXPERIMENT 2 ACID DISSOCIATION CONSTANT OF AN INDICATOR DYE OBJECTIVES Using spectrophotometric method: determine the wavelengths at which the acid and base forms of the dye in aqueous medium exhibit maximum absorption; determine the molar absorptivities of the acid and base forms of the dye and estimate an unknown concentration of the dye in solution using the Beer-Lambert’s Law; and determine the acid dissociation constant of the indicator dye. THEORY The absorption or reflection of
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spectrophotometric analysis of copper sulphate Introduction: In the modern usage. The term spectroscopy includes a large group of techniques which differ widely in their mode of application and information they reveal. As a useful working definition‚ spectroscopy is a study of interaction of electromagnetic radiation with matter in the experiment it means it’s the usage of ultra-light to measure the absorbance of the copper sulpate. The regions of the electromagnetic spectrum immediately adjacent
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ESTIMATION OF IRON IN IRON ORE-SPECTROPHOTOMETRIC METHOD By: Taylor Villari Experiment conducted on 7/22/13 Components of each test tube examined in the spectrophotometer Trial | Volume of Iron solution (mL) | Micrograms of Iron | Volume of 10% sodium acetate | Volume of 0.1% o-phenanthroline | Volume of water (mL) | 1(blank) | 0.0 | 0.0 | 1.0 mL | 1.0 mL | 8.0 mL | 2 | 1.0 mL | 10 | 1.0 mL | 1.0 mL | 7.0 mL | 3 | 3.0 mL | 30 | 1.0 mL | 1.0 mL | 5.0 mL | 4 | 5.0 mL | 50 | 1.0 mL
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use of spectrophotometer. The preparation of four known concentration of KMnO4 was done namely‚ 2.00×10-4M‚ 1.50×10-4M‚ 1.00×10-4M‚ 5.00×10-5M‚ respectively and is to be place on the spectrophotometer with the unknown and distilled water for the determination of each concentration’s absorbance. As the concentration is proportional with the absorbance of the solution‚ to determine the concentration of the solution is possible by drawing a graph of concentration against the absorbance. At the end of the
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The spring constant Manuel Cereijido Fernández – UO237242 PL-4 -----------------------------------------------------------------------------------1. Objectives The main objective of this experiment was to determine the spring constant using the dynamic method. 2. Theoretical fundamentals On the one hand‚ when a spring oscillates‚ the movement which describes can be classify as a simple harmonic motion. Therefore‚ its position‚ velocity and acceleration equations respect the time will
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Experiment 3: Chemical Equilibrium Purpose The purpose of this experiment was to determine the equilibrium constant for the formation of FeSCN2+. Introduction Chemical equilibrium is the point in a reversible reaction where the concentration of the reactants and that of the products remains constant. This point of equilibrium is referred to as the Kc value‚ which can be obtained using the formula: Kc = [product] [reactant] In this experiment‚ we used a spectrophometer to
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Chemical Equilibrium: Le Chatelier Principle By Sarah Ramos and Kristina Todorovic Chemistry 203 DEN Dr. Mohamed El-Maazawi Part A. Acid-Base Indicators Purpose In this part of the experiment‚ we will find a reagent that will shift the acid-base equilibrium reaction described by Equation (2) in one direction and then a second reagent that will cause the equilibrium position to shift back in the opposite direction. Introduction An acid–base indicator
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Determination of Formation Constant‚ Kf of Thiocyanoiron(III)‚ FeSCN+2 Dr. Fred Omega Garces Chemistry 201 Miramar College Chemical Equilibrium: Finding the Formation Constant of FeSCN2+ (aq) Fe3 +(aq) iron(III) + SCN–(aq) FeSCN2+(aq) D thiocyanate thiocyanoiron(III) kf = € FeSCN2 + [ ] Fe +3 [SCN− ] [ ] Objective The purpose of this experiment is to determine the constant formation‚ Kf‚ (equilibrium constant) for the formation of thiocyanoiron(III)
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