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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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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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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Long Lam Experiment 9: Rate Law Determination of the Crystal Violet Reaction Goals: Under stand 1st‚ 2nd ‚ and 3rd order chemical reactions‚ learn graphing options available on LogerPro Purpose: Determine the reaction order with respect to crystal violet for the reaction between crystal violet and sodium hydroxide. Introduction: The rate expression for this reaction is of the form: rate = K(CV+)M(OH-)N Where k = re constant‚ m is the order of the reaction with respect to the concentration of
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enzyme involves monitoring the change in absorbance of the reaction medium at 405 nm. Exergonic (i.e energy producing reactions) exhibit a negative free energy change. Sometimes these reactions occur spontaneously‚ but generally some energy must be supplied to initiate the reaction; in other word an energy barrier exists between the reactants and the products. The “energy barrier” represents the activation energy of a chemical reaction. In this practical the activation energy of hydrolysis
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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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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy Curtis M. Franklin Thursday‚ February 14‚ 2013 ABSTRACT An ice calorimetric measurement was used to determine that a reaction involving solid magnesium metal and 1.00M sulfuric acid produces an experimental a value of ∆H = -226 ± 28 kJ/mol at 0°C. This is about 48.4% lower than the expected value reported at 25°C. Introduction Many chemical reactions exhibit themselves by exchanging heat energy‚ either be absorbing
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