SPECTROPHOTOMETRIC DETERMINATION OF THE EQUILIBRIUM CONSTANT OF A REACTION Methodology The following stock solutions were prepared: 1.0 M HCl‚ 0.1 M HCl‚ 0.1 M KSCN‚ 0.002 M KSCN (in 0.1 M HCl)‚ 0.2 M FeCl3 (in 0.1 M HCl)‚ and 0.002 M FeCl3(in 0.1 M HCl). Using the prepared stock solutions‚ the standard (Table 1) and Unknown (Table 2) solutions were prepared. Table 2. Preparation of Standard Solutions 0.10 M KSCN 0.002 M FeCl3 0.1 M HCl Blank 2.0 ml 0.0 ml 8 ml S1 2.0 ml 0.1 ml 7
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Spectrophotometric Determination of the Equilibrium Constant of a Reaction DEPARTMENT OF MATERIALS‚ METALLURGICAL AND MINING ENGINEERING‚ COLLEGE OF ENGINEERING July 26‚ 2012 ------------------------------------------------- ABSTRACT ------------------------------------------------- Before proceeding to test the next solution‚ we must first clean the cuvette‚ using similar steps earlier. First‚ we rinse with water‚ then with the solution‚ and then we fill it up and test
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Spectrophotometric determination of Ascorbic acid Concentration in an Unknown Solution Introduction: The naturally occurring organic compound with antioxidant properties is Ascorbic acid shortly referred as (AA). Normally the color of Ascorbic acid is white‚ but in some cases of impure samples it appears yellow in color. Ascorbic acid is solid in state. In water it dissolves well to give mildly acidic solutions. Ascorbic acid is one form ("vitamer") of vitamin C [1]. So‚ Ascorbic Acid (AA)
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Spectrophotometric Methods: The Determination of Iron The goal of this laboratory experiment was the quantitative spectrophotometric determination of Fe (II) by using a calibration plot‚ which obeyed the Beer-Lambert Law. In order to determine the Fe (II) concentration‚ a series of solutions of known concentrations were made. The solutions were analyzed by the Ocean Optics spectrophotometer in order to determine their absorbance. The concentration of the unknown Fe (II) was determined by the “eye-ball”
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Determination of Equilibrium Constants Introduction Bromothymol blue is an indicator for many acid-base titrations. When adding different solutions within the indicator it is to react and change colors‚ in this experiment the different colors were blue‚ green‚ and yellow. In the following experiment‚ obtaining the absorbance levels for each one makes it possible to calculate the equilibrium constant. Materials and Methods For this specific experiment there are a few materials that are crucial
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Determination of the Rate Constant for a Chemical Reaction Department of Chemistry Abstract This experiment was performed to determine the rate constant k‚ for hydrolysis of tertiary butyl chloride to tertiary butanol. The solvent system for this reaction is 45% isopropyl alcohol and 55% water. The rate of hydrolysis of t-butyl chloride is measured by the decrease in the concentration of this reagent with time. The rate of decomposition of t-butyl chloride must be equal to the rate of formation
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Ngoc Pham Chem162B Lab #2: Trends in Periodic Table Date: 01/10/2011 Lab partner: Ian Bauer Result Section: Table I: The solubility of the alkaline earth metal ions | SO42- | CO32- | C2O42- | IO32- | Mg2+ | S | I | S | S | Ca2+ | I | S | S | I | Sr2+ | S | S | S | I | Ba2+ | I | I | I | S | Key: I- insoluble‚ S-soluble Table II: Color of water (Halide) and Halogen (Hexane) layers | Cl2 | Br2 | I2 | Hexane layer | Clear | orange | Pink | Water layer | Clear‚
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Determination of an Equilibrium Constant Abstract: In this experiment‚ two reactions were run to determine the molar absorptivity and the equilibrium constant of FeSCN2+. The main principles used in this lab are equilibrium‚ LeChatlier’s Principle‚ Beer’s Law and Spectrocopy. The first reaction was run to completion using LeChatier’s Principle and the second reaction was run to equilibrium. A spectrophotometer was used to measure absorbances. Using a graph of absorbance versus concentration
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DETERMINING THE EQUIVALENT MASS AND DISSOCIATION CONSTANT OF AN UNKNOWN WEAK ACID BY TITRIMETRY INTRODUCTION Acids are substances that donate hydrogen ions and bases are substances that accept hydrogen ions. Acids and bases react with each other by transferring hydrogen ions. One way to distinguish an acid is by its equivalent mass‚ which is the number of grams of the acid needed to transfer one mole of hydrogen ion to a base. For a monoprotic acid‚ which only transfers one hydrogen ion‚ its
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CH 127 – Chem 2 Lab Determination of an Equilibrium constant Goals The purpose of this experiment is to determine the equilibrium constant for the reaction Fe3+(aq) + HSCN(aq) –>FeSCN2+(aq) + H+(aq). The equilibrium constant expression Kc for Reaction is kc=FeSCN2+[H+]Fe3++[HSCN] Procedure *Preparation of the Beer’s law plot Prepare five solutions of FeSCN2+(aq) of known concentrations between 1x10-5M and 1x10-4M by diluting various volumes of 4.62x10-4 HSCN. Calculate the Final concentration
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