SPECTROPHOTOMETRIC DETERMINATION OF THE EQUILIBRIUM CONSTANT OF A REACTION M. L. SANGA CHEMICAL ENGINEERING‚ COLLEGE OF ENGINEERING UNIVERSITY OF THE PHILIPPINES‚ DILIMAN‚ QUEZON CITY‚ PHILIPPINES DATE PERFORMED: JANUARY 15‚ 2014 INSTRUCTOR’S NAME: MOISES JEROME GARRERO ______________________________________________________________________________________________________________________________ ABSTRACT The experiment aimed to determine the equilibrium constant Keq of the formation of Fe(SCN)2+
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Determination of pKa James McDuffie ABSTRACT: In this lab‚ the pKa of unknown solution #4 was measured Introduction: This lab focused on the equilibrium constant‚ Ka. Ka is associated with chemical properties of acids. The equivalence point will be reached once the moles of OH- equal the moles of HA and once this point is reached‚ the PH changes very quickly. With the results‚ a titration curve should be produced. Experimental Section Materials and Methods: A buret with NaOH solution
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| [Solubility Product Constant] | Experiment 11 | | Molly McCabe | 4/18/2013 | | Data Tables: Part 1 and Part 2 Experimental Data: Standard | Calculated volume of copper sulfate in standards | Absorbance values | Blank | 0.0 mL | 0.0 | 1 | 1.25 mL | 0.094 | 2 | 3.75 mL | 0.065 | 3 | 2.50 mL | 0.099 | 4 | 3.50 mL | 0.129 | 5 | 5.00 mL | 0.187 | Collected Data | Test tube 1 | Test tube 2 | Test tube 3 | Test tube 4 | Test Tube 5 | Initial volume (mL) | 0.05
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Mateo Castro April 3‚ 2013 Lab Partner: Unur Abdul Kader T.A: Katie Experiment 22: Molar Solubility‚ Common-Ion Effect Abstract The purpose of this experiment was to determine the molar solubility‚ the solubility constant‚ and the effect of a common ion on the molar solubility of calcium hydroxide. To accomplish this the experiment was split into two parts; part A and Part B. in Part A of the experiment a standardized 0.05 M solution of HCl was titrated into a 25 mL solution of saturated
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feature of a system at equilibrium is its ability to return to equilibrium after a change in conditions moves it away from the state. this drive to reattain equilibrium is state in Le Chatelier’s principle: when a chemical system at equilibrium is disturbed‚ it reattain equilibrium by undergoing a net reaction that reduce the effect of the disturbance. Two phrases in this statement need further explanation. First‚ what does it means to ‘disturb’ a system? At equilibrium‚ Q equals K. When a change
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Destiny Stuart Partner’s Name: Shanygne Swann Lab Report #2 Title of Experiment: Static Friction and Limiting Equilibrium Brief Theory of Experiment: In limiting equilibrium‚ the sum of the forces on block X and on the hanging masses (load) Y is zero. The load is increased to a value until block X just slides at constant speed when the table is tapped. Tapping the table destroys the limiting equilibrium condition momentarily by altering the balance between tension (T) in the string and
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Notes 12.1 The N2O4-NO2 Equilibrium System When you put a sample of N2O4‚ a colorless gas‚ in a closed container at 100C a reddish-brown color starts to show. This is due to NO2 formed by the decomp. of part of the original substance. The forward and reverse reactions are taking place at the same rate. The concentrations of species present remain constant with time. These concentrations are independent of the direction from which equilibrium is approached. The equilibrium constant K is where the
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concerning equilibrium is not true? A) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. B) Equilibrium in molecular systems is dynamic‚ with two opposing processes balancing one another. C) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. D) A system moves spontaneously toward a state of equilibrium. E) The equilibrium constant
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Position of Equilibrium * There are many equilibrium mixtures possible for a given chemical reaction‚ depending on the concentrations of solutions‚ the pressure of gases and the temperature of the reaction. * The term position of equilibrium can be used to describe a particular set of equilibrium concentrations for a reaction. * If either the temperature‚ pressure or concentration of one of the substances changes‚ then the concentrations of all the substances will change until a new
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Chp. 15 Chemical equilibrium: Occurs when a reaction and its reverse reaction (opposing reactions) proceed at the same rate At equilibrium the rate at which products are produced from reactants equals the rate at which reactants are produced from products At equilibrium a particular ratio of concentration terms equals a constant The composition of an equilibrium mixture does not change with time Kc: equilibrium constant 15.2 Law of mass action: expresses the relationship between
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