less number of drops in order to change the color of the solution. This is because the more concentrated a substance is‚ less of the substance is needed to cause an equilibrium shift. 2) When you add 6.0M NaOH into the iron (III) thiocyanate ion equilibrium system‚ the concentration of Fe3+ ion decreases. This causes the equilibrium system to shift to the left (reactant) side. This is why the solution becomes lighter yellow. Fe(OH)3 is also formed during the experiment. 3) If the hydrated cobalt
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acid solution used was H2SO4 because it is highly acidic. 2CrO4-2(aq) + 2H3O+(aq) ⇄ 3H2O(L) + Cr2O7-2(aq) is the balance chemical equation of the system. When the acid solution is added the equilibrium shifts to the left making the solution orange and when basic solution is added to the solution the equilibrium shifts to the right making the solution yellow. Therefore‚ chromate is the stable as base and dichromate is stable as
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University of Exeter‚ Cornwall‚ UK. Bailey‚ R.‚ 1987. The characteristics of activated carbon adsorption. The South African IMM‚ vol. 1. Chamber of Mines of South Africa‚ Johannesburg. pp. 383–393. Barbosa‚ O.‚ Monhemius‚ A.J.‚ 1989. Thermochemistry of Thiocyanate Systems for Leaching Gold and Silver Ores. Royal School of Mines‚ London. Precious Metals Õ89. MMMS‚ 1988. pp. 307–339. Davidson‚ R.J.‚ 1974. The properties of activated carbon adsorption. J. South African IMM‚ 67. Eaton‚ G.M.‚ 1965. The Chemistry
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CHEMICAL EQUILIBRIUM Cristian C. Calizo Joshua Kevin K. Uy College of Engineering College of Engineering Date Performed: Jan. 7‚ 2014 Date Submitted: Jan 14‚ 2013 Methodology Iron (II) – Silver Ions System 1 ml each of 0.10 M FeSO4 and 0.10 M AgNO3 were mixed and shaked in a 4-inch test tube. The mixture was centrifuged‚ and the supernate was decantated into a test tube. Separate drops of the supernate was tested for presence of Fe2+‚ Ag+ and Fe
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Objectives Validate the Beer-Lambert law for KMnO4. To determine the pKa for an acid-base indicator To estimate the equilibrium constant for the formation of complex ion Fe(NSC)²ꭞ The function of part two of the experiment is to find the value of the constant K‚ in the following equilibrium constant: K=[Fe (NSC) ²⁺]/ [Feᶟ⁺] [NCS⁻]‚ while not disrupting the equilibrium. Theory For part one. The majority of chemical compounds are known to absorb UV or visible light. Depending on the
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Chloride in Urine in Different Circumstances Aim: To determine the chloride content by titrating mixtures of urine against potassium thiocyanate under in different circumstances. Research Question: How do different conditions of urine samples collected affect its concentration of chloride which is measured by titrating the mixture of urine with potassium thiocyanate until it turns red? Hypothesis: The greater the consumption of food‚ the higher the chloride concentration in urine. This can
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sublimates; principle of flame test‚ borax-bead test‚ cobalt nitrate test‚ fusion test‚ chromyl chloride test; analytical reactions for the detection of nitrate‚ nitrite‚ halides‚ phosphate‚ arsenate‚ arsenite‚ sulphide‚ thiosulphate‚ sulphate‚ thiocyanate‚ borate‚ boric acid‚ carbonate. Analytical reactions for the detection of Cr3+‚ Fe3+‚ Ni2+‚Cu2+‚ As3+‚ Mn2+‚ Importance of common-ion effect in the separation of Group II cations‚ and Group III cations. Unit II. Basic inorganic chemistry III
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Chemical Thermodynamics Chapter 19 Lecture Worksheet Homework: 19.29‚ 19.31‚ 19.37‚ 19.39‚ 19.41‚ 19.43‚ 19.47‚ 19.51‚ 19.53a‚ 19.55‚ 19.61‚ 19.73‚ 19.75‚ 19.77 Recall from Chapter 5 - 1st Law of Thermodynamics o Energy is neither ____________________________________________. o Energy of the universe is constant. o Enthalpy Change ▪ Heat energy transferred at _____________________________________ ▪ Negative
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of this lab is to identify the presence of cations and anions in four unknown solutions by identifying whether they are copper‚ silver‚ iron‚ or chloride ions which is done by adding sodium hydroxide‚ solid copper‚ silver nitrate‚ and potassium thiocyanate to the solutions and analyzing the chemical reactions. Introduction: Chemical change‚ unlike physical change is the change in the composition of a substance rather than simply its shape‚ size‚ or state (Marie‚ 2015). Signs that a chemical change
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Testing for Ions Analysis Chemical Changes of Test Solutions Test Solution Silver Nitrate Barium Chloride Potassium Thiocyanate Sodium Sulfate - Stayed white in color - Turned cloudy in color - Precipitation formed in solution - Stayed white in color Potassium Chloride - Turned cloudy in color - Precipitation formed in solution - Stayed white in color - Stayed white in color Iron (III) Nitrate - Stayed orange in color - Stayed orange in color - Changed color from orange
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