* 1 To measure the molar solubility of a sparingly soluble salt in water. * 2 To prepare a calibration curve based on complex ion formation for absorbance enhancement. * 3 To calculate the solubility product constant (Ksp) of a sparingly soluble salt from its molar solubility. * 4 To confirm the common ion effect on the molar solubility of a sparingly soluble salt. Introduction In previous introductory chemistry courses‚ you learned some basic solubility rules that are useful in
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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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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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1. Provide a general discussion of the solubility/miscibility behavior observed in procedure A-D. For part A of the procedure we worked with the solubility of solid compounds in various solvents. The three solid compounds that were worked with during this procedure were benzophenone‚ malonic acid‚ and biphenyl. These three solids were then mixed with water (highly polar)‚ methyl alcohol (intermediately polar)‚ and hexanes (nonpolar). When benzophenone is mixed with water the results turned out to
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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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Brooke Thomas September 13‚ 2012 Separating Salt and Sand Lab Report Separating components of a mixture of salt and sand and calculate the mass of each. Salt is soluble and sand will sink to the bottom‚ you can separate the rest with filtering and distillation (boiling). If salt and sand are a mixture‚ then we can separate them by physical processes. Materials Ring with ring stand Funnel Wire triangle Stirring rod Filtering paper Beakers (400mL and 250mL) Rinse bottle Evaporation
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Modeling Effective Dose: Salt Tasting lab Purpose The purpose of this lab is to see at what measurements (of salt) can the salt be detected by taste. Abstract The science of toxicology is based on the principle that there is a relationship between a toxic reaction (the response) and the amount of poison received (the dose). An important assumption in this relationship is that there is almost always a dose below which no response occurs or can be measured. A second assumption is that once a maximum
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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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Purpose/Objective The purpose of this experiment is to identify the periodic trends in the solubility of the alkaline earth metals and compare the results to that of lead Materials 1. Pencil 2. Lab notebook 3. 5 small test tubes 4. Droppers Chemicals 1. 0.2 M Mg(NO3)2 2. 0.2 M Ca(NO3)2 3. 0.2 M Sr(NO3)2 4. 0.2 M Ba(NO3)2 5. 0.2 M Pb(NO3)2 6. 1 M NaOH 7. 0.2 M NaBr 8. 0.2 M NaI 9. 0.2 M Na2SO4 10. 0.1 M Na2CO3 11. 0.2 M Na2C2O4 12. 1 M NaCl Data and Results Mg(NO3)2
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Abstract The chloride present in an unknown soluble sample was precipitated into silver chloride through precipitation gravimetry. The colloidal silver chloride originally formed was converted to a crystalline solid by controlling certain parameters of the experiment such as temperature‚ pH of the solution‚ and concentration of AgNO3. Once the solid was large enough‚ it could be washed‚ filtered‚ and weighed. The percentage of chloride present was found to be 24.73695223 (±0.00000006) %.
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