there was no need for distillation. Next‚ a solubility test was given. When one drop of the unknown liquid was added to about 2 mL of water‚ the sample was tested to be soluble due to the dissolubility between the two compounds. By following the chart that was given on the sheet‚ the pH of the solution was tested. Since the two litmus did not changed color‚ the sample was identify to have a low molecular weight and a neutral substance. Based on the solubility test‚ some possible
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Solubility and Stoichiometry I. Introduction The first purpose of this experiment is to apply solubility rules to choose two of eight given reactants to do a precipitation reaction. The second purpose is to use stoichiometry to calculate how much of a reactant will be used in a precipitation reaction‚ assuming that the amount of product is given‚ and to figure out the actual yield vs. the theoretical yield and to calculate the percent yield. The other purpose of this experiment is to practice the
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Preliminary Test and Solubility Classification of Organic Compound Keene Louise Topacio‚ Christopher Jay Robidillo Abstract The experiment focuses on how to classify organic compounds by its functional groups. It is done by preliminary test and with the solubility test. Preliminary test used two known compounds also the unknowns. Physical state‚ color‚ odor‚ and ignition test were noted. The known compounds are inorganic and organic compounds. A comparison is made from the observation in the unknown
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INVESTIGATE FACTORS INFLUENCING THE SOLUBILITY OF SALTS Research question How does temperature affect the dissolving time of various salts.? Hypothesis I predict that with water of high temperature the salts will dissolve quicker. Controlled Variable Amount of water (solvent) Amount of salt used (solute) Type of cups taken and their sizes Independent variable Temperature of water Dependent variable Time taken for each salt to dissolve Material Required Measuring
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1. In the first group of four reactions‚ Iron phosphate and calcium phosphate are the two products that are insoluble in water. In the three of the four reactions a cloudy white or yellow formed. This indicated the formation of a precipitate‚ caused by the generally insoluble phosphate anion. Potassium chloride‚ Iron nitrate‚ and potassium sulfate where the products which were soluble in water. With these products there was no evidence of a precipitate forming. 2. Based on the results from reactions
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Solubility Product Constant Q: Write the equilibrium equation for a saturated solution of the following salts and the corresponding solubility product expressions. a) BaSO4 (s) b) MgF2 (s) c) Ag2S (s) d) Cu(IO3)2 (s) [ ][ [ [ A: [ ( Q: ) ] ][ ][ ] ] What is the equilibrium concentration of Cd2+ ions in a saturated solution made by shaking CdS(s) with water? Ksp = 6.0x10-27 for CdS. [ A: [ Q: ][ ] ][ ] ; ][ ] √ √ A solution in equilibrium with a precipitate of AgCl was found to contain
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J. Phys. Chem. B 2007‚ 111‚ 9001-9009 9001 Improving Carbon Dioxide Solubility in Ionic Liquids Mark J. Muldoon‚† Sudhir N. V. K. Aki‚‡ Jessica L. Anderson‚ JaNeille K. Dixon‚ and Joan F. Brennecke* Department of Chemical and Biomolecular Engineering‚ UniVersity of Notre Dame‚ Notre Dame‚ Indiana 46556 ReceiVed: March 8‚ 2007; In Final Form: May 4‚ 2007 Previously we showed that CO2 could be used to extract organic molecules from ionic liquids without contamination of the ionic liquid
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Purpose: Our purpose here to determine the affects of temperature on potassium nitrate’s solubility in water. Materials Used in the Experiment: Latex gloves Laboratory coat Safety goggles Thermometer Stir rod Test tubes Beaker Weighing dish Hot plate Potassium nitrate Distilled water Description of the Object of the Experiment Potassium Nitrate: The chemical compound potassium nitrate is a naturally occurring mineral source of nitrogen. It is a nitrate with chemical
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Experiment 10: Solubility Product for Calcium Hydroxide GOAL AND OVERVIEW A saturated solution of Ca(OH)2 will be made by reacting calcium metal with water‚ then filtering off the solids: Ca(s) + H2O → Ca(OH)2(s) Ca2+(aq) + 2OH-(aq) The concentration of dissolved hydroxide will be determined by acid-base titration with standardized HCl solution. The Ksp for Ca(OH)2 will be calculated from the experimentally determined saturation concentration of hydroxide. Objectives of the data analysis understand
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Study of Solubility Equilibrium of Potassium Hydrogen Tartrate Wang Haina 1. Aim 1. To determine the solubility of potassium hydrogen tartrate (KHT) at various temperatures from 10°C to 50 °C‚ and determine the corresponding Ksp at these temperatures. 2. To obtain the changes in enthalpy and entropy of the dissolution of KHT from the dependence of Ksp on temperature. 2. Results and discussion 2.1 Collection of data A portion of KHT (1 to 1.5 g) was added into about 100 mL of deionised
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