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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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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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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The primary focus of experiment 4 was to teach a student the basic solubility rules of salts in aqueous solutions. After developing and using a scheme for the qualitative analysis of three cations in an aqueous mixture‚ a student would use a centrifuge to identify‚ precipitate‚ and separate the three ions in the mixture. After becoming familiar with all three cations‚ the student would use the scheme again to identify at least two of the cations in an unknown solution. In order to begin the separation
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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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Identifying a Salt by Creating its Heating Curve Introduction: Solubility is a substance’s ability to be dissolved in a liquid‚ usually water‚ and some substances are more soluble than others. A solution can be saturated‚ unsaturated or supersaturated. Temperature plays a large role in the solubility of substances. For example‚ on table G of the Chemistry reference tables it shows that 10g of KClO3 will dissolve in 100g of water at about 25°C‚ but at about 48°C‚ 20g will dissolve. The higher the
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