Solubility and Functional Groups _______________________________________________________ You will recall from general chemistry that a solution has two components: the solvent‚ which is the substance present in greater amount‚ and the solute‚ which is dissolved in the solvent. Solubility is defined as the mass (in grams) of solute dissolved in 100 g of solute at saturation. Molar solubility is defined as the amount (in moles) of solute per liter of saturated solution. The solubility of one compound
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Effect of Temperature on Solubility Lab Purpose: What is the solubility of minerals in water? What is the relationship between temperature and solubility? Hypothesis: If salt and sugar are each tested in water of varying temperatures‚ then salt and sugar’s solubility will increase as the temperature also increases. Materials: Two 250 mL beakers Tap water 100 mL graduated cylinder Hot plate Two petri dishes Glass stirring rod Salt Sugar Thermometer
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Megan Ly Chemistry 231L February 20‚ 2013 SOLUBILITY Purpose: To better comprehend solubility behavior by investigating the solubility of various substances in different solvents‚ looking at miscible and immiscible pairs of liquids‚ and observing the solubility of organic acids and bases. Reference: Pavia
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The main purpose of this lab is to experiment the molecular polarity on the solubility of solutes in variates of solvents and helped us to determine the polarity of the unknown solute. In this lab‚ we observed the effects of adding polar liquid solutes to non-polar liquid solvents. Materials used: Safety goggles 3 graduated cylinders ethanol‚C2H5OH solid iodine‚ I2 glycerol‚ C3H5(OH)3 water 10 rubber stoppers 10 test tubes kerosene ammonium chloride
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Introduction: Solubility equilibrium refers to the dissolution of a compound in water. Specifically‚ the degree to which a compound is soluble (Tro‚ 739). This can be measured using the expression Ksp = [Mb+]a[Xa-]b‚ in which Ksp represents the solubility product constant (Thorne‚ 90). This constant is important because it does not change at a given temperature‚ regardless of the solution a compound is in; a smaller constant would indicate lower overall solubility. It is important to note that
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Lab 3: Solubility of Organic Compounds Objectives: Understanding the relative solubility of organic compounds in various solvents. Exploration of the effect of polar groups on a nonpolar hydrocarbon skeleton. Introduction: The solubility of a solute (a dissolved substance) in a solvent (the dissolving medium) is the most important chemical principle underlying three major techniques you will study in the organic chemistry laboratory: crystallization‚ extraction‚ and chromatography.
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rules to determine how soluble each chemical is and if it is at all. This is what we call solubility laws. These laws show what chemicals are soluble and which ones are insoluble. They also describe what chemicals can be dissolved and what chemicals cannot dissolve. These chemicals are them recorded on Solubility tables which list solubility and how soluble the chemicals are. According to Busch (2015) the Solubility Rules are as follows: 1. Salts containing Group I elements are soluble (Li+‚ Na+‚ K+
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. Yes‚ comparably to TLC plate 2 and 3. The benzophenone is more neutral but as the same time its nonpolar‚ being that Silica gel in TLC 2 was polar and the solvent ethyl acetate-hexane is non-polar it moved relatively with the solvent. The stationary phase in TLC 3‚ alumina is non polar and the solvent ethyl acetate is polar so from the ideal that polar does not attract non-polar benzophenone stick stronger to alumina non-polar rather than moving up with polar solvent ethyl acetate as it did in
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We reached our goals through our experimentation. We tested the solubility of each of the starting and ending materials in water‚ HCl‚ NaOH‚ toluene‚ and acetone. We discovered that the starting materials would only dissolve in toluene. To make the soap‚ we obtained about 10 mL of vegetable oil and 10 g of lard and we placed them both in separate 250 mL beakers. While we were stirring the compounds‚ we also added 15 mL of 6 M NaOH drop by drop and 1 mL of glycerol. We then heated our solutions
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Solubility Product Determination Purpose • To determine the solubility product constant‚ Ksp‚ of an ionic compound. Introduction The solubility product constant‚ Ksp‚ is a particular type of equilibrium constant. The equilibrium is formed when an ionic solid dissolves in water to form a saturated solution. The equilibrium exists between the aqueous ions and the undissolved solid. A saturated solution contains the maximum concentration of ions of the substance that can dissolve at
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