The Solubility Study

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Required Materials: Solids: KNO3 unknown concentration, KNO3 Liquids: Tap Water, DI Water Other: 1 burette, 1 1000 mL beaker, 5 test tubes, thermometer, heating pad Objectives: • To determine the effect of temperature of the solubility of a salt. • To construct a solubility curve for the salt. • To determine the mass of an unknown size sample of the salt. Theory: Solubility is a measure of t he amount of one substance that can be dissolved in a measured amount of another substance. In this experiment we are going to measure the solubility of KNO3 in water at various temperatures. Results can be reported in different ways ranging from grams or salt dissolving in a milliliter of water to grams of salt in 100 mL of H2O In general, systems tend to go to a state of disorder or to a state of greater entropy. During the dissolving process, the particles of the solid become randomly distributed through the solvent in sharp contrast to their orderly arrangement in the solid state. Ion the solid state there are strong forces holding these particles together. In order to dissolve the solid, energy must be expended to overcome these forces. When the solid has dissolved, there are attractive forces between the particles and the solvent particles. Energy is released when these forces take effect. The net energy change during dissolving is the sum of these two opposing forces. For most substances, the energy to break up the attractive forces in the solid state is greater than the energy released when the particles are solvated. In these cases, addition of energy (heating) should cause an increase in solubility. If energy of solvation is greater than the energy needed to break up the solid, then heating would decrease solubility. Procedure: Part 1 – Solubility of KNO3 1. Weigh out 5 samples of KNO3 approximately 3.0g, 4.0g, 6.0g, 8.0g and

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