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Lab Report Titration

Lab Report Titration - Zach Lashaway Chemistry Lab 134...

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Zach Lashaway Chemistry Lab 134 Drawer #92 Tuesday 3-22-08 The Effect of Salts and Nonelectrolytes on the Solubility of Potassium Bitartrate Introduction When finding the solubility of an electrolyte it can be found using the equilibrium equation known as the solubility product constant. The solubility product constant is denoted as Ksp, the sp represents solubility product, and the K stands for constant. Solubility product constant expresses the extent to which the dissociation occurs. The difference between solubility and molar solubility; is that solubility is the quantity that dissolves to form a saturated solution, while the molar solubility is the number of moles of solute that dissolves to form one liter of solution. To calculate the solubility product constant (Ksp) is similar to calculating the other equilibrium- product expression, which is the solubility product, equals the products divided by the reactants each raised to the coefficient of each aqueous molecule. The solids are liquids are not included in the solubility product constant, because they do not dissociate (not aqueous). The following is an example of the dissolution of salt (AZ) and the Ksp equation. AZ(s) = A + (aq) + Z - (aq) => Ksp= [A + ][Z - ].
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The calculation of the solubility product constant (Ksp) will determine the magnitude of the solubility of the solid. When reactants are greater than products a lesser Ksp value is determined. A calculated low Ksp represents a solid with very little dissociation in solution. With products being greater than reactants, the Ksp value will be larger. Likewise a large calculated Ksp indicates the solid dissociates greatly in the solution.
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