L07 Chem 151 Lecture 14: Experiment 5 Lecture
5 Mar 2017
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Equilibrium between an ionic solid and its dissociated cations/anions. Supersaturated solution: q > ksp -> more than theoretical dissolution. Causes supersaturated solution to go in reverse direction (shift left) If concentrated naoh is added to a saturated sodium acetate solution, the equilibrium will shift left, less solute will dissolve. The presence of ions common to the solid decreases the solubility of the solid. Solubility (s) maximum amount of solute that can be dissolved in 1l of solution (moles/liter or grams/liter) If ca2+ is only source of ca2+, then solubility = [ca2+]sat. Pipet from the bottom of the solution so the solid on the surface won"t be disturbed. Volume of hcl needed is greater for the naoh solvent. [oh-]tot increases (is greater for the naoh solvent) [ca2+] = [oh-] as long as pure water is solvent. Use a dry container for filtrate if not dry, rinse the glassware with filtrate first. Film of particles may form on the liquid surface.
