Lab #2 "Developing a Mastery of the Solubility Product Constant," introduces an experimental way to determine the Ksp for Ca(IO3)2. Remember that chemistry is an experimental science where measurements are made. The Ksp Tables you see in the textbook have been crafted from experimental data, and proper interpretation of these values can tell a chemist a great deal about solubility.
Experimentally we can consider solubility equilibria to make predictions about the amount of a given compound that will dissolve. As we progress through the solubility unit we will then discuss various ways to manipulate the solubility of various salts.
Be sure to have a grasp of what an equilibrium constant tells you. A large value for k favors the products, and a small value of k favors reactants. If you have the experimental value for the Ksp you can calculate the molar solubility for a slightly soluble salt. I ended class with several calculations of how to determine the molar solubility of a list of slightly soluble salts and will sontinue with that discussion on Monday.
Today's inspirational quote was submitted by Erin Riley
“We are what we repeatedly do. Excellence, therefore, is not an act, but a habit."
-Aristotle
Songs Played Before Class
Bruce Springsteen - Glory Days
Mase - Welcome Back
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