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What is the relation of K(sp), solubility constant to soulubility?
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What is the common ion effect?
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MCAT Acids/Bases

QuestionAnswer
What is the relation of K(sp), solubility constant to soulubility? K(sp) is directly related to solubility; therefore the larger the K(sp) the more soluble the product
What is the common ion effect? Another form of Le Chatelier's Principle, the the decrease in the solubility of a salt occurs because another salt is added that contains one of its ions.
What is the relatonship bw autoionization of water K(w) and temp it increases when temp increases
polyprotic can accept or donate more than one H+
high [H] means... low pH and the solution is acidic
pH + pOH = 14
pH = -log[H] or -log[H3O+]
pOH = -log[OH]
What is the relation bw K(a) and pKa? The larger the K(a) value the smaller the pKa value and therefore the stronger the acid
What is the Henderson-Hasselbalch equation? pH = pKa + log {[conjugate base]/[weak acid]}
what happens at a half-equivalence point? the pKa equals the pH
K(w) = [H3O+][OH-]
Titration equation pH = [vol acid]/ [vol base]
pKa + pKb = 14
Created by: studypants
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