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Unformatted text preview: ith the dissolved substances – Given a compound added to an acid or base at equilibrium, predict equilibrium shifts (to the left or right), if [H+] or , if [OH–] or , and if pH or , – Calculate the pH of an acid or base solution when a common ion is added. Acid‐Base Titrations – Distinguish between endpoint (when indicator changes color) and equivalence point (when equal amounts of H+ or HA and OH– present) – Know general pH range for equivalence point of following: – strong acid‐strong base titration (pH≈7) – weak acid‐strong base titration (pH>7) – strong acid‐weak base titration (pH<7) – Recognize that pH=pKa at halfway to equivalence point for a weak acid‐strong base titration. – Given titration data, calculate the pH at any point during an acid‐base titration. Write the net ionic equations for the neutralization reactions. Account for amount of H+ and OH– neutralized and the resulting initial [HA] or [A–] Set up ICE table then solve for x to get [H+] or [OH–] Calculate pH based on [H+] or [OH–] Carry out titration calculations for polyprotic acids or for salts c...
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This document was uploaded on 03/22/2014 for the course CHEM 162 at Seattle Central Community College.
- Fall '11