Transcription of Test3 ch17b Buffer-Titration-Equilibrium Practice Problems
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Test3 ch17b Buffer-Titration-Equilibrium Practice Problems
1 General Chemistry II Jasperse Buffers/ titrations /Solubility. Extra Practice Problems General Types/Groups of Problems : Buffers General p1 Titration Graphs and Recognition p10 What Kind of Solution/pH at End? p2 Titration Calculations p11 Preparation and Recognition of Buffers p4 pH Estimations/Calculations after acid/ base are added (including at Equivalence Point) p12 Buffer Calculations p5 Solubility Problems p14 Disrupted Buffers: After Acid or base are Added p7 Impact on Solubility When Common Ions are Present p16 Titration-Related Problems p9 Impact of pH on Solubility p17 Key Equations Given for Test: For weak acids alone in water: [H+] = KaxWA[] For weak bases alone in water: [OH-] = KbxWB[] pZ= -logZ General definition for p of anything pH + pOH = 14 [H+][HO-] = x 10-14 KaKb= x 10-14 for conjugate acid/ base pair For Buffer: pH = pKa + log[ base ]/[acid] Henderson-Hasselbalch Equation S = S (products) S (reactants) G = G (products) G (reactants) G = H T S (T in Kelvin) BUFFERS 1.
Answer: A buffer consists of a weak acid and its conjugate base in roughly equal amounts. If acidis added to the solution, it is consumed by the conjugate base. If base is added to the solution, it is consumed by the weak acid. If the amounts are such that the ratio of conjugate base/weak acid concentrations doesn’t change much, then the pH
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