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.
e. phosphoric acid and dihydrogen phosphate ion. 15. Which of the following can be mixed together in water to produce a buffer solution? a. HClO 4 and NaClO 4 d. H 3PO 4 and NaH 2PO 4 b. HNO 3 and NaNO 3 e. HCl and NaCl c. H 2SO 4 and NaHSO 4 16. Which one of the following would make the best buffer? (Ac = acetate, CH 3CO 2) a.
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