2003 (2-28) 1220-E2

2003 (2-28) 1220-E2 - (5(5(5 0(a l 2 3 4 February 28...

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Unformatted text preview: (5) (5) (5) 0.(a) l. 2. 3. 4. February 28, CHEMISTRY 1220 SECOND EXAM 11121! g Work! 2003 Name (Circle One) Seat # 0.(b) TA: Ben, Blake, Rehan (7:30, 8:35, 9:40) HClO4 and HNO3 appear equally acidic in aqueous solution because: (9) (h) they are equally acidic molecules. they are Bronsted—Lowry Acids. they are Lewis Acids. both (b) and (c). their conjugate bases are equally weak. of the common ion effect. they are monoprotic. of acid leveling. At the half—neutralization point (midpoint) of a titration of a weak acid with a strong base, the pH is: (a) (b) (c) (d) (e) 14 — pKa PKa pKa ‘ pr PKb - PKa 7 — pKa A buffer solution containing a weak acid and its conjugate base: (a) (b) (c) (d) will always be acidic due to the common ion effect. may be acidic, basic, or neutral depending on Ka and concentrations. will always be basic since the conjugate base must be strong. must have a lower pH than a buffer composed of a weak base and its conjugate acid. both (a) and (C). Which of the following, as a 1:1 mixture, would not lead to a buffered solution on dissolution in water? (a) (b) (C) (d) (e) (f) H3 P04 /NaH2 P04 NaH2 P04 /Na2HPO4 NazHPO4 /Na3 P04 HCN/NaCN HF/NaF HCl/NaCl 2 (5) 5. The reason that indicators change colors in acid/base titrations is that: (a) they are chosen to share a common ion with the salt formed at the endpoint. (b) they are weak acids or bases whose conjugate forms differ in color. (c) they are weak acids or bases which can not be used to make buffered solutions. (d) they are polyprotic acids or bases for which only the intermediate amphiprotic specie(s) is/are colored. (e) they are Lewis acids or bases, but not Bronsted-Lowry acids or bases. (5) 6. which of the following should not be able to be a ligand (Lewis base) in any usual way? (a) H20 (b) NH3 (c) NH4+ (d) BH3 (e) (a) and (b) (f) (C) and (d) (10) 7. Give the get iQEiE eguations that occur as a result of the mixing of a 1.0 M solution of NaZHPO4 with: (a) (b) an equal volume of 1.0 M HCl. an equal volume of 1.0 M NaOH. (lO) 8. (15) 9. Low spin: Determine the value of K for the following aqueous reaction: 2NH4+ + Ag+ + 21-120 ——x Ag(NH3)2+ + 2 H3o+ K: While almost all six—coordinate complexes involve octahedral coordination, a very few have trigonal prismatic coordination (right). For a hypothetical trigonal prismatic complex of stoichiometry MXZZ4 (X and Z are simple ligands), provide a drawing for each possible isomer. Also, what is the smallest value of n for which one can have high and low spin dn configurations? Show the electron populations for each below. ‘_ High spin: '—“ ‘— < M at center = ligand dxz, dyz dfi dxy, dx2_y2 (l0) 10. What would the pH be for a solution which was prepared by dissolving 1.0 moles of NaF and 0.10 moles of HP in enough water to give a total volume of 1.0 liters? pH=______— 11. What is the oxidation state of Cr in the compound [Cr(NH3)5Cl]SO4? Answer I 12. Given that the value of Kf for the Fe(SCN)2+ complex is 920, determine the values of [Fe(SCN)2+], [Fe3+], and [SCN'] that would result on dissolving 0.50 moles of Fe3+ and 0.50 moles of SCN‘ in water until the volume reached 1.0 liters. [Fe(SCN)2+] = [Fe3+] = [SCN'] = 2221‘}; HF 6.9-10‘4 Kf Ag(NH3)2+ 1.7-107 NH4+ 5.6-10'10 HCN 5.8-10’10 ...
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