Question

ANSWER ALL 3 QUESTIONS AND ALL PARTS

Question 1 Using the standard reduction potentials on page 127, draw a complete galvanic cell in the space below for Fe Ag a) Clearly label the electrodes, the solutions and the salt bridge. Clearly label which metal is the cathode and anode and a chemical you might use for the salt bridge. b) Give the half-reaction that occurs at the cathode and the half-reaction that occurs at the anode and indicate the direction of the electron flow and the ion(s) flow c) Give the complete, balanced redox reaction and determine the cell potential under standard conditions. Question 2: Using the titration curve given below; a) Calculate the molecular weight of the unknown weak base if 2.00 g of this weak base was used for the titration. Assume the base reacts with the acid in a 1:1 mole ratio. b) Indicate (with a circle or dot): L the positions of the equivalence point; Il the half equivalence point; and IIL buffer region. Titration of a weak base with a strong acid 12 10 0 5 10 15 20 25 30 35 40 45 50 55 60 Volume of 1 M HCI added (mL) Question 3: Using the titration curve given below; c) Calculate the molecular weight of the unknown weak acid if 1.50 g of this weak acid was used for the titration. Assume the base reacts with the acid in a 1:1 mole ratio. d) Indicate (with a circle or dot): IV. the positions of the equivalence point; V. the half equivalence point; and VIbuffer region. Weak acid titration with a strong base 12 10 a. 12 12.5 13.5 14 14.5 15 13 Volume of 0.9 M NaOH added (mL) Table of Standard Reduction Potentials at 25 C E (V 3.05 V Li (ag)L K+ (aq) + e. → K (s) Ba, (aq) + 2e → Ba (s) Sr (aq) + 2e- Sr (s) Ca2+ (aq) + 2e. → Ca (s) Na+(aq) + e. → Na (s) + 2 e. → Mg(s) Be2+ (aq) + 2e. → Be (s) AP (aq) + 3e Al (s) Mn'' (aq) + 2 e-→ Mn (s) 2H20 (I) + 2e → H2 (g) + 2 OH. (ag) Zn2 (ag) + 2e-Zn (s) Cr (aq) +3e- r (s) Fe (ag) + 2e- Fe (s PbS04 (s) + 2 e. → Pb (s) + SO42-(aq) Co (ag) + 2e Co (s) Ni (ag)+ 2e Ni (s) 2.93 V 2.90 V 2.89 v 2.87 V - 2.37 V 1.85 V 1.66 V -0.83 V 0.76 V 0.74 V 0.44 V -0.31 V 0.28 V 0.25 V 0.14 V Pb2 (ag) + 2e-Pb (s) Fe (aq) + 3e Fe(s) 2 H' (aq) + 2 e-→ H2 (g) Sn+ (aq) +2e-Sn2 (aq) Cu2+ (aq) + e. → Cu+ (aq) AgCl (s) + e-Ag(s) + Cl. (aq) (aq) + 2e-Cu(s 02 (8)+ 2H20+4e-4OH(aq 12 (s) + 2 e-→ 21. (ag) Mnor (aq) + 2 Hao (l) + 3 e.-MnO2 (s) + 40H (ag) 0.13 V -0.04 V 0.00 +0.13 V +0.15 V +0.22 V +0.34 V +0.40 V +0.53 V +0.59V +0.68 V +0.77 V +0.80 V Hg22+ (aq) + 2 e. → 2 Hg (l) NOs (aq)+ 4H (aq)+ 3e-NO (8) +2 H20 1) Br2 (1) + 2 e-2 Br (aq) + 4H' (aq) + 4 e. → 2 H2O MnO2(3)+ 4H (ag+ 2eMn(aq)+2 HO +0.85 V + 0.96 V +1.07 V +1.23 V +1.23 V +1.33 V + 2 e. → 2 Cl. 2 e2 Cl (aq) + 1.36 V C12( +1.50 V + 1.51 V Au'+ (aq) + 3 e. → Au (s + 1.61 V + 1.70 V Ce (aq)+e-Ce PbSO4 (s) + 2 e. → + 2 Hao (1) Ht (ag) + SO42 (ag) Pb02(s) + H202 (aq)+ 2 H (aq)+ 2 Co" (aq) 2e2 H2O + 1.77 V + 1.82 V Co - 02 (g) + HO ) +2.07 V 03 (g)+ 2 H +2.87 V

Answer 1

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