1)Which of the reactions involving metal ions (equations 1A - 6B)(there is no 5A

Question

1)Which of the reactions involving metal ions (equations 1A - 6B)(there is no 5A) represent redox reaction(s)? Write down the entire equation(s) AS WELL AS their corresponding balanced oxidation half-reaction(s) AND reduction half-reaction(s). 2)The Al3+ and Zn2+ ions are amphoteric. Describe how the amphoteric nature of these ions is shown in your testing.

MIXTURE A (Test Tube A-1). Presence of silver ion, Ag [Perfom same tests to unknown U-1]: Silver ion A is one of a limited number of metal ions which form a precipitate in acidic solutions since the chloride ion is a weak conjugate base that does not react further with hydronium ion 1. Mix 1mL of each of 0.2M AgNO 3(aq 0.2M Fe(NO3)3(ag), 0.2M Co (NO3)2(aq) n test tube A-1 2. Add 8 drops of 6M aq solution to test tube A-1 Ag (aq HC aq H20 Agc s, white H30 aq Eq. 1A 3. Silver ions can now be separated as solid AgCls) from the mixture by centrifuging the test tube and decanting the supernatant into test tube A-2 for further analyses. 4. Wash the silver ion precipitate, AgC s), with 1mL of DI water. Centrifuge and discard water 5. To confirm that the precipitate that remains in test tube A-1 is indeed made up of silver ions add a ligand, 1mL of 6 M NH3(aq) which forms a colorless complex with silver ions but more importantly increases solubility of AgC and shifts equilibrium to the right AgCl (s) 2NH3(aq) F [Ag (NH3)21+ aq C aq Eq. 2A 6. Add nitric acid, HNO 3 (aq dropwise which reacts with ammonia, NH3, for equilibrium to shift to the left, until more precipitate, AgC 1.8x10 10 forms sp MIXTURE A, test tube A-2. Presence of iron (III) ion, Fe n the supernatant 3+ Iron (IID On (Fe3+) forms an insoluble hydroxide in basic solutions 7. Add ammonia, 6M NH3(ag), dropwise (3 or so) to the supernatant that was decanted until its pH rises to basic levels. Use red litmus paper to confirm that pH is basic. Once the solution is

Explanation / Answer

The redox reaction is :

2Mn^2+ +5BiO3^- + 14H3O+ = 2MnO4^- + 5Bi^3+ + 21H2O

Oxidation reaction : Mn^2+ 4H2O ---------> MnO4^- + 8H+ + 5e

Reduction : BiO3^- + 6H+ + 2e- -------------> Bi^3+ + 3H2O

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Al^3+ and Zn^2+ forms soluble complexes[ Al (H2O)3(OH)4]^- and [Zn(OH)4]^2- which indicates their amphoteric nature

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