Question

Write balanced net ionic equations for each anion experiment (B through F)

B. IODIDE (I) 13. Place five drops of your anion solution in a test tube. Add five drops of 6 M HC,H,O, followed by two drops of 0.2 M KNO, A reddish-brown color confirms the presence of I (in I2). Record your results. С.BROMIDE (Br.) Place five drops of your anion solution in a test tube and add five drops of chlorine water. A brown colortion confirms the presence of Br (in the form of Br.). D. CARBONATE (CO,2) 15. Place a small amount of the solid anion sample in a test tube and add four drops of 6 M H,SO If a colorless, oderless gas is observed, hold a drop of Ba(OH), solution over the test tube. If the drop turns milky, CO,2 ions are confirmed. E. CHLORIDE (Cl) NOTE: Bromide and iodide will interfere with this test. 16. Place 10 drops of a solution of your anion in a test tube and add one drop of AgNO, solution.A white precipitate confirms the presence of chloride (as AgCI). F. NITRATE (NO,) NOTE: Bromide and iodide will interfere with this test. 17. Place 10 drops of your anion solution in a test tube. Add five drops of FeSO, and mix. 18. Carefully (without agitating the solution) pour conc. H,SO, down the side of the test tube so it forms two layers. If a brown ring forms between the two layers after 1-2 minutes, NO, ion is present.

Answer 1

B. Iodide

2KI + 2KNO₂ + 4CH₃COOH = 4CH₃COOK + I₂ + 2NO + 2H₂O

C. Bromide

2 Br^- + Cl₂ → Br₂ + 2 Cl^-

D. Carbonate

1. CO₃^2- + 2 H⁺ → H₂O + CO₂

2. CO₂ + Ba(OH)₂ → BaCO₃ (milky white) + H₂O

E. Chloride

Cl^- + AgNO₃ → AgCl + NO₃^-

F. Nitrate

1. NO₃^- + 3 Fe²⁺ + 4 H⁺ → NO + 3 Fe³⁺ + 2 H₂O

2. [Fe(H₂O)₆]²⁺ + NO → [Fe(H₂O)₅(NO)]²⁺ (Brown ring)