You are titrating 25.025.0 mL of 0.0100 M Sn2 Sn2 in 1 M HCl HCl with 0.0500 M Tl3 Tl3 resulting in the formation of Sn4 Sn4 and Tl Tl . A PtPt indicator electrode and a saturated Ag|AgCl Ag|AgCl reference electrode are used to monitor the titration. What is the balanced titration reaction

Sn²⁺ + Tl³⁺ → Sn⁴⁺ + Tl⁺

Explanation:

The Sn²⁺ is oxidized to Sn⁴⁺. Whereas Tl³⁺ is reduced to Tl⁺. The half-reactions are:

Sn²⁺ → 2e⁻ + Sn⁴⁺ (Oxidation, loosing electrons)

Tl³⁺ + 2e⁻ →Tl⁺ (Reduction, gaining electrons)

The sum of the reactions gives:

Sn²⁺ + Tl³⁺ + 2e⁻ → 2e⁻ + Sn⁴⁺ + Tl⁺

Subtracting the electrons in both sides of the reaction: