For the redox reaction: I⁻ + ClO3⁻ + H2SO4 - Cl⁻ + HSO4⁻ + I2, which of the following statements is/are correct?

Question

For the redox reaction: I⁻ + ClO3⁻ + H2SO4 -> Cl⁻ + HSO4⁻ + I2, which of the following statements is/are correct?

Accepted Answer

Iodide ion is oxidised in this reaction. Balancing the equation gives: 6I⁻ + ClO3⁻ + 3H2SO4 -> Cl⁻ + 3HSO4⁻ + 3I2 + 3H2O. Wait — let me recount: multiply oxidation half by 3 and reduction half by 1: 6I⁻ -> 3I2 + 6e⁻; ClO3⁻ + 6H⁺ + 6e⁻ -> Cl⁻ + 3H2O. Combined (using H2SO4 as source of H⁺): 6I⁻ + ClO3⁻ + 6H⁺ -> Cl⁻ + 3I2 + 3H2O; 6H⁺ comes from 3H2SO4 giving 6HSO4⁻? No — H2SO4 -> H⁺ + HSO4⁻, so 6H⁺ from 6H2SO4? Let me re-examine: 6H2SO4 -> 6H⁺ + 6HSO4⁻; so coefficient of HSO4⁻ = 6. I⁻ goes from -1 to 0 (oxidised). Cl goes from +5 to -1 (reduced). S stays +6. H2O is a product (3 molecules). So correct statements: HSO4⁻ coefficient is 6, iodide is oxidised, water is a product.

For the redox reaction: I⁻ + ClO3⁻ + H2SO4 -> Cl⁻ + HSO4⁻ + I2, which of the following statements is/are correct?

Solution

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