A 0.213-g sample of uranyl(VI) nitrate, UO₂(NO₃)₂, is dissolved in 20.0 mL of 1.0 M H₂SO₄ and shaken with Zn. The zinc reduces the uranyl ion, UO₂²⁺, to a uranium ion, Uⁿ⁺. To determine the value of n, this solution is titrated with KMnO₄. Permanganate is reduced to Mn²⁺ and Uⁿ⁺ is oxidized back to UO₂²⁺.
(a) In the titration, 12.47 mL of 0.0173 M KMnO₄ was required to reach the equivalence point. Use this information to determine the charge on the ion Uⁿ⁺.
(b) With the identity of Uⁿ⁺ now established, write a balanced net ionic equation for the reduction of UO₂²⁺ by zinc (assume acidic conditions).
(c) Write a balanced net ionic equation for the oxidation of Uⁿ⁺ to UO₂²⁺ by MnO₄⁻ in acid.