In neutral medium $\mathrm{KMnO}_4$ oxidises $\mathrm{MnSO}_4$ to _________

In a neutral or weakly alkaline medium, potassium permanganate ($\mathrm{KMnO}_4$) acts as an oxidizing agent and is reduced to manganese dioxide ($\mathrm{MnO}_2$). The chemical reaction between $\mathrm{KMnO}_4$ and $\mathrm{MnSO}_4$ in a neutral medium is given by: $2\mathrm{KMnO}_4 + 3\mathrm{MnSO}_4 + 2\mathrm{H}_2\mathrm{O} \rightarrow 5\mathrm{MnO}_2 + \mathrm{K}_2\mathrm{SO}_4 + 2\mathrm{H}_2\mathrm{SO}_4$ In this reaction, the manganese ion $\mathrm{Mn}^{2+}$ from $\mathrm{MnSO}_4$ is oxidized to $\mathrm{MnO}_2$ (where the oxidation state of Mn is +4), and the permanganate ion $\mathrm{MnO}_4^-$ is reduced to $\mathrm{MnO}_2$. Thus, the product formed is $\mathrm{MnO}_2$. Answer: $\mathrm{MnO}_2$