Iodide ions, I−(aq)\text{I}^-(\text{aq})I−(aq), react with permanganate ions, MnO4−(aq)\text{MnO}_4^-(\text{aq})MnO4−(aq), in a basic solution. The unbalanced equation is shown below:
I−(aq)+MnO4−(aq)+H2O(l)→I2(s)+MnO2(s)+OH−(aq) \text{I}^-(\text{aq}) + \text{MnO}_4^-(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightarrow \text{I}_2(\text{s}) + \text{MnO}_2(\text{s}) + \text{OH}^-(\text{aq}) I−(aq)+MnO4−(aq)+H2O(l)→I2(s)+MnO2(s)+OH−(aq)What is the ratio of MnO2(s)\text{MnO}_2(\text{s})MnO2(s) to OH−(aq)\text{OH}^-(\text{aq})OH−(aq) in the balanced chemical equation?
1:41 : 41:4
1:21 : 21:2
3:43 : 43:4
3:83 : 83:8
