) ] + (aq) + 3OH – (aq) → C H COO – (aq) + 2Ag(s) + 4NH (aq) + H O(l) (d) C H CHO(l) + 2Cu + (aq) + 5OH – (aq) → No change observed. What inference do you draw about the behaviour of Ag + and Cu + from these reactions ? . Balance the following redox reactions by ion – electron method : (a) MnO – (aq) + I – (aq) → MnO (s) + I (s) (in basic medium) (b) MnO – (aq) + SO (g) → Mn + (aq) + HSO – (aq) (in acidic solution) (c) H O (aq) + Fe + (aq) → Fe + (aq) + H O (l) (in acidic solution) (d) Cr O – + SO (g) → Cr + (aq) + SO – (aq) (in acidic solution) .
Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent. (a) P (s) + OH – (aq) → PH (g) + HPO – (aq) (b) N H (l) + ClO – (aq) → NO(g) + Cl – (g) (c) Cl O (g) + H O (aq) → ClO – (aq) + O (g) + H + . What sorts of informations can you draw from the following reaction ? (CN) (g) + 2OH – (aq) → CN – (aq) + CNO – (aq) + H O(l) .
The Mn + ion is unstable in solution and undergoes disproportionation to give Mn + , MnO , and H + ion. Write a balanced ionic equation for the reaction. . Consider the elements : Cs, Ne, I and F (a) Identify the element that exhibits only negative oxidation state.
(b) Identify the element that exhibits only postive oxidation state. (c) Identify the element that exhibits both positive and negative oxidation states.