Explain the following a. Oxidising and reducing nature of water b. Hydrolysis reaction

1. Water as oxidising agent: Water oxidised metals and reduces itself to give Hydrogen. This is because, metals have reduction potential less than 0 and can be oxidised by Hydrogen as it has electrical potential equal to zero. For example:

       2 Na(s) + 2 H₂O (l) $\to$ 2 NaOH(aq) + H₂(g)

2. Water as reducing agent: Those elements that have electrical reduction potential more than zero, are reduced by water. For example:

  H₂O (aq) + Cl_​2(g) $\to$ HCl(aq) + HClO(aq)

3. Hydrolysis Reaction: When some transition metal ions are dissolved in water, they undergo a reaction with water molecules and the reaction is called hydrolysis. This is as shown:

               Cu²⁺(aq) + 2 H₂O (aq) $\to$ [Cu(OH)₂]²⁺ (aq) + 2 H⁺ (aq)