The enthalpy of formation of `H_(2)O(l)` is `-285 KJ mol^(-1)` and enthalpy of neutralization of a stron acid and a strong bas is `-55 KJ mol^(-1)`. What is the enthalpy of formation of `OH^(-)` ions?

Explanation

To find the enthalpy of formation of `OH^(-)` ions, we can use the given data about the enthalpy of formation of `H2O(l)` and the enthalpy of neutralization of a strong acid and a strong base.

### Step-by-Step Solution:

1. **Identify the given values**:
- Enthalpy of formation of `H2O(l)`: ΔH_f(H2O) = -285 kJ/mol
- Enthalpy of neutralization of a strong acid and a strong base: ΔH_neutralization = -55 kJ/mol

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