The ionic product of water is constant at all temperature.True/False.

Answer

To determine whether the statement "The ionic product of water is constant at all temperatures" is true or false, we can analyze the dissociation of water and its relationship with temperature.

### Step-by-Step Solution:

1. **Understanding the Ionic Product of Water (Kw)**:
- The ionic product of water (Kw) is defined as the product of the concentrations of hydrogen ions (H⁺) and hydroxide ions (OH⁻) in water at equilibrium.
- Mathematically, it is expressed as:
\[ K_w = [H^+][OH^-] \]

2. **Dissociation of Water**:
- Water undergoes dissociation to form H⁺ and OH⁻ ions:
\[ H_2O \rightleftharpoons H^+ + OH^- \]

3. **Effect of Temperature on Dissociation**:
- The dissociation of water is an endothermic process, meaning it absorbs heat.
- According to Le Chatelier's principle, if the temperature increases, the equilibrium will shift to favor the endothermic direction, which is the dissociation of water.

4. **Increasing Temperature**:
- When the temperature increases, the dissociation of water increases, leading to a higher concentration of H⁺ and OH⁻ ions.
- Therefore, as the concentrations of H⁺ and OH⁻ ions increase, the ionic product (Kw) also increases.

5. **Conclusion**:
- Since the ionic product of water (Kw) changes with temperature, the statement "The ionic product of water is constant at all temperatures" is **False**.

### Final Answer:
**False** - The ionic product of water is not constant at all temperatures; it increases with an increase in temperature.