State True/False
`La(OH)_3` is less basic than `Lu(OH)_3`

Explanation

To determine whether the statement "La(OH)₃ is less basic than Lu(OH)₃" is true or false, we need to analyze the basicity of the hydroxides of lanthanum (La) and lutetium (Lu).

### Step-by-step Solution:

1. **Understanding Basicity**: Basicity refers to the ability of a substance to accept protons (H⁺ ions) or donate electron pairs. In the case of metal hydroxides, basicity is often related to the ionic character of the compound.

2. **Lanthanide Contraction**: The lanthanide series shows a trend known as lanthanide contraction, where the size of the lanthanide ions decreases from lanthanum (La) to lutetium (Lu). This occurs due to the poor shielding effect of the f-electrons.

3. **Effect of Ion Size on Basicity**: As the size of the cation decreases, the covalent character of the hydroxides increases. Smaller cations tend to polarize the hydroxide ion (OH⁻) more effectively, leading to a stronger bond and thus a weaker base.

4. **Comparing La(OH)₃ and Lu(OH)₃**:
- La³⁺ is larger than Lu³⁺.
- Therefore, La(OH)₃ has a more ionic character compared to Lu(OH)₃, which has a greater covalent character due to the smaller size of Lu³⁺.

5. **Conclusion**: Since La(OH)₃ is more ionic and thus more basic than Lu(OH)₃, the statement "La(OH)₃ is less basic than Lu(OH)₃" is false.

### Final Answer:
The statement is **False**.