can you just tell me if this statement is correct

if a compounds conjugate base is aromatic then it is more acidic compared to a compound whose conjugate base is anti or non aromatic

if a base is aromatic it is weaker than a base that is anti aromatic

To evaluate these statements, we need to consider the concept of aromaticity, acid strength, and base strength in organic chemistry.

1. "If a compound's conjugate base is aromatic, then it is more acidic compared to a compound whose conjugate base is anti or non-aromatic."

Aromatics are generally more acidic compared to anti-aromatic or non-aromatic compounds. The presence of a stable aromatic system in a compound stabilizes its conjugate base, making it more likely to dissociate and release a proton (H+). This is known as the "conjugate base stability" principle. So, the statement is generally correct.

To determine the acidity of a compound or compare it with its conjugate base, you can consider the following factors:

- Resonance stabilization: Look for stable resonance structures involving the conjugate base. Aromatic systems have considerable resonance stabilization.
- Electron withdrawing groups: Compounds with electron-withdrawing groups at the acidic site increase acidity, as they stabilize the conjugate base through induction or resonance.
- Hybridization: Greater acidity is often observed when the acidic hydrogen is more "s" character and less "p" character, as a more stable base can be formed.

2. "If a base is aromatic, it is weaker than a base that is anti-aromatic."

This statement is not entirely accurate. In fact, aromatic bases are generally weaker than non-aromatic bases. Basicity is determined by the ability to donate electrons and accept protons (H+). Aromatic rings tend to have stable localized electron density due to the delocalization of pi-electrons, which decreases their tendency to accept protons. Therefore, non-aromatic bases, which lack this stabilization, are usually stronger.

To compare the basicity of different compounds or bases, you should consider the following factors:

- Electron donating groups: Compounds or groups that donate electrons will increase basicity since they can easily give lone pairs.
- Steric hindrance: Bulky groups near a basic site will hinder the donation of lone pairs, reducing basicity.
- Resonance effects: In some cases, resonance stabilization can lead to the enhancement of basicity by enabling better delocalization of the lone pair of electrons. However, this is less common for aromatic bases.

Remember, these guidelines are general, and specific compounds may have unique factors affecting their acidity or basicity.