In acid-base chemistry, the leveling effect refers to the limitation imposed by the solvent on the strength of acids and bases in solution. When a base stronger than the solvent's conjugate base is used, it deprotonates the solvent until the base is entirely consumed, making it ineffective against weaker acids. Conversely, an acid stronger than the solvent's conjugate acid protonates the solvent until the acid is depleted, rendering it ineffective against weaker bases. Essentially, the solvent neutralizes stronger acids and bases, preventing them from reacting as intended with other compounds.

For example, in water (an aqueous solution), a strong base like the amide ion deprotonates water, predominantly forming hydroxide ions and leaving few amide ions. This prevents the amide ions from effectively deprotonating compounds like acetylene, which have a higher pKa than water. However, if a more basic solvent like ammonia is used, the amide ions can successfully deprotonate acetylene, facilitating the desired reaction.

In summary, the solvent's acidity limits the effectiveness of strong bases, and its basicity limits the effectiveness of strong acids. The chosen solvent must, therefore facilitate the acid-base reaction without undergoing a significant reaction itself.