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How do strong bases differ from weak bases in water?

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sodium sulfate — acid–base reaction Sodium sulfate, also called Glauber's salt, is, like other salts, the product of an acid-base reaction.

In chemistry, the distinction between strong and weak bases in water is defined by their degree of dissociation or their ability to produce hydroxide ions (OH⁻) in solution.123

Strong Bases: These substances dissociate completely in aqueous solution. Common examples include the hydroxides of alkali and alkaline earth metals, such as sodium hydroxide or calcium hydroxide. Because they ionize fully, they produce a high concentration of hydroxide ions.413
Weak Bases: These substances do not dissociate completely in water. Instead, they exist in a state of equilibrium where only a portion of the base reacts with water to produce hydroxide ions. Ammonia and its organic derivatives, the amines, are classic examples of weak bases that produce hydroxide ions by reacting with water molecules.512

The relative strength of a base can be quantified using a dissociation constant ( $K_{b}$ ), which measures the basic strength of a substance relative to the lyate ion of the solvent. Bases with readily measurable, smaller dissociation constants are classified as weak, while those that react so completely that a constant is difficult to measure are considered strong.5