Differentiate between the terms strength and concentration as they apply to acids and bases. When is \(\mathrm{HCl}\) strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?

The strength of an acid or base refers to their ability to ionize in water, with strong acids/bases ionizing almost completely, and weak acids/bases partially ionizing. This is represented by the dissociation constant, Ka for acids and Kb for bases. Concentration refers to the amount of substance in a solution, usually expressed in moles per liter or molarity. HCl is a strong acid, but it becomes weak if not completely ionized due to the presence of other molecules. It is concentrated when its molarity is high and dilute when low. Ammonia is a weak base with a low Kb value. It is concentrated when its molarity is high and dilute when low. The conjugate base of a weak acid is usually a weak base, as it does not readily attract protons to form the corresponding acid. However, some exceptions exist.