The conjugate base of a strong acid is a weak base; therefore, the conjugate acid of a strong base is a weak acid. Acid-Base Pairs and Buffer Chemistry A buffer solution contains a weak acid and its conjugate base or a weak base and its conjugate acid. Buffers work by reacting with a base or acid to control the pH of a solution.
When a weak base and a strong acid are mixed, they react according to the following net-ionic equation: B (aq) + H₃O⁺ (aq) → HB⁺ (aq) + H₂O (l). If the acid and base are equimolar, the pH of the resulting solution can be determined by considering the equilibrium reaction of HB⁺ with water. If the base is in excess, the pH can be

Transcript. In a weak base-strong acid titration, the acid and base will react to form an acidic solution. A conjugate acid will be produced during the titration, which then reacts with water to form hydronium ions. This results in a solution with a pH lower than 7. An example of this is the titration of hydrochloric acid (strong acid) into

There are very few strong bases (Table \(\PageIndex{1}\)); any base not listed is a weak base. All strong bases are OH - compounds. So a base based on some other mechanism, such as NH 3 (which does not contain OH − ions as part of its formula), will be a weak base.

The hydrogen ion from the acid combines with the hydroxide ion to form water, leaving the nitrite ion as the other product. The resulting solution is not neutral (pH \(= 7\)), but instead is slightly basic. Reactions can also involve a weak base and strong acid, resulting in a solution that is slightly acidic.

Ammonia (NH3) is a weak base because it partially dissociates in water to produce hydroxide ions (OH-) and ammonium ions (NH4+). In a solution of ammonia, not all ammonia molecules will react with water, leading to a limited number of OH- ions. Potassium hydroxide (KOH), on the other hand, is a strong base because it completely dissociates in
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    • which hydroxide is a weak base