titration of weak acid with a weak base

This type of titration is carried out between a weak acid such as acetic acid (CH 3 COOH) and weak base such as ammonium hydroxide (NH 4 OH). There is no sharp change in the pH during the titration. Hence, no sharp equivalence..

This type of titration is carried out between acetic acid and sodium hydroxide. The free H + ion from the weak acid is neutralized by OH - ions from the base and there is a small increase in pH. Around the equivalence point large increase in pH..

The heat of neutralization of a weak acid or a weak base is less than -57.1 kJ and is also different for different weak acids or bases. For example for acetic acid the enthalpy of neutralization is -54.9 kJ. This can b..

In this case both the cation and anion undergo hydrolysis to the same or different extents. The resulting solution may be neutral, acidic or basic depending upon the relative strengths of acids and bases. The hydrolysis may be written as: Some common examples are CH 3 ..

A base that dissociates in water only partially is known as a weak base. Example: Examples of Bases Strong Weak Sodium hydroxide: NaOH Magnesium hydroxide: Mg(OH) 2 Potassium hydroxide: KOH Calcium hydroxide: Ca(OH) 2 Ammonium ..

Here, cation B + undergoes hydrolysis to give free H + ions. Therefore the resulting solution will be acidic in character having pH less than 7. For example, ..

Salt of a Strong Acid and Weak Base - Here, cation B + undergoes hydrolysis to give free H + ions. Therefore the resulting solution will be acidic in character having pH less than 7. For example, Other examples of this type of salts are NH 4 Cl, CuSO 4 , AlCl..

An acid which dissociates very feebly in water and whose molecules mostly remain in the undissociated form is categorized as a weak acid. It behaves as a weak electrolyte. ..

A base that dissociates only partially into ions in aqueous medium is called a weak base. It behaves as a weak electrolyte..

A weak electrolyte ionises or dissociates only partially to form free mobile ions. Most of the electrolyte remains as un-ionised molecules. For example in acetic acid, the number of its dissociated ions (the acetate and hydrogen ions) is less compared to the total amount of acet..