Why does the pH of an acidic buffer remian constant even when a few drops of a strong acid are added to it?

The pH of an acidic buffer can be raised by 2 units by

In some solutions, the concentration of H_(3)O^(+) remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as :

pH of a salt of a strong base with weak acid

The pH of an acidic buffer solution & a basic buffer solution at 25^(@)C is :

A buffer solution is made by mixing a weak acid HA (K_(a) =10^(-6)) with its salt NaA in equal amounts. What should be amount of acid or salt that should be added to make 90 mL of buffer solution in which if 0.1 mole of strong acid are added into 1 L of this buffer solution then change in pH is unity ?

pH of a 1 L buffer solution changes from 4.5 to 4.6 when 0.2 mole of a strong base is added to it. Its buffer capacity will be

State one appropriate observation for each of the following: A few drops of dilute hydrochloric acid are added to silver nitrate solution, followed by addition of ammonium hydroxide solution.

When a strong acid, strong base or their salt are dissolved in water, they are completely ionised. If a strong acid is added to a strong base, H^(+) ions from the former combine with OH^(-) ions of the latter forming water. The formation of each water molecule liberates a certain quantity of energy and the reaction is exothermic. The heat liberated when one mole of water is formed by combining hydrochloric acid sodium hydroxide is 13.7 kcal. The heat liberated when one mole of water is formed by combining sulphuic acid and sodium hydroxide is

The buffering action of an acidic buffer is maximum when its pH equals to

To an acidic solution of an anion, a few drops of Kmno_(4) solution are added. Which of the following, if present, will not decolourise the KMnO_(4) solution?