Which salt can furnish $H^{+}$ ion in its aqueous solution?

Calculate the dissociation constant of a $0.001 \ M$ weak monoacidic base undergoing $2 \%$ dissociation.

The Bronsted acids in the reversible reaction are $HCO_3^- (aq) + OH^- (aq) \rightleftharpoons CO_3^{2-} (aq) + H_2O (l)$

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 and sodium hydroxide is $13.7 \, kcal$. The heat liberated when one mole of water is formed by combining sulphuric acid and sodium hydroxide is......$kcal$

The conjugate base of $H_{2}PO_{4}^{-}$ is:

What are diprotic and triprotic acids? Explain with differentiation.