The `K_(a)` values for `HPO_(4)^(2-)` and `HSO_(3)^(-)` are `4.8xx10^(-13)` and `6.3xx10^(8)` repectively. Therefore, it follows the `HPO_(4)^(2-)` is … acid than `HSO_(3)^(-)` and `PO_(4)^(3-)` is a …… base than `SO_(3)^(2-)`

The anhydride of acid H_(3)PO_(4) and HPO_(3) are:

K_(a1),K_(a2),K_(a3) values for H_(3)PO_(4) are 10^(-3),10^(-8) and 10^(-12) respectively .If K_(w)(H_(2)O)=10^(-14) then , (i) What is dissociation constant of HPO_(4)^(2-) ? (ii) What is K_(b) of HPO_(4)^(2-) (iii) What is K_(b) of H_(2)PO_(4)^(-) ? (iv) What is order of K_(b) of Po_(4)^(3-)(K_(b_(3))),HPO_(4)^(2-)(K_(b_(2))) and H_(2)PO_(4)^(-)(K_(b_(1))) ?

Identify the acid-base pair in the following reaction : HSO_(4)^(-) (aq) + PO_(4)^(3-) (aq) to SO_(4)^(2-) (aq) +HPO_(4)^(2-) (aq)

The conjugate base of H_(2)PO_(4)^(-) is : a) H_(3)PO_(4) b) H_(2)PO_(4)^(-) c) HPO_(4)^(2-) d) PO_(4)^(3-)

pH of 0.1M Na_(2)HPO_(4) and 0.2M NaH_(2)PO_(4) are respectively: (pK_(a)"for" H_(3)PO_(4) are 2.12, 7.21 and 12.0 for respective dissociation to HPO_(4)^(2-), HPO_(4)^(-) and PO_(4)^(3-)) :

Out of the following, amphiprotic species are I. HPO_(3)^(2-) II. OH^(-) III. H_(2)PO_(4)^(-) IV. HCO_(3)^(-)