For a dibasic acid, `H_(2)A hArr HA^(-) + H^(+) (K_(1))`
`HA^(-) hArr A^(2-) + H^(+)(K_(2))`
`H_(2)A hArr 2H^(+) + A^(-2)(K)` then

For H_(3)PO_(4) , H_(3)PO_(4) hArr H_(2)PO_(4)^(-) + H^(+) (K_(1)) H_(2)PO_(4)^(-) hArr HPO_(4)^(2-) + H^(+) (K_(2)) HPO_(4)^(2-) hArr PO_(4)^(3-) + H^(+) (K_(3)) then

K_(a_(1)), K_(a_(2)) and K_(a_(3)) are the respective ionisation constants for the following reactions. H_(2)S hArr H^(+)+HS^(-) HS^(-)hArr H^(+)+S^(2-) H_(2)S hArr 2H^(+)+S^(2-) The correct relationship between K_(a_(1)), K_(a_(2)) and K_(a_(3)) is

The following equilibrium constants are given : N_(2) + 3 H_(3) hArr 2 NH_(3) , K_(1) N_(2) + O_(2) hArr 2 NO , K_(2) H_(2) + 1/2 O_(2) hArr H_(2) O , K_(3) The equilibrium constant for the oxidation of NH_(3) by oxygen to give NO is :

The relation between K_(p) and K_(c) is K_(p)=K_(c)(RT)^(Deltan) unit of K_(p)=(atm)^(Deltan) , unit of K_(c)=(mol L^(-1))^(Deltan) H_(3)ClO_(4) is a tribasic acid, it undergoes ionisation as H_(3)ClO_(4) hArr H^(o+)+H_(2)ClO_(4)^(-), K_(1) H_(2)ClO_(4)^(-) hArr H^(o+)+HClO_(4)^(2-), K_(2) HClO_(4)^(2-) hArr H^(o+)+ClO_(4)^(3-), K_(3) Then, equilibrium constant for the following reaction will be: H_(3)ClO_(4) hArr 3H^(o+)+ClO_(4)^(3-)