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Consider the equilibrium reactions, H...

Consider the equilibrium reactions,
`H_(3)PO_(4)overset(K_(1))(hArr ) H^(+)+H_(2)PO_(4)^(-)`
`H_(3)PO_(4)^(-)overset(K_(2))(hArr ) H^(+)+HPO_(4)^(-2)`
`HPO_(4)^(-2)overset(K_(3))(hArr)H^(+)+PO_(4)^(-3)`
The equilibrium constant K for the following dissociation
`H_(3)PO_(4)hArr 3H^(+)+PO_(4)^(-)` is

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Phosphoric acid ionises as : H_(3)PO_(4)overset(K_(1))hArr H^(+)+H_(2)PO_(4)^(-) H_(2)PO_(4)^(-)overset(K_(2))hArr H^(+)+H_PO_(2)^(-) H_(2)PO_(4)^(2-)overset(K_(3))hArr H^(+)+PO_(3)^(-) The equilibrium constant, K for the reaction : H_(3)PO_(4)hArr 3H^(+)+PO_(4)^(3-) is :

The equilibrium constant for the reactions are : H_3PO_4 oversetKrarr H^+ + H_2PO_4^- : K_1 H_2PO_4 oversetKrarr H^+ + HPO_4^(2-) : K_2 HPO_4^(2-) oversetKrarr H^+ + PO_4^(3-) : K_3 The equilibrium constant for H_3PO_4 rarr 3H^+ + PO_4^(3-) will be :

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-)

H_(4)underline(P_(2))O_(6)+H_(2)O to H_(3)PO_(3)+H_(3)PO_(4)

H_(4)underline(P_(2))O_(6)+H_(2)O to H_(3)PO_(3)+H_(3)PO_(4)

H_(4)underline(P_(2))O_(6)+H_(2)O to H_(3)PO_(3)+H_(3)PO_(4)