Consider the following equilibrium constants for a triprotic acid H3PO4--- First ionisation constant is k1. Second ions. const. is k2 and likewise third ionisation constant is k3. So, which of the following orders is correct ? k1>k3>k2 k3>k2>k1 k1>k2>k3 and what is the reason for this ?

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For $C u^{2 +}$ ion in $[C u (H_{2} O)_{4} (e n)]^{2 +}, [C u (H_{2} O)_{2} (e n)_{2}]^{2 +}$ and $[C u (e n)_{3}]^{2 +}$ with the stability constant $k_{1}, k_{2}$ and $k_{3}$ respectively, which of the following holds true?

Q. If

K_{1}, K_{2} a n d K_{3}

are equilibrium constant for formation of

A D, A D_{2} a n d A D_{3}

respectively as follow

A + D ⇌ A D, A D + D ⇌ A D_{2}, A D_{2} + D ⇌ A D_{3}

then equilibrium constant 'K" for

A + 3 D ⇌ A D_{3}

is related as

Q. If

K_{1}

K_{2}

be first and second ionisation constant of

H_{3} P O_{4}

and

K_{1} >> K_{2}

which is incorrect

Q. The equilibrium constants for the reactions are

H_{3} P O_{4}_{1} H^{+} + H_{2} P O_{4}^{-}; K_{1}

H_{2} P O_{4}^{-}_{2} H^{+} + H P O_{4}^{2 -}; K_{2}

H P O_{4}^{2 -}_{3} H^{+} + P O_{4}^{3 -}; K_{3}

The equilibrium constant for,

H_{3} P O_{4} ⇌ 3 H^{+} + P O_{4}^{3 -}

will be :

Q. For three reactions of first, second and third order,

k_{1} = k_{2} = k_{3}

, when concentration is expressed in

m o l / L

. What will be relation among

k_{1}, k_{2}

and

k_{3}

if the concentration is expressed in mol/

m L

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