For[H3PO4], H3PO4↔H2PO4-+H+(K1)H2PO4-↔HPO42-+H+(K2)HPO42-↔PO43-+H+(K3), then

# For$\left[{H}_{3}P{O}_{4}\right]$, ${H}_{3}P{O}_{4}↔{H}_{2}P{{O}_{4}}^{-}+{H}^{+}\left({K}_{1}\right)$${H}_{2}P{{O}_{4}}^{-}↔HP{{O}_{4}}^{2-}+{H}^{+}\left({K}_{2}\right)$$HP{{O}_{4}}^{2-}↔P{{O}_{4}}^{3-}+{H}^{+}\left({K}_{3}\right)$, then

1. A

${K}_{1}>{K}_{2}>{K}_{3}$

2. B

${K}_{1}<{K}_{2}<{K}_{3}$

3. C

${K}_{1}<{K}_{2}>{K}_{3}$

4. D

${K}_{1}.{K}_{2}.{K}_{3}={K}_{W}$

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### Solution:

It is given to find the correct relation between K values for given reactions.
${K}_{1}=\frac{\left[{H}_{2}P{{O}_{4}}^{-}\right]\left[{H}^{+}\right]}{\left[{H}_{3}P{O}_{4}\right]}$

${K}_{2}=\frac{\left[HP{{O}_{4}}^{2-}\right]\left[{H}^{+}\right]}{\left[{H}_{2}P{{O}_{4}}^{-}\right]}$
${K}_{3}=\frac{\left[P{{O}_{4}}^{3-}\right]\left[{H}^{+}\right]}{\left[HP{{O}_{4}}^{2-}\right]}$
K values depend on a greater number of protons.
Hence, the correct answer is option (A) ${K}_{1}>{K}_{2}>{K}_{3}$.

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