The equilibrium constant for the reaction H3 PO4 ⇌H^++H2 PO4^-is K1, for reaction H2 PO4 ⇄H^++HP

step 1 Here in this question you need to find the value of equilibrium constant k for the reaction H3 P

The equilibrium constant for the reaction H3 PO4 ⇌H^++H2...

The equilibrium constant for the reaction $\mathrm{H}_3 \mathrm{PO}_4 \rightleftharpoons \mathrm{H}^{+}+\mathrm{H}_2 \mathrm{PO}_4^{-}$is $\mathrm{K}_1$, for reaction $\mathrm{H}_2 \mathrm{PO}_4 \rightleftarrows \mathrm{H}^{+}+\mathrm{HPO}_4{ }^{2-}$ is $\mathrm{K}_2$ and for reaction $\mathrm{HPO}_4{ }^{2-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{PO}_4{ }^{3-}$ is $\mathrm{K}_3$. The equilibrium constant ( K ) for $\mathrm{H}_3 \mathrm{PO}_4 \rightleftarrows 3 \mathrm{H}^{+}+\mathrm{PO}_4{ }^{3-}$ will be (a) $\mathrm{K}_1, \times \mathrm{K}_2 \times \mathrm{K}_3$ (b) $\mathrm{K}_1 / \mathrm{K}_2 \mathrm{~K}_3$ (c) $\mathrm{K}_2 / \mathrm{K}_1 \mathrm{~K}_3$ (d) $\mathrm{K}_1,+\mathrm{K}_2+\mathrm{K}_3$

The equilibrium constant for the reaction
$\mathrm{H}_3 \mathrm{PO}_4 \rightleftharpoons \mathrm{H}^{+}+\mathrm{H}_2 \mathrm{PO}_4^{-}$is $\mathrm{K}_1$,
for reaction $\mathrm{H}_2 \mathrm{PO}_4 \rightleftarrows \mathrm{H}^{+}+\mathrm{HPO}_4{ }^{2-}$ is $\mathrm{K}_2$ and
for reaction $\mathrm{HPO}_4{ }^{2-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{PO}_4{ }^{3-}$ is $\mathrm{K}_3$.
The equilibrium constant ( K ) for
$\mathrm{H}_3 \mathrm{PO}_4 \rightleftarrows 3 \mathrm{H}^{+}+\mathrm{PO}_4{ }^{3-}$ will be
(a) $\mathrm{K}_1, \times \mathrm{K}_2 \times \mathrm{K}_3$
(b) $\mathrm{K}_1 / \mathrm{K}_2 \mathrm{~K}_3$
(c) $\mathrm{K}_2 / \mathrm{K}_1 \mathrm{~K}_3$
(d) $\mathrm{K}_1,+\mathrm{K}_2+\mathrm{K}_3$

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Key Concepts

Equilibrium Constant

The equilibrium constant is a numerical value that expresses the ratio of the concentrations (or pressures) of products to reactants for a reaction at equilibrium, each raised to the power of their stoichiometric coefficients. It provides insight into the position of the equilibrium and the extent to which a reaction proceeds in either direction.

Acid Dissociation Constant (Ka)

An acid dissociation constant quantifies the degree to which an acid donates its proton in water, resulting in a reversible reaction that establishes an equilibrium between the undissociated acid and its ionized forms. Each step in a polyprotic acid's dissociation has its own equilibrium constant, reflecting the sequential loss of protons.

Multiplicative Combination of Equilibrium Constants

When a reaction proceeds through a series of sequential, independent steps, the overall equilibrium constant for the overall reaction is the product of the equilibrium constants for each individual step. This principle allows one to relate the stepwise dissociation constants of a polyprotic acid to the equilibrium constant of its overall dissociation reaction.

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