Acid-base equilibrium reaction between [tex]{\text{Cl}}{{\text{O}}^ - }[/tex] and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] is as follows:
[tex]\boxed{{\text{Cl}}{{\text{O}}^ - } + {{\text{H}}_{\text{2}}}{\text{O}} \to {\text{HOCl}} + {\text{O}}{{\text{H}}^ - }}[/tex]
Further Explanation:
Equilibrium is the state at which concentration of reactants and products do not change with time and becomes constant. At this condition, the rate of forward reaction becomes equal to that of backward reaction.
Consider a general equilibrium reaction as follows:
[tex]{\text{A}} + {\text{B}} \rightleftharpoons {\text{X}} + {\text{Y}}[/tex]
Where,
A and B are reactants.
X and Y are products.
In this reaction, sign of equilibrium indicates that the rate of forward reaction is equal to the rate of backward reaction. In other words, formation of X and Y is balanced by the consumption of A and B.
[tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] isamphoteric in nature that indicates it can act as both acid and base. As an acid, it can donate hydrogen ions in solutions whereas it can accept hydrogen ions due to presence of lone pair on it and acts like a base. But [tex]{\mathbf{Cl}}{{\mathbf{O}}^{\mathbf{ - }}}[/tex] is a weak base so [tex]{{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}[/tex] acts as an acid when reacted with [tex]{\text{Cl}}{{\text{O}}^ - }[/tex]. [tex]{\text{Cl}}{{\text{O}}^ - }[/tex] accepts hydrogen ions donated by molecule to form HOCl and as a result, [tex]{\text{O}}{{\text{H}}^ - }[/tex] is also formed.
Acid-base equilibrium reaction between [tex]{\text{Cl}}{{\text{O}}^ - }[/tex] and [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] is as follows:
[tex]{\text{Cl}}{{\text{O}}^ - } + {{\text{H}}_{\text{2}}}{\text{O}} \to {\text{HOCl}} + {\text{O}}{{\text{H}}^ - }[/tex]
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Equilibrium
Keywords: equilibrium, reactants, products, A, B, X, Y, concentration, forward reaction, backward reaction, HOCl, OH-, H2O, ClO-.
