Question

What is meant by the ionic product of water?
A) Concentration of hydrogen ions.
B) Concentration of hydroxyl ions.
C) The product of the concentration of hydrogen and hydroxyl ions.
D) None of these.

Answer 1

Hint: We know that water is a weak electrolyte and undergoes self-ionization to a little extent. The products of concentrations of hydrogen and hydroxyl ions in water at a specific temperature are understood as ionic products of water.

Complete step by step answer:
The self-ionization of water (the process during which water ionizes to hydronium ions and hydroxide ions) occurs to a really limited extent. When two molecules of water collide, there is often a transfer of a proton from one molecule to the opposite. The products are a charged hydronium ion and a charged hydroxyl ion.
\[{H_2}O(l) + {H_2}O(l) \rightleftarrows {H_3}{O^ + }(aq) + O{H^ - }(aq)\]
We often use the simplified sort of the reaction:
\[{H_2}O(l) \rightleftarrows {H^ + }(aq) + O{H^ - }(aq)\]
The constant for the self-ionization of water is mentioned because the ion-product for water is given the symbol\[{K_w}\].
${K_w} = \left[ {{H^ + }} \right]\left[ {O{H^ - }} \right]$
The ion-product of water is the product of the concentration of hydrogen ions and hydroxide ions.

So, the correct answer is Option C .

Note:
We must remember that the water isn't included within the ion-product expression because it's a pure liquid. The worth is extremely small, as compared with a reaction that favors the reactants. At, the experimentally determined value of pure water is \[1.0{\text{ }} \times {\text{ }}{10^{ - 14}}\]. In pure water, the concentrations of hydrogen and hydroxide ions are equal. Pure water or any other aqueous solution in which the ratio of hydrogen and hydroxyl ion holds is said to be neutral.