Which of the following relations is correct f | vedclass

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(B) In an aqueous solution at $25^{\circ}C$,the product of the concentrations of hydronium ions and hydroxide ions is constant,given by $[H_3O^+][OH^-

Vedclass · Accepted Answer

$[OH^-] > 10^{-7} \; M$

Vedclass · Answer

(B) In an aqueous solution at $25^{\circ}C$,the product of the concentrations of hydronium ions and hydroxide ions is constant,given by $[H_3O^+][OH^-] = 10^{-14}$.For a neutral solution,$[H_3O^+] = [OH^-] = 10^{-7} \; M$.For a basic solution,the concentration of hydroxide ions is greater than the concentration of hydronium ions,meaning $[OH^-] > [H_3O^+]$.Since $[H_3O^+][OH^-] = 10^{-14}$,if $[OH^-] > 10^{-7} \; M$,then $[H_3O^+] Therefore,for a basic solution,the correct relation is $[OH^-] > 10^{-7} \; M$.

Which of the following relations is correct for a basic aqueous solution?

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