What happens to the pH of a basic aqueous sol | vedclass

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(B) The $pH$ scale is defined as $pH = -\log[H^+]$.In an aqueous solution,the product of the concentrations of hydrogen ions and hydroxide ions is con

Vedclass · Accepted Answer

It increases.

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(B) The $pH$ scale is defined as $pH = -\log[H^+]$.In an aqueous solution,the product of the concentrations of hydrogen ions and hydroxide ions is constant at a given temperature,represented by the ionic product of water: $[H^+][OH^-] = K_w = 10^{-14}$.If the concentration of $[OH^-]$ increases,the concentration of $[H^+]$ must decrease to maintain the constant value of $K_w$.Since $pH$ is inversely proportional to the concentration of $[H^+]$ (specifically,$pH = 14 + \log[OH^-]$),a decrease in $[H^+]$ concentration leads to an increase in the $pH$ value.Therefore,as the basicity of the solution increases due to higher $[OH^-]$ concentration,the $pH$ value increases.

What happens to the $pH$ of a basic aqueous solution if the concentration of $[OH^-]$ ions increases?

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