Which of the following statements is true for | vedclass

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(B) $1$. In an aqueous solution, the product of $[H_3O^+]$ and $[OH^-]$ is constant at a given temperature $(K_w = [H_3O^+][OH^-])$.$2$. $A$ solution

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In a basic solution, there is an excess of $[OH^-]$ ions.

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(B) $1$. In an aqueous solution, the product of $[H_3O^+]$ and $[OH^-]$ is constant at a given temperature $(K_w = [H_3O^+][OH^-])$.$2$. $A$ solution is basic if the concentration of hydroxide ions is greater than the concentration of hydronium ions, i.e., $[OH^-] > [H_3O^+]$.$3$. Therefore, a basic solution contains an excess of $[OH^-]$ ions.$4$. Option $(A)$ is true for neutral solutions. Option $(C)$ is true for acidic solutions. Option $(D)$ is incorrect because $pOH = -\log[OH^-]$.

Which of the following statements is true for a basic solution?

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