QuestionJuly 14, 2025

[H_(3)O^+]=6.8times 10^-2M [OH^-]=square M This solution is (Choose one)

[H_(3)O^+]=6.8times 10^-2M [OH^-]=square M This solution is (Choose one)
[H_(3)O^+]=6.8times 10^-2M [OH^-]=square M This solution is (Choose one)

Solution
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Answer

Acidic Explanation 1. Calculate [OH^-] Use the formula for water dissociation constant: K_w = [H_3O^+][OH^-]. At 25°C, K_w = 1.0 \times 10^{-14}. Solve for [OH^-]: [OH^-] = \frac{K_w} H_3O^+ = \frac{1.0 \times 10^{-14}}{6.8 \times 10^{-2}}. 2. Determine solution type Compare [H_3O^+] and [OH^-]. If [H_3O^+] > [OH^-], the solution is acidic; if [H_3O^+] < [OH^-], it's basic; if equal, neutral.

Explanation

1. Calculate $[OH^-]$<br /> Use the formula for water dissociation constant: $K_w = [H_3O^+][OH^-]$. At 25°C, $K_w = 1.0 \times 10^{-14}$. Solve for $[OH^-]$: $[OH^-] = \frac{K_w}{[H_3O^+]} = \frac{1.0 \times 10^{-14}}{6.8 \times 10^{-2}}$.<br /><br />2. Determine solution type<br /> Compare $[H_3O^+]$ and $[OH^-]$. If $[H_3O^+] > [OH^-]$, the solution is acidic; if $[H_3O^+] < [OH^-]$, it's basic; if equal, neutral.
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