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The pH is calculated using the formula:

\( pH = -\log{[H_{3}O^+]} \)

When you have a pH value, you can easily determine the \[H_{3}O^+\] concentration by rearranging the equation:

\[ [H_{3}O^+] = 10^{-pH} \]

• If a solution has a high \[H_{3}O^+\] concentration, it means the solution is more acidic.
• Given a pH of -1, the \[H_{3}O^+\] concentration in our example turns out to be 10 moles/L, reflecting very high acidity.

To find the \[OH^-\] concentration, we use the relationship between \[H_{3}O^+\] and \[OH^-\] concentrations which is governed by the ion product of water (\(K_w\)):

\[ K_w = [H_{3}O^+][OH^-] \]

For pure water at 25掳C, \(K_w\) is constant, equal to \(1 \times 10^{-14}\). This means we can explore how acid and base concentrations are inversely related:

\[ [OH^-] = \frac{K_w}{[H_{3}O^+]} \]

• Substituting values allows calculation: \([OH^-] = \frac{1 \times 10^{-14}}{10}\), resulting in \([OH^-] = 1 \times 10^{-15} \) moles/L.
• A low \[OH^-\] concentration alongside a high \[H_{3}O^+\] concentration reinforces the acidity of the solution.

• If \[H_{3}O^+\] concentration is greater than \[OH^-\], the solution is acidic.
• If \[OH^-\] concentration exceeds \[H_{3}O^+\], the solution is basic.

From the provided example, where \[H_{3}O^+\] concentration is 10 moles/L and \[OH^-\] concentration is \(1 \times 10^{-15}\) moles/L, it's evident that:

• The solution has significantly more hydronium ions than hydroxide ions.
• This results in an acidic solution, confirming the direct impact of these ion concentrations on the nature of the solution.

Thus, understanding these ion concentrations helps classify a solution and predict its behavior in chemical reactions.