Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M

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Identify the given concentration: \([H^+] = 2.5 \times 10^{-10} \text{ M}\).

Use the relationship between \([H^+]\) and \([OH^-]\) in water: \([H^+][OH^-] = 1.0 \times 10^{-14}\).

Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{1.0 \times 10^{-14}}{[H^+]}\).

Substitute the given \([H^+]\) value into the equation to find \([OH^-]\).

Determine if the solution is acidic, basic, or neutral by comparing \([H^+]\) and \([OH^-]\): if \([H^+] > [OH^-]\), it's acidic; if \([H^+] < [OH^-]\), it's basic; if \([H^+] = [OH^-]\), it's neutral.

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주요 개념

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pH and pOH

pH is a measure of the hydrogen ion concentration in a solution, while pOH measures the hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. Understanding this relationship is crucial for determining the acidity or basicity of a solution.

Acidic, Basic, and Neutral Solutions

A solution is considered acidic if its pH is less than 7, basic if its pH is greater than 7, and neutral if its pH is exactly 7. The concentration of hydrogen ions (H+) and hydroxide ions (OH-) determines these classifications. For example, a higher concentration of H+ indicates acidity, while a higher concentration of OH- indicates basicity.

Calculating pOH from H+ Concentration

To find the pOH from the concentration of hydrogen ions (H+), first calculate the pH using the formula pH = -log[H+]. Then, use the relationship pOH = 14 - pH to find the pOH. This calculation is essential for determining the nature of the solution based on its hydroxide ion concentration.