Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M

Verified step by step guidance

1. Identify the given concentration: \([H^+] = 0.0505\, \text{M}\).
2. Use the relationship between \([H^+]\) and \([OH^-]\) in water: \([H^+][OH^-] = 1.0 \times 10^{-14}\, \text{at 25°C}\).
3. Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{1.0 \times 10^{-14}}{[H^+]}\).
4. Substitute the given \([H^+]\) value into the equation: \([OH^-] = \frac{1.0 \times 10^{-14}}{0.0505}\, \text{M}\).
5. Determine if the solution is acidic, basic, or neutral by comparing \([H^+]\) and \([OH^-]\): If \([H^+] > [OH^-]\), the solution is acidic; if \([H^+] < [OH^-]\), it is basic; if \([H^+] = [OH^-]\), it is neutral.

Key Concepts

pH and pOH

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. The pOH is similarly a measure of hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. Understanding these concepts is essential for determining the nature 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-) in a solution determines its classification. For example, a higher concentration of H+ indicates acidity, while a higher concentration of OH- indicates basicity.

Calculating pOH from pH

To find the pOH from a given concentration of H+, one first calculates the pH using the formula pH = -log[H+]. Once the pH is determined, pOH can be calculated using the relationship pOH = 14 - pH. This calculation is crucial for determining the hydroxide ion concentration and the overall nature of the solution.