1. What is pH and pOH?

pH is a measure of hydrogen ion concentration, while pOH is a measure of hydroxide ion concentration. They are related through the equation: pH + pOH = 14 (at 25°C). Lower pH values indicate higher acidity, while lower pOH values indicate higher basicity.

2. How Does the Calculator Work?

The calculator uses these equations:

Where:

• \( [H^+] \) — Hydrogen ion concentration (mol/L)
• \( [OH^-] \) — Hydroxide ion concentration (mol/L)
• \( pH \) — Negative logarithm of hydrogen ion concentration
• \( pOH \) — Negative logarithm of hydroxide ion concentration

Explanation: The equations convert the logarithmic pH and pOH scales back to actual ion concentrations.

3. Importance of pH and pOH

Details: pH and pOH measurements are crucial in chemistry, biology, medicine, and environmental science. They affect chemical reactions, biological processes, and water quality.

4. Using the Calculator

Tips: Enter pH and pOH values between 0 and 14. The calculator will compute the corresponding ion concentrations in mol/L (molarity).

5. Frequently Asked Questions (FAQ)

Q1: What is the relationship between pH and pOH?
A: In aqueous solutions at 25°C, pH + pOH = 14. This relationship comes from the ion product of water (Kw = 1.0 × 10⁻¹⁴).

Q2: What are neutral pH and pOH values?
A: At 25°C, neutral solutions have pH = 7 and pOH = 7, where [H+] = [OH-] = 1.0 × 10⁻⁷ M.

Q3: How does temperature affect pH and pOH?
A: The neutral point changes with temperature (e.g., pH 6.8 at 37°C). The pH + pOH relationship remains but the sum changes with Kw.

Q4: Can I calculate [H+] if I only know [OH-]?
A: Yes, using Kw = [H+][OH-] = 1.0 × 10⁻¹⁴ at 25°C. [H+] = Kw/[OH-].

Q5: Why use logarithmic scales for acidity/basicity?
A: The logarithmic scale compresses the wide range of possible ion concentrations (10⁻¹⁴ to 1 M) into a more manageable 0-14 scale.