The pH scale is a crucial concept in chemistry, typically ranging from 0 to 14 at a temperature of 25 degrees Celsius and a maximum concentration of 1 molar. Understanding the relationship between pH and pOH is essential for analyzing acidity and basicity in solutions. The fundamental equation connecting these two measures is:

pH + pOH = 14

This equation allows for the conversion between pH and pOH values. To delve deeper, we can express pH in terms of hydrogen ion concentration, represented as [H⁺]. The formula is:

pH = -\log[H⁺]

From this, we can derive the concentration of hydrogen ions:

[H⁺] = 10^{-pH}

Similarly, pOH can be defined in relation to hydroxide ion concentration, [OH^-], using the equation:

pOH = -\log[OH^-]

Thus, the concentration of hydroxide ions can be calculated as:

[OH^-] = 10^{-pOH}

These equations collectively form a comprehensive framework for understanding the interplay between pH and pOH, reinforcing the principle that their sum always equals 14. This knowledge is vital for various applications in chemistry, biology, and environmental science.