Enter your Base Concentration, Number of OH⁻ ions (n), and Temperature into the Strong Base pH Calculator to find the pH of your solution, plus the pOH, [OH⁻] concentration, and [H⁺] concentration — because strong bases deserve a full breakdown, not just a number.
pH
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pOH
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[OH⁻] Concentration
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[H⁺] Concentration
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A strong base completely dissociates in water, releasing all available OH⁻ ions. Examples include NaOH, KOH, and Ba(OH)₂. Unlike weak bases, strong bases don't require equilibrium calculations.
For strong bases: [OH⁻] = n × C (where n is stoichiometry and C is concentration), then pOH = -log[OH⁻], and pH = 14 - pOH at 25°C.
Temperature changes the water ionization constant (Kw). At 25°C, Kw = 1×10⁻¹⁴, but it increases with temperature, affecting the pH + pOH = 14 relationship.
The stoichiometry number indicates how many OH⁻ ions each molecule of base releases. For example, NaOH has n=1, while Ba(OH)₂ has n=2.
Strong bases typically have pH values above 7, often ranging from 10-14 depending on concentration. Higher concentrations result in higher pH values.
Yes, in very concentrated strong base solutions, pH can exceed 14. The pH scale isn't limited to 0-14, though this range covers most common aqueous solutions.
At 25°C, pH + pOH = 14 (due to Kw = 1×10⁻¹⁴). For bases with high pH, the pOH will be correspondingly low, and vice versa.