Precise Acidic Solution Analysis
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Strong acids (like HCl, HNO₃, H₂SO₄) completely dissociate in water, releasing H⁺ ions. The pOH is calculated from pH using the relationship pOH = 14 - pH, where pH = -log[H⁺]. Higher acid concentration means lower pOH values.
Weak acids (like acetic acid, citric acid) only partially dissociate in water. Their dissociation is governed by an equilibrium constant Ka. The [H⁺] concentration is calculated using the formula [H⁺] = √(Ka × concentration), which is then used to find pH and pOH.
When multiple acids are present in solution, each contributes to the total [H⁺] concentration. This calculator determines the combined effect of two acids on solution pOH by summing their individual [H⁺] contributions and then calculating pOH = 14 - pH.
Key concepts in acid chemistry:
Classification and properties:
Practical uses of pOH calculations:
For deeper understanding:
Important factors in real-world applications:
pH = -log[H⁺]
pOH = 14 - pH
[H⁺] = n × Ca
Where n is the number of acidic hydrogens and Ca is acid concentration
Ka = [H⁺][A⁻]/[HA]
[H⁺] = √(Ka×Ca)
α = [H⁺]/Ca
Where Ka is the acid dissociation constant and α is the degree of dissociation
pH = -log(Σ[H⁺])
Total [H⁺] = Σ[H⁺]ᵢ
pOH = 14 - pH
Where Σ[H⁺]ᵢ is the sum of hydrogen ion concentrations from all acids