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pH Formula for Strong Acids:
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pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. It ranges from 0 (very acidic) to 14 (very basic), with 7 being neutral.
The calculator uses the pH formula for strong acids:
Where:
Explanation: The formula calculates pH by taking the negative logarithm of the hydrogen ion concentration. For strong acids that completely dissociate, this provides an accurate pH measurement.
Details: Accurate pH calculation is essential in chemistry, biology, environmental science, and industrial processes. It helps determine solution acidity, predict chemical behavior, and maintain optimal conditions in biological systems.
Tips: Enter hydrogen ion concentration in mol/L (molarity). The value must be greater than 0. For strong acids, this equals the acid concentration; for weak acids, additional calculations are needed.
Q1: What is the difference between strong and weak acids?
A: Strong acids completely dissociate in water, while weak acids only partially dissociate. This calculator is designed for strong acids.
Q2: What are typical pH values for common substances?
A: Battery acid: ~0.5, Lemon juice: ~2.0, Pure water: 7.0, Baking soda: ~8.3, Ammonia: ~11.0.
Q3: How do I calculate pH for weak acids?
A: For weak acids, you need the acid dissociation constant (Ka) and use the formula: pH = -log(√(Ka × C)), where C is the concentration.
Q4: What is the relationship between [H⁺] and pH?
A: As [H⁺] increases by a factor of 10, pH decreases by 1 unit. This inverse logarithmic relationship means small concentration changes can cause significant pH changes.
Q5: When is this calculation not accurate?
A: This calculation assumes ideal conditions, temperature of 25°C, and complete dissociation. It may be less accurate for very concentrated solutions or at extreme temperatures.