Strong Acid Molarity Formula:
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The molarity from pH calculation determines the concentration of hydrogen ions (H⁺) in a solution based on its pH value. For strong acids that completely dissociate in water, this directly gives the acid's molar concentration.
The calculator uses the formula:
Where:
Explanation: The pH scale is logarithmic, so each whole pH value below 7 is ten times more acidic than the next higher value. For strong acids, the molarity equals the hydrogen ion concentration.
Details: Converting pH to molarity is essential for preparing solutions with precise concentrations, chemical reactions, and understanding acid strength in laboratory and industrial settings.
Tips: Enter the pH value (typically between 0-14 for aqueous solutions). The calculator will output the molarity in both decimal and scientific notation.
Q1: Does this work for all acids?
A: No, this calculation is only accurate for strong acids that completely dissociate. Weak acids require additional information about their dissociation constant (Ka).
Q2: What's the relationship between pH and molarity?
A: pH is the negative base-10 logarithm of the hydrogen ion molarity: pH = -log[H⁺]. For strong acids, [H⁺] equals the acid's molarity.
Q3: What are common strong acids?
A: Hydrochloric acid (HCl), sulfuric acid (H₂SO₄), nitric acid (HNO₃), and perchloric acid (HClO₄) are common strong acids.
Q4: Why is scientific notation often used?
A: Because pH values produce very small numbers (e.g., pH 3 = 0.001 M), scientific notation makes them easier to read and compare.
Q5: How accurate is this calculation?
A: The calculation is mathematically precise, but actual solution concentrations may vary due to measurement errors or incomplete dissociation.