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Henry's Law with Common Ion Adjustment:
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Henry's Law with Common Ion Adjustment describes the solubility of a gas in a solution containing a common ion. It states that the concentration of a dissolved gas is proportional to its partial pressure above the solution, adjusted for the presence of common ions that may affect solubility.
The calculator uses the Henry's Law equation:
Where:
Explanation: The equation calculates the solubility of a gas in a solution, accounting for the common ion effect that may reduce gas solubility.
Details: Accurate gas solubility calculation is crucial for understanding gas absorption processes, environmental studies, industrial applications, and predicting the behavior of gases in various solutions.
Tips: Enter Henry's constant in atm/M and pressure in atm. All values must be valid (K_H > 0, P > 0).
Q1: What is Henry's constant?
A: Henry's constant (K_H) is a measure of the solubility of a gas in a liquid. It represents the ratio of the partial pressure of the gas above the solution to its concentration in the solution.
Q2: How does common ion affect gas solubility?
A: The presence of a common ion in the solution can decrease the solubility of a gas due to the common ion effect, which shifts the equilibrium and reduces the amount of gas that can dissolve.
Q3: What units are used for Henry's constant?
A: Henry's constant is typically expressed in atm/M (atmospheres per molar concentration) for gas solubility calculations.
Q4: When is this calculation most applicable?
A: This calculation is particularly useful in chemistry and environmental science for predicting gas behavior in solutions containing ions that may affect solubility.
Q5: Are there limitations to this equation?
A: The equation assumes ideal behavior and may be less accurate at very high pressures or concentrations, or in solutions with significant ionic strength effects.