Degree of Dissociation Formula:
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Definition: The Degree of Dissociation is the extent of generating current carrying free ions, which are dissociated from the fraction of solute at a given concentration.
Purpose: It helps quantify how much a weak electrolyte dissociates into ions in solution.
The calculator uses the formula:
Where:
Explanation: The degree of dissociation is calculated as the square root of the ratio of the acid dissociation constant to the ionic concentration.
Details: Understanding the degree of dissociation is crucial for predicting the behavior of weak electrolytes in solution, including their conductivity and pH.
Tips: Enter the dissociation constant (Ka) of the weak acid and the ionic concentration (in mol/L). All values must be > 0.
Q1: What is the range for degree of dissociation?
A: For weak electrolytes, α typically ranges between 0 and 1, where 0 means no dissociation and 1 means complete dissociation.
Q2: How does concentration affect degree of dissociation?
A: For weak electrolytes, the degree of dissociation increases with dilution (lower concentration).
Q3: What's a typical Ka value for weak acids?
A: Weak acids typically have Ka values between 10^-2 and 10^-10. For example, acetic acid has Ka ≈ 1.8 × 10^-5.
Q4: Can this formula be used for strong electrolytes?
A: No, this formula is only valid for weak electrolytes. Strong electrolytes are considered completely dissociated (α ≈ 1).
Q5: What are the limitations of this calculation?
A: This is an approximation that becomes less accurate for higher concentrations or very weak electrolytes where other factors become significant.