Dissociation Constant of Weak Base given pKb Calculator

Formula Used:

\[ K_b = 10^{-pK_b} \]

Dissociation Constant of Weak Base (Kb):

Definition: The dissociation constant (Kb) measures the extent to which a weak base dissociates in water.

Purpose: It helps quantify the strength of a weak base in solution and predict its behavior in chemical reactions.

The calculator uses the formula:

\[ K_b = 10^{-pK_b} \]

Where:

Explanation: The pKb value is converted back to the Kb value using the inverse logarithmic relationship.

Details: Knowing Kb helps predict base strength, calculate pH of basic solutions, and understand equilibrium concentrations.

Tips: Enter the pKb value (must be ≥ 0). The calculator will output the Kb value in scientific notation.

Q1: What does a higher Kb value indicate?
A: A higher Kb means a stronger base that dissociates more completely in water.

Q2: What's the relationship between pKb and Kb?
A: pKb is the negative logarithm of Kb (pKb = -log10(Kb)).

Q3: What are typical Kb values for weak bases?
A: Weak bases typically have Kb values between 10^-2 and 10^-12.

Q4: How is Kb related to Ka?
A: For conjugate acid-base pairs, Ka × Kb = Kw (water ionization constant, 1.0×10^-14 at 25°C).

Q5: Why is Kb important in buffer solutions?
A: Kb helps calculate the pH of buffer solutions containing weak bases and their conjugate acids.