Calculate,
(i) Dissociation constant of conjugate base of `HF`, `K_a=6.8xx10^(-4)`
(ii) Dissociation constant of conjugate acid of `CO_3^(2-), K_b=2.1xx10^(-4)`

Explanation

To solve the problem, we will calculate the dissociation constants for the conjugate base of HF and the conjugate acid of CO₃²⁻ using the relationship between the dissociation constants of acids and their conjugate bases.

### Given:
1. For HF: \( K_a = 6.8 \times 10^{-4} \)
2. For CO₃²⁻: \( K_b = 2.1 \times 10^{-4} \)
3. \( K_w = 1.0 \times 10^{-14} \) (the ion product of water)

### (i) Calculate the dissociation constant of the conjugate base of HF (K_b):
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