Hypobromous acid (Ka = 2.8 × 10⁻⁹) and hydrocyanic acid (Ka = 4.9 × 10⁻¹⁰) are both weak acids. Determine if reactants or products are favored in the following reaction.
HBrO (aq) + CN⁻ (aq) ⇌ BrO⁻ (aq) + HCN (aq)

• A. Reactants
• B. Products
• C. Both directions are favored equally
• D. Neither direction is favored

Answer: (B)

Verified step by step guidance

1. Identify the relationship between the base dissociation constant (Kb) and the acid dissociation constant (Ka) for a conjugate acid-base pair. This relationship is given by the equation: \( K_w = K_a \times K_b \), where \( K_w \) is the ion-product constant of water, typically \( 1.0 \times 10^{-14} \) at 25°C.
2. Rearrange the equation to solve for the acid dissociation constant \( K_a \): \( K_a = \frac{K_w}{K_b} \).
3. Substitute the given values into the equation: \( K_a = \frac{1.0 \times 10^{-14}}{1.76 \times 10^{-5}} \).
4. Perform the division to calculate \( K_a \). This will give you the acid dissociation constant of the conjugate acid of NH3.
5. Compare the calculated \( K_a \) value with the provided options to determine the correct answer.