Equilibrium constant for two complexes are `A: K_4[Fe(CN)_6]2.6xx10^(37)` (for dissociation) B : `K_3[Fe(CN)_6]1.9xx10^(17)` (for dissociation)

Options

A. A and B are equally stable
B. A is more stable than B
C. B is more stable than A
D. the predictable stability

Answer

To determine the stability of the two complexes based on their equilibrium constants for dissociation, we can follow these steps:

### Step 1: Understand the Equilibrium Constant
The equilibrium constant (K) for dissociation indicates how readily a complex dissociates into its components. A higher value of K means that the complex dissociates more readily, while a lower value indicates that the complex is more stable and less likely to dissociate.

### Step 2: Write Down the Given Values
- For complex A: \( K_{4}[Fe(CN)_{6}] = 2.6 \times 10^{37} \)
- For complex B: \( K_{3}[Fe(CN)_{6}] = 1.9 \times 10^{17} \)

### Step 3: Compare the Equilibrium Constants
Now, we compare the two equilibrium constants:
- \( K_A = 2.6 \times 10^{37} \)
- \( K_B = 1.9 \times 10^{17} \)

### Step 4: Analyze the Values
Since \( K_A \) is significantly larger than \( K_B \), this indicates that complex A dissociates more readily than complex B.

### Step 5: Determine Stability
Since stability is inversely related to the equilibrium constant for dissociation:
- A lower equilibrium constant (like that of complex B) indicates greater stability.
- A higher equilibrium constant (like that of complex A) indicates lower stability.

### Conclusion
Therefore, complex B is more stable than complex A.

### Final Answer
Complex B is more stable than complex A.

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