`NH_(4)CN` is a salt of weak acid `HCN(K_(a)=6.2xx10^(-10))` and a weak base `NH_(4)OH(K_(b)=1.8xx10^(-5))`. 1 molar solution of `NH_(4)CN` will be :-

Options

A. neutral
B. strongly acidic
C. strongly basic
D. weakly basic.

Explanation

To determine the nature of a 1 molar solution of `NH₄CN`, we need to analyze the properties of the salt formed from a weak acid and a weak base. Here’s a step-by-step solution:

### Step 1: Identify the components of the salt
`NH₄CN` is formed from the weak acid `HCN` and the weak base `NH₄OH`.

### Step 2: Write down the equilibrium constants
We are given:
- The dissociation constant for the weak acid `HCN` (Ka) is \( 6.2 \times 10^{-10} \).
- The dissociation constant for the weak base `NH₄OH` (Kb) is \( 1.8 \times 10^{-5} \).

### Step 3: Compare Ka and Kb
To determine whether the solution of `NH₄CN` is acidic, basic, or neutral, we compare the values of Ka and Kb:
- If \( K_a > K_b \), the solution is acidic.
- If \( K_a < K_b \), the solution is basic.
- If \( K_a = K_b \), the solution is neutral.

Here, we see that:
- \( K_b (1.8 \times 10^{-5}) > K_a (6.2 \times 10^{-10}) \)

### Step 4: Conclusion
Since \( K_b \) is greater than \( K_a \), the solution of `NH₄CN` will be weakly basic.

### Final Answer
A 1 molar solution of `NH₄CN` will be weakly basic.

---