Which factor will shift the following equilibrium in forward direction ?
`AgCl(s) rarr Ag^(+)(aq) + Cl^(-)(aq)`

Options

A. Addition of `NH_(3)(aq)`
B. Addition of `AgNO_(3)(aq)`
C. Addition of NaCl(aq)
D. Addition of AgCl(s)

Explanation

To determine which factor will shift the equilibrium of the reaction

\[ \text{AgCl(s)} \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) \]

in the forward direction, we can apply Le Chatelier's principle. This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.

### Step-by-Step Solution:

1. **Identify the Reaction Components**:
The reaction involves a solid (AgCl) dissociating into its ions (Ag⁺ and Cl⁻).

2. **Understand the Principle**:
According to Le Chatelier's principle, increasing the concentration of reactants or removing products will shift the equilibrium to the right (forward direction).

3. **Analyze the Options**:
- **Option A: Addition of NH₃**: This does not directly affect the concentration of AgCl, Ag⁺, or Cl⁻, so it may not shift the equilibrium.
- **Option B: Addition of AgNO₃**: This introduces Ag⁺ ions into the solution, which could shift the equilibrium to the left (backward direction) as it increases the product concentration.
- **Option C: Addition of NaCl**: This increases the concentration of Cl⁻ ions, which could also shift the equilibrium to the left.
- **Option D: Addition of AgCl**: This increases the amount of the solid reactant (AgCl), which will shift the equilibrium to the right (forward direction) according to Le Chatelier's principle.

4. **Conclusion**:
The factor that will shift the equilibrium in the forward direction is the addition of AgCl (Option D).

### Final Answer:
The addition of AgCl will shift the equilibrium in the forward direction.

---