Physical and chemical equilibrium can respond to a change in their pressure, temperature, and concentration of reactants and products. To describe the change in the equilibrium we have a principle named Le Chatelier principle. According to this principle, even if we make some changes in equilibrium, then also the system even re-establishes the equilibrium by undoing the effect.
If we add `SO_(4)^(2-)` ion to a saturated solution of `Ag_(2)SO_(4)`, it will result in a//an

Options

A. Result in an increase in `Ag^(o+)` concentration
B. Result in a decrease in `Ag^(o+)` concentration
C. Shift `Ag^(o+)` ions from solid `Ag_(2)CrO_(4)` into solution.
D. Result in a decrease the `CrO_(4)^(2-)` ion concentration in the solution.

Explanation

To solve the question regarding the effect of adding `SO₄²⁻` ions to a saturated solution of `Ag₂SO₄`, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Equilibrium Reaction**:
The dissociation of silver sulfate (`Ag₂SO₄`) in water can be represented as follows:
\[ \text{Ag}_2\text{SO}_4 (s) \rightleftharpoons 2 \text{Ag}^+ (aq) + \text{SO}_4^{2-} (aq) \]
Here, solid silver sulfate dissociates into two moles of silver ions and one mole of sulfate ions.

2. **Applying Le Chatelier's Principle**:
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change (in this case, an increase in the concentration of sulfate ions), the system will respond by shifting the equilibrium position to counteract that change.

3. **Effect of Adding `SO₄²⁻` Ions**:
When we add `SO₄²⁻` ions to the saturated solution, we are increasing the concentration of one of the products (sulfate ions). The system will respond by shifting the equilibrium to the left to reduce the concentration of sulfate ions.

4. **Resulting Changes in Ion Concentrations**:
As the equilibrium shifts to the left, some of the `Ag⁺` ions will combine with the added `SO₄²⁻` ions to form more solid `Ag₂SO₄`. This will result in a decrease in the concentration of silver ions (`Ag⁺`) in the solution.

5. **Conclusion**:
Therefore, the correct answer to the question is that adding `SO₄²⁻` ions to the saturated solution of `Ag₂SO₄` will result in a **decrease in silver ion concentration**.

### Final Answer:
The correct option is: **Result in a decrease in silver ion concentration**.

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