If we add `SO_(4)^(2-)` ion to a saturated solution of `Ag_(2)SO_(4)`, it will result in a//an

Options

A. Increase in `Ag^(o+)` concentration.
B. Decrease in `Ag^(o+)` concentration
C. It will shift `Ag^(o+)` ions from solid `Ag_(2)SO_(4)` into solution.
D. It will decrease the `SO_(4)^(2-)` ion concentration in the solution.

Answer

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

### Step 1: Understand the Saturated Solution
A saturated solution of `Ag₂SO₄` contains the solid `Ag₂SO₄` in equilibrium with its dissociated ions in solution:
\[ \text{Ag}_2\text{SO}_4 (s) \rightleftharpoons 2 \text{Ag}^+ (aq) + \text{SO}_4^{2-} (aq) \]

### Step 2: Write the Expression for Ksp
The solubility product constant (Ksp) for this equilibrium can be expressed as:
\[ K_{sp} = [\text{Ag}^+]^2 [\text{SO}_4^{2-}] \]
where \([\text{Ag}^+]\) is the concentration of silver ions and \([\text{SO}_4^{2-}]\) is the concentration of sulfate ions in the solution.

### Step 3: Effect of Adding `SO₄²⁻` Ions
When additional `SO₄²⁻` ions are added to the saturated solution, the concentration of sulfate ions \([\text{SO}_4^{2-}]\) increases. According to Le Chatelier's principle, if we increase the concentration of one of the products (in this case, `SO₄²⁻`), the equilibrium will shift to the left to counteract this change.

### Step 4: Resulting Changes in Ion Concentration
As the equilibrium shifts to the left, more `Ag₂SO₄` will form from the ions, which means the concentration of silver ions \([\text{Ag}^+]\) will decrease. This is because the system is trying to reduce the effect of the added sulfate ions by consuming them and producing more solid `Ag₂SO₄`.

### Step 5: Conclusion
Therefore, the addition of `SO₄²⁻` ions to a saturated solution of `Ag₂SO₄` will result in a decrease in the concentration of `Ag^+` ions in the solution.

### Final Answer
The correct answer is that the concentration of `Ag^+` ions will **decrease**.

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