To `Ag_(2)CrO_(4)` solution over its own percipitate `CrO_(4)^(2-)` ions are added . This results in

Options

A. increase in `Ag^(+)` concentration
B. decrease in `Ag^(+)` concentration
C. increase in solubiity product
D. Shifting of `Ag^(+) ` ions from the precipitate into the solution

Answer

To solve the question regarding the addition of chromate ions to a solution of silver chromate over its own precipitate, we can follow these steps:

### Step 1: Understand the System
Silver chromate (Ag₂CrO₄) is a sparingly soluble salt that dissociates in water to form silver ions (Ag⁺) and chromate ions (CrO₄²⁻). The equilibrium can be represented as:

\[ \text{Ag}_2\text{CrO}_4 (s) \rightleftharpoons 2 \text{Ag}^+ (aq) + \text{CrO}_4^{2-} (aq) \]

### Step 2: Add Chromate Ions
When additional chromate ions (CrO₄²⁻) are added to the solution, according to Le Chatelier's principle, the equilibrium will shift to counteract the change. The system will try to reduce the concentration of CrO₄²⁻ ions by forming more solid silver chromate.

### Step 3: Effect on Silver Ion Concentration
As the equilibrium shifts to the left to form more solid Ag₂CrO₄, the concentration of silver ions (Ag⁺) in the solution will decrease. This is because some of the Ag⁺ ions will react with the added CrO₄²⁻ ions to form more precipitate:

\[ 2 \text{Ag}^+ (aq) + \text{CrO}_4^{2-} (aq) \rightarrow \text{Ag}_2\text{CrO}_4 (s) \]

### Conclusion
Thus, the addition of CrO₄²⁻ ions to the silver chromate solution results in a decrease in the concentration of Ag⁺ ions in the solution due to the formation of more precipitate.

### Final Answer
The addition of CrO₄²⁻ ions over the precipitate of Ag₂CrO₄ results in a decrease in the concentration of Ag⁺ ions.

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