When `15mL` of `0.05M AgNO_(3)` is mixed with `45.0mL` of `0.03M K_(2)CrO_(4)`, predict whether precipitation of `Ag_(2)CrO_(4)` occurs or not? `K_(sp)` of `Ag_(2)CrO_(4) = 1.9 xx 10^(-12)`

Explanation

To determine whether precipitation of silver chromate (Ag₂CrO₄) occurs when 15 mL of 0.05 M AgNO₃ is mixed with 45 mL of 0.03 M K₂CrO₄, we can follow these steps:

### Step 1: Calculate the final concentrations of Ag⁺ and CrO₄²⁻ ions
1. **Calculate the total volume of the solution:**
\[ V_{\text{total}} = V_{\text{AgNO}_3} + V_{\text{K}_2\text{CrO}_4} = 15\, \text{mL} + 45\, \text{mL} = 60\, \text{mL} \]

...