Final answer:
To find the equilibrium concentrations of ionic species when silver nitrate reacts with potassium chromate, one must calculate the initial concentrations and then apply the solubility product constant (Ksp) expression, taking into account the stoichiometry of the reaction.
Step-by-step explanation:
The question involves determining the equilibrium concentrations of ionic species when silver nitrate is mixed with potassium chromate. This is a solubility equilibrium problem that requires the use of the solubility product constant (Ksp).
To solve this, we start by writing out the chemical equation for the reaction of AgNO3 and K2CrO4 to form Ag2CrO4, which is:
2 Ag+ (aq) + CrO42- (aq) ⇌ Ag2CrO4 (s)
Next, we apply the Ksp expression:
Ksp = [Ag+]2[CrO42-]
Given the concentrations of the reactants and the total volume of the mixture, we can calculate the initial ion concentrations. For Ag+, this is (0.1000 M)(25.00 mL) / (25.00 mL + 35.00 mL) = 0.05882 M. For CrO42-, this is (0.05000 M)(35.00 mL) / (25.00 mL + 35.00 mL) = 0.02941 M. However, these initial concentrations will decrease when Ag2CrO4 begins to precipitate until the reaction reaches equilibrium. The equilibrium concentrations can then be calculated by setting up the Ksp expression and solving for the unknown concentrations, taking the stoichiometry of the reaction into account.