Addition of Silver nitrate water solution to weak solution of Potassium chromate leads to precipitation in case of: C^2(Ag^+)cdot C(CrO_(4)^2-)gt K_(s)^circ (Ag_(2)CrO_(4)) C(AgNO_(3))gt C(K_(2)CrO_(4)) C(Ag^+)=C(CrO_(4)^2-) C(Ag^+)cdot C(CrO_(4)^2-)=K_(s)^circ (Ag_(2)CrO_(4))

The correct answer is:<br /><br />$C(Ag^{+})\cdot C(CrO_{4}^{2-})=K_{s}^{\circ }(Ag_{2}CrO_{4})$<br /><br />Explanation: When silver nitrate (AgNO3) is added to a weak solution of potassium chromate (K2CrO4), a precipitation reaction occurs if the product of the concentrations of the ions exceeds the solubility product constant (Ksp) of the precipitate, silver chromate (Ag2CrO4). The condition for precipitation to occur is when the ion product (Q) is greater than Ksp, which is represented by the equation $C(Ag^{+})\cdot C(CrO_{4}^{2-})=K_{s}^{\circ }(Ag_{2}CrO_{4})$. This equation indicates that the concentrations of silver ions (Ag+) and chromate ions (CrO42-) are such that their product equals the solubility product constant of silver chromate, leading to the formation of a precipitate.