A solution is 0.1M in Cl^- and 0.1M in CrO₄^-- ions. If solid AgNO₃ is gradually added to this solution which one will precipitate first? At what concentration of Cl^-, Ag₂CrO₄ starts precipitating? (K_sp of AgCl= 1.7x10^-19, K_sp of Ag₂CrO₄ = 1.9x10^-12).

Dear student,

• Solubility Product, K_sp, refers to an ionic compound dissolving to form ions
• For the reaction: MA(s) M⁺(aq) + A^-(aq)

  The equilibrium constant K is:

  K =	[M+][A-]
  	[MA]

   

• Since the concentration of the solid is a constant, it is effectively incorporated into the equilibrium constant: K_sp = [M⁺][A^-]
• [M⁺][A^-] is referred to as the ion product.
• At equilibrium, the ion product = solubility product (K_sp) and the solution is said to be saturated.
• A precipitate will form when two solutions are mixed if the ion product is greater than the solubility product, ie, [M⁺][A^-] > K_sp

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