What is the concentration of Ag⁺ ions in water saturated with Ag₃PO₄( K _sp = 1.60×10^{- 18}) ?

Question

Quizplus · Accepted Answer

The given compound Ag₃PO₄ is the solubility product constant for Ag⁺. Using the formula for solubility product constant, we can write: Ksp = [Ag^+][-] Since the water is saturated with Ag₃PO₄, we can assume that all of the Ag₃PO₄ compound is dissolved and dissociated to release Ag^{+ and}- ions. Therefore, we can substitute the Ksp value into the equation and solve for the concentration of Ag^{+ and}- ions: 1.60×10_sp = [Ag^+][-] [Ag^{+] = [}-] = sqrt(1.60×10_sp) = 3.56×10^{- 5} Therefore, the concentration of Ag^{+ and}- ions in water saturated with Ag₃PO₄ is 3.56×10^{- 5} M. However, the question asks for the concentration of Ag⁺ ions (which are both present in equal concentration due to being in a 1:1 ratio in the dissociation equation) so the answer is 4.68×10^{- 5} M (which is twice the concentration of either ion). Therefore, the correct answer is A.

What Is the Concentration of Ag+ Ions in Water Saturated

What Is the Concentration of Ag⁺ Ions in Water Saturated