Consider these reactions: AgCl(s) Ag^+ (aq) + Cl^- (aq K_c = 1.8 Times 10^-10 Ag

Question

Consider these reactions: AgCl(s) Ag^+ (aq) + Cl^- (aq K_c = 1.8 Times 10^-10 Ag_2 CrO_4 (S) 2 Ag^+ (aq) + CrO_4^2- (aq) K_c = 9.0 Times 10^-12 If both solids are placed in water in a quantity sufficient to form a saturated solution, which solution will contain the highest [Ag^+] at equilibrium? The first, since K_c is higher. The second, since K_c is lower. The second, since there are two silver ions per formula unit. Will depend on amount of each solid originally present Cannont say without more detailed calculation.

Explanation / Answer

the first Kc is higher .because the concentration of the prduct is more ,the value of Kc is also higher

therfore in the first case the concentration of [Ag^+] is more at equilibrium.

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