Ag+(aq) + Cl-(aq) ---> AgCl (aq) K= 2.0 e3 AgCl (aq) + Cl- (aq) ----> AgCl-2 K =

Question

Ag+(aq) + Cl-(aq) ---> AgCl (aq) K= 2.0 e3 AgCl (aq) + Cl- (aq) ----> AgCl-2 K =9.1e1 AgCl (s)----> Ag+ (aq) + Cl- (aq) K= 1.8 e-10
If the concentrations of HCl is 0.60M, what are the concentrations of the soluble silver compounds in solution? Use these 3 equations to calculate. Almost like silver alloy lab Ag+(aq) + Cl-(aq) ---> AgCl (aq) K= 2.0 e3 AgCl (aq) + Cl- (aq) ----> AgCl-2 K =9.1e1 AgCl (s)----> Ag+ (aq) + Cl- (aq) K= 1.8 e-10
If the concentrations of HCl is 0.60M, what are the concentrations of the soluble silver compounds in solution? Use these 3 equations to calculate. Almost like silver alloy lab AgCl (aq) + Cl- (aq) ----> AgCl-2 K =9.1e1 AgCl (s)----> Ag+ (aq) + Cl- (aq) K= 1.8 e-10
If the concentrations of HCl is 0.60M, what are the concentrations of the soluble silver compounds in solution? Use these 3 equations to calculate. Almost like silver alloy lab

Explanation / Answer

Given [HCl] = [Cl-(aq)] = 0.60 M

AgCl(s) ---------> Ag+(aq) + Cl-(aq); K = Ksp = 1.8x10-10

Hence 1.8x10-10 = [Ag+(aq)]x[Cl-(aq)]

=> 1.8x10-10 = [Ag+(aq)]x0.60

=> [Ag+(aq)] = 1.8x10-10 / 0.60 = 3.0x10-10 M ------ (1)

Also given

Ag+(aq) + Cl-(aq) ------- > AgCl(aq): K = 2.0x103  

K = 2.0x103 = [AgCl(aq)] / [Ag+(aq)]x[Cl-(aq)]

=> 2.0x103 = [AgCl(aq)] / (3.0x10-10 x 0.60) [ From eqn(1)]

=> [AgCl(aq)] =  2.0x103 x (3.0x10-10 x 0.60) = 3.6x10-7 M (answer)

Also given

AgCl(aq) + Cl-(aq) ------- > AgCl2-(aq): K = 9.1x101

K = 9.1x101 = [AgCl2-(aq)] / [AgCl(aq)]x[Cl-(aq)]

=> 9.1x101 =  [AgCl2-(aq)] / (3.6x10-7 x 0.60)

=>  [AgCl2-(aq)] =  9.1x101 x(3.6x10-7 x 0.60) = 1.97x10-5 M (answer)

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