Ag(NH3)2^+ (aq) -------------> Ag^+ (aq) + 2NH3(aq) Kd = 5.9*10^-8
Ag^+ (aq) + 2NH3(aq) -----------> Ag(NH3)2^+ (aq) 1/Kd =
AgI(s) -------------> Ag^+ (aq) + I^- (aq) Ksp = 8.3*10^-17
Ag^+ (aq) + 2NH3(aq) -----------> Ag(NH3)2^+ (aq)
AgI(s) -------------> Ag^+ (aq) + I^- (aq)
-----------------------------------------------------
AgI(s) + 2NH3(aq) -----------> Ag(NH3)2^+ (aq) + I^- (aq) KC = (1/Kd)*Ksp
Kc = 1/Kd * KSp
= (1/5.9*10^-8 )*8.3*10^-17
= 1.7*10^7 *8.3*10^-17
= 1.4*10^-9
b.1.4*10^-9 >>>>.answer
Q27.
molarity of Zn(OH)2 = W/G.M.Wt * volume in L
= 0.000222/99.424 = 2.23*10^-6M
Zn(OH)2(s) --------------> Zn^2+ (aq) + 2OH^- (aq)
s 2s
Ksp = [Zn^2+][OH^-]^2
= s*(2s)^2
= 4s^3
= 4(2.23*10^-6)^3
= 4.5*10^-17
a.4.5*10^-17 >>>answer
please answer both questions QUESTION 26 Given the two equilibria below, Ag(NH3)2 (aq) = Ag (aq)...
1. Given the two equilibria below, Ag(NH3)2(aq) = Agt(aq) + 2NH3(aq); Kd = 5.9 x 10-8 AgBr(s) Ag+(aq) + Br" (aq); Ksp = 5 x 10-13 what is K, for the following equilibrium? AgBr(s) + 2NH3(aq) = Ag(NH3)2(aq) + Br" (aq) a. 3 x 10-20 b.2.7 x 100 c. 7.2 x 10-11 d. 8.5 x 10-6 e. 1.2 x 105
Account for your observations. Consider the following equilibria: Ag^+(aq)+Cl^-(aq)<->AgCl(s) Ag^+(aq)+2NH3(aq)<->[Ag(NH3)2]^+(aq) NH3(aq)+H^+(aq)<->NH4^+(aq) Observations: adding NaCl: went from clear to a white solution adding NH3: went from white solution to. clear solution adding HNO3: solution warmed up
Ag+ forms complex ions with NH3 and S2O32- according to the following equilibria: Ag+(aq) + 2 NH3(aq) = [Ag(NH3)2]+(aq) K = 1.7 x 107 Ag+(aq) + 2 S2O32-(aq) = [Ag(S2O32-)2]3-(aq) K = 2.9 x 1013 Determine the value of K for the equilibrium: [Ag(S2O32-)2]3-(aq) + 2 NH3(aq) = [Ag(NH3)2]+(aq) + 2 S2O32-(aq) Using your K value as a guide, predict what would happen when 1 M NH3(aq) is added to a solution of [Ag(S2O32-)2]3-(aq). Explain your reasoning.
Use the following information to answer the following 3 questions: 2 Ti (NO3)2 (aq) + Ag (OH)4 (aq) <---> 2 Ti (OH)2 (aq) + Ag (NO3)4 (aq) Trial Ti(NO3)4, M Ag(OH)4 M R, M/s Trial 1: 0.0250 0.0442 3.4 x 10^-8 Trial 2: 0.0133 0.0224 4.9 x10^-9 Trial 3: 0.0133 0.0442 9.7 x 10^-9 a) determine the rate law and calculate the rate constant for the forward reaction: Reaction forward: 2 Ti(NO3)2...
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