The solubility product of reaction below at 25C is 1.6x10^-10: AgCl(s) <-> Ag+(aq) + Cl-(aq) show...
Consider the Gibbs energies at 25 ∘C. SubstanceSubstance ΔG∘f (kJ⋅mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq)Ag+(aq) 77.177.1 Cl−(aq)Cl−(aq) −131.2−131.2 AgCl(s)AgCl(s) −109.8−109.8 Br−(aq)Br−(aq) −104.0−104.0 AgBr(s)AgBr(s) −96.9−96.9 (a) Calculate ΔG∘rxn for the dissolution of AgCl(s)AgCl(s). kJ⋅mol−1 (b) Calculate the solubility-product constant of AgCl. K= (c) Calculate ΔG∘rxnΔGrxn∘ for the dissolution of AgBr(s)AgBr(s). kJ⋅mol−1kJ⋅mol−1 (d) Calculate the solubility-product constant of AgBr. K=K=
Consider the reaction for the dissolution of AgCl in water below at 25⁰C: AgCl(s) DAg+(aq) + Cl-(aq) Using the standard free energy of formation values (ΔG⁰f) from the appendix, calculate the Kc value for this reaction. Calculate the ΔG for the dissolving of AgCl in water at 25⁰C when: [Ag+]=[Cl-]= 1.00 x 10-4M
AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about the dissolution of AgCl in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-] =...
Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2(s)+2Ag+(aq)⇌2AgCl(s)+Pb2+(aq)
What is the solubility of AgCl in pure water at 25°C? The Ksp of AgCl is 1.8x10^-10. 9.0 x 10^-11 1.3 x 10^-5 1.8 x 10^-3 3.6 x 10^-10 What is the solubility of AgCl in 10 M NH3? The Kf of Ag(NH3)2+ from AgCl(s) in aqueous NH3 is 0.0031, which is for the balanced reaction shown below. AgCl(s) + 2 NH3(aq) → Ag(NH3)2+(aq) + Cl-(aq) Kf = 0.0031 0.176 M 0.426 M 0.023 M 0.557 M
Based on the ∆Go = -RTlnK expression, would you predict that AgCl (s) dissolving into Ag+ (aq) and Cl- (aq) (Ksp = 1.8x10-10) is a spontaneous process? Yes or no. I am having a hard time grasping this concept, so could you show your work please? Thank you :)
AgCl dissolves in aqueous solutions of S2O3 2- via formation of complex, Ag(S2O3) 3- AgCl(s) + 2 S2O3 2- (aq) → Ag(S2O3)2 3- (aq) + Cl-(aq). Using Ksp and Kf, Calculate the value of KC for the above reaction. Kf for Ag(S2O3)2 3- is 2.9 x 1013 ; Ksp for AgCl is 1.8 x 10-10. Show the sequence of equations that yield the above reaction. Please help :)
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...
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product constant, Ksp = 8.3 x 10-17 at 25°C. Calculate AG for the reaction when [Ag+]=1.5 x 10-3 M and [Br] =1.5 x 10-2 M. Is the reaction spontaneous or nonspontaneous at these concentrations? AG = 98 kJ/mol, spontaneous AG = 92 kJ/mol, nonspontaneous AG = -65 kJ/mol, spontaneous AG = 65 kJ/mol, nonspontaneous AG = -92 kJ/mol, spontaneous
follow the instructions properly please As determined from emf measurements, the solubility product constant at 25C of Aglu C of AgCl is Ksp 1.72x10-10 (molal units). (a) Find the solubility (in mol kg1) of AgCl in pure water. (b) If sufficient NaCl is added to the system to form a 0.01 molal solution of NaCl, what is the solubility of NaCI? (c) What is the solubility of AgCl in a 0.01 molal solution of NaNO3? rl K, en pie c...