The "insoluble" salt, silver sulfide, has a solubility product, Ksp=6.3*10^-51 at 298 K.
Ag2S(s)=2Ag+ (aq)+ S2-(aq)
What is the concentration of Ag+ at equilibrium, at this temperature?
The "insoluble" salt, silver sulfide, has a solubility product, Ksp=6.3*10^-51 at 298 K. Ag2S(s)=2Ag+ (aq)+ S2-(aq)...
Complete the following reaction table and Ksp expression to calculate the solubility of silver sulfide. (48219831453 252 SS32530 25 Concentration (M) Ag2S(s) = 2Agt(aq) + 52 (aq) Initial Change Equilibrium Кsp
20 points water is 1.3 x 10-16mol/L. The solubility of silver sulfide can be greatly increased by formation of a complex ion such as Ag(NH3)2. Calculate the molar solubility of AgaS in 10M NH3. Show your work for full credit. Sulfides salts are generally very insoluble. The solubility of silver sulfide, AgaS, in pure Ag2S Ksp= 8.0 x 1048 Ag(NHs)2 Kr 1.7x 10
Consider the solubility of this salt in water at a temperature of 298. K. The equilibrium constant is K0.0011 at 298 K. CdCl,(s)Cd2 (aq) 2Cl-(aq) Solid NaCl is added to a saturated solution of cdcl, to make the NaCI concentration 0. 188 M. Calculate AG for Cdcl, immediately after the NaCl dissolves and before any further reaction of the CdCl, occurs. Assume no volume change takes place when the NaCl is added. Plus or minus 2% 2 Attempts Submit J/mol...
For the insoluble salt cadmium (II) iodate, the solubility product, Ksp, is 2.3 x 10-8. a) Write the solubility product expression for cadmium (II) iodate. b) Determine the molar solubility (M) of cadmium (II) iodate in pure water. c) Calculate the solubility (M) of cadmium (II) iodate in a solution of 0.20 M Cd(NO3)2. Comment on whether the solubility has increased or decreased from part (b). d) Predict whether the solubility of cadmium (II) iodate will increase or decrease if...
Silver cobonate Ag2CO3 is a salt of low solubility, when placed in water it dissolved until equilibrium is reached Ag2CO3(s)----> 2Ag+(aq) + CO32-(aq) Write a solubility product constatnt Ksp of silver carbonate.
Find Ksp The generic metal A forms an insoluble salt AB(s) and a complex ACs(aq). The equilibrium concentrations in a solution of ACs were found to be (A) = 0.100 M, [C] = 0.0140 M, and [ACs) = 0.100 M. Determine the formation constant, K, of AC5. Number K,= 1.86 x 10 The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.175 M. What is the Ksp of AB? Number
Silver is found as Ag2S (Ksp = 6x10-51) in the ore argentite. Given the formation constant of silver cyanide complex Ag(CN) - as 1.0x1021, determine the following: 2 (a) The equilibrium constant for the cyanidation of Ag S to Ag(CN) . 2 2- Answer:K=6x10^(-9) (b) Would cyanidation be a practical means of leaching silver from argentite ore? Answer: K<<1; Cyanidation is not practical (c) Silver is found as AgCl in horn silver ore. Determine the equilibrium constant for the cyanidation...
An insoluble salt, MX2, dissociates slightly in water, MX2(s) + M2+ (aq) + 2X-(aq); Ksp = 9.5 x 10-14 at 25 oC. Calculate AG for the dissociation reaction when the concentration of ions are: [M2+] = 6.4 x 10-2 M and {X-} = 9.4 x 10-5 M.
answer these please 17. The solubility of AgCl is 0.000 013 mol/L. Calculate the Ksp for AgCl. 18. If the concentration of chloride ion remaining in solution after silver chloride has been precipitated is 0.2 M, what is the concentration of the silver ion? Kap of AgCl is 2.8 X 10-10 19. What is the experimental Ksp of CaCO3 if the residue after evaporation of a 1.00 L saturated solution is found to have a mass of 0.006 90 g?...
1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present in 2.0 L of a saturated strontium fluoride solution. A.9.0×10-8 B.2.7×10-11 C.6.9×10-9 D.1.1×10-10 E.1.4×10-6 2. Choose the correct equilibrium constant expression (Ksp) for the dissolution of Ag2S . (is the answer D?) A. [ Ag2S ] Ksp = [ Ag+]2 [ S2-] B. Ksp = [ Ag+][ S2-]2 C. [ Ag+] [ S2-] Ka = [ Ag2S ] D. Ksp = [ Ag+]2 [...