The Ksp of Ag2CO3 is 8.1x10-12. What is the molar solubility of silver
Silver Chloride has a larger Ksp than silver carbonate (Ksp = 1.6x10‐10 and 8.1x10‐12 respectively). Does this mean that AgCl also has a larger molar solubility than Ag2CO3? Explain
Calculate the molar solubility of silver carbonate in a 0.0100M silver nitrate solution. ( Ksp ( Ag2CO3) = 8.1X E-12
What is the molar solubility of silver carbonate (Ag2CO3)? Kaip = 8.1 x 10-12
What is the molar solubility of silver carbonate (Ag2CO3) in water? The solubility product constant for Ag2CO3 is 8.1 x 10-12 at 25°C OA 1.4 x 10-6 OB 2.0 x 10-4 OC 40 x 10-6 OD.1.3 x 10-4 OE 2.7 * 10-12
Silver (I) carbonate (Ag2CO3 (s)) is a slightly soluble ionic compound with Ksp = 1.8 x 10-12. Calculate the solubility of Ag2CO3 (s) in mol/L.
(4) What is the molar solubility of silver carbonate (Ag2CO3 ) in water? The solubility-product constant for Ag2CO3 is 8.1 x 10-12 at 25°C. (SO (DOCHOV Shorts (Hint: Ag2CO3 will dissociate as 2Ag+ (aq) + CO32- calculate the solubility using ICE table) A) 1.4 x 10-6 WERE- B) 2.7 * 10-12 (OL C) 4.0 x 10-6 overw bywa to not soort nollapse D) 1.3 x 10-4 HONEY E) 2.0 * 10-4
If the Ksp of Ag2CO3 at 25 oC is 8.46e-12 , what is the molar solubility of Ag2CO3 at this temperature? a) At this temperature the molar solubility of Ag2CO3 is 6.05e-34 mol/L. b) At this temperature the molar solubility of Ag2CO3 is 2.04e-04 mol/L. c) At this temperature the molar solubility of Ag2CO3 is 2.91e-06 mol/L. d) At this temperature the molar solubility of Ag2CO3 is 1.28e-04 mol/L. e) At this temperature the molar solubility of Ag2CO3 is 2.42e-33...
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.
A lump of silver carbonate, Ag2CO3 , was placed in 450.0 mL of pure water. The Ksp for the dissolution of Ag2CO3 is 8.46 x 10-12 M3 and is described by: Ag2CO3 (s) « 2 Ag+ (aq) + CO32- (aq) After a length of time the equilibrium concentration of Ag+ ion in this solution would be: (a) 1.30 x 10-3 M (b) 7.17 x 10-3 M (c) 1.30 x 10-4 M (d) 2.57 x 10-4 M
I am interested in how to set this problem up, so not just that only silver will precipitate but why? A contaminated solution is 1.0x10-6M each for Pb2+ and Ag+ ions. If the carbonate level is raised to 0.00013 M, what will happen? (Ksp of PbCO3=7.4x10-14; Ag2CO3=8.1x10-12) only silver ions will precipitate only lead ions will precipitate neither contaminant will precipitate both contaminants will precipitate