solubility product id defined as the product of concentration of
ions in the solution.
Which is the correct Ksp expression for Ag2CrO4 (s) dissolving in water? Ksp = [Ag*12(CrO42-1 Ksp...
Oc Asp – [Ag2+? [C03-] Which is the correct Ksp expression for Ag2CO3 (s) dissolving in water? Ksp = [Ag2+1 C03-12 O B. Ksp - [Ag2+1 (003-] OA OD . Ksp = [Ag+12 [CO32- Ksp = [Ag"] [CO32-
Which is the correct Ksp expression for PbCl2 (s) dissolving in water? Ksp = [Pb2+] [c1-32 Ksp = [Pb2+] [61] Ksp = [Pb2+12 [014] Ksp = [PbCit] [C1) Ksp = [Pb+] (C12-2
Given: Ksp(Ag2CrO4) = 1.2×10-12 Ksp(BaCrO4) = 2.1×10-10 For a solution which is initially 0.060 M in Ba2+ and 0.060 M in Ag+, it is desired to precipitate one of these ions as its chromate (CrO42−) salt to the maximum possible degree without precipitating any of the other cation. From this solution, which ion can be selectively first-precipitated by controlled addition of CrO42− and, ideally, what is the maximum possible percentage of that ion which can be exclusively so precipitated? (Assume...
Given: Ksp(Ag2Cro4) = 1.2x10-12 Ksp(BaCro4) 2.1x10-10 For a solution which is initially 0.002 M in Ba2 and 0.002 M in Ag*, it is desired to precipitate one of these ions as its chromate (CrO42 salt to the maximum possible degree without precipitating any of the other cation. From this solution, which ion can be selectively first-precipitated by controlled addition of CrO42- and, ideally, what is the maximum possible percentage of that ion which can be exclusively so precipitated? (Assume that...
Please help me slove the blanks please absorbance (CrO4)2- [Ag+] ksp of Ag2CRO4 0.504 0.506 0.506 Average ksp: SD: PLEASE SO CALCULATION.INFORMATION NEED TO Solve this problem would be. inital[CrO42-]=0.0024M VOL OF 0.0024M K2CrO4 total vol Cro4- absorbance 1ml 100ml 0.000024 0.057 5ml 100ml 0.00012 0.284 10ml 100ml 0.00024 0.432 15ml 100ml 0.00036 0.502 AVG MOLAR ABSORPTION COEFFICEINT: SD: Molar absorbtion coefficient [Cro42-] 1.3*10-6cm-1M-1, 2.3*10-5 cm-1M-1, 108*10-5cm-1M-1, 1.8*10-4CM-1M-1 CAN YOU ALSO FIND THE AVERAGE FOR THE MOLAR ABSORPTION COEFFICIENT AND...
Calculate the solubility of Ag2CrO4 in water at 25°C. You'll
find Ksp data in the ALEKS Data tab. Round your answer to 2
significant digits.
(Ksp=1.12x10^-12)
Calculate the solubility of Ag, CrO4 in water at 25 °C. You'll find K data in the ALEKS Data tab. Round your answer to 2 significant digits. Flora x 6 ?
18. If the Ksp for a compound dissolving in water at 25°C is 2.4. Determine AG at 25°C. Is this process spontaneous our not? (3 pts)
What is the correct expression for Ksp when BaSO4(s) dissolves in water
For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5.
calculate deltaG standard at 25 degrees C.
12. For the dissolving of PbCl2 in water Ksp is 1.7 x 10-5. Calculate AG at 25°C. If [Pb2+] = .010M and [Cl-) = .01M what is AG?
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 :)