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 that there is no change in the total volume of the
solution.)
Ba2+ or Ag+
%???
Given: Ksp(Ag2CrO4) = 1.2×10-12 Ksp(BaCrO4) = 2.1×10-10 For a solution which is initially 0.060 M in...
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...
Timer Notes Evaluate Feedback Print Inf Course Contents >> ... >> Given: Ksp(Ag Croa) = 41.2x10-12 Ksp(Bacroa) = 2.1x10-10 For a solution which is initially 0.005 M in Ba2+ and 0.005 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...
Given that, for AgCl, at 25°C, K = 1.6x10-10: What is the solubility (g/mL) of AgCl in water at 25°C? 1.26 x 10-5 M You have entered that answer before This question expects a numeric answer. Tries 0/5 Previous Tries Submit Answer 35.0 mL of 0.070 M NaCl is mixed with 35.0 mL of 0.140 M AgNO3. What is [CI] in the supernatant solution at equilibrium, at 25°C? Tries 0/5 Submit Answer What is the solubility (mass/volume) of AgCl in...
A solution containing a mixture of 0.0441 M 0.0441 M potassium chromate ( K 2 CrO 4 K2CrO4 ) and 0.0513 M 0.0513 M sodium oxalate ( Na 2 C 2 O 4 Na2C2O4 ) was titrated with a solution of barium chloride ( BaCl 2 BaCl2 ) for the purpose of separating CrO 2− 4 CrO42− and C 2 O 2− 4 C2O42− by precipitation with the Ba 2+ Ba2+ cation. The solubility product constants ( ? sp Ksp...
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
You have a mixture of three soluble cations with the following concentrations: i. Ag+ with [Ag+] = 0.02 M ii. Ca2+ with [Ca2+] = 0.1 M and iii. Ba2+ with [Ba2+] = 0.1 M Assuming that you are slowly adding CrO42- ions, which ion will precipitate first, second and third? The following Ksp values are provided. Ksp of Ag2CrO4 is 1.9 × 10-12 Ksp of CaCrO4 is 7.1 × 10-4 Ksp of BaCrO4 is 1.2 × 10-10 1. Ag+ first,...
Would you expect a precipitate to form in a solution that is 3.2 x 10-4 M CrO42- and 5.7 x 10-9M Ba2+? Ksp BaCrO4 = 1.2 x 10-10
If the Ksp of silver chromate (Ag2CrO4) is 1.1 x 10-12 and the silver ion concentration in the solution is 0.0005 M, what is the chromate ion concentration? 1.0 x 10-4 M 4.4 x 10-6 M 5.0 x 10-7 M 1.0 x 10-6 M 6.5 x 10-5 M
A solution contains 0.040 M of Na2SO4 and 0.050 M of NaIO3. Another solution of Ba2+ is added to the first solution.( You must accept that the original solution does not include HSO-4). a) Which of the Baryum salts precipitate firstly? b) Calculate the Ba2+ concentration while the first precipitate is occuring. c) While the more dissolved precipitate is precipitating, what is the concentration of anion which forms the less dissolved Baryum salt ? Ba(IO3) Ksp= 1.57x10-9 BaSO4 Ksp= 1.1x10-10
12. If a solution is 0.25 Min Ba2+ and 0.50 MPb+ upon addition of Na2CrO4(s) which solid will precipitate first and at what concentration of Cr042-will the second solid begin to form? Ksp(BaCrO.) 2.1 × 10-10 Ksp(PbCrO.) 2.3x 10-13 A. BaCrO4 will precipitate first, a [Cro,--] = 8.4 × 10-10 M will cause PbCrO4(s) to form. B. BaCrO4 will precipitate first, a [Cr042-] = 4.6 x 10-13 M will cause PbCrO4(s) to form. C. PbCrO4 will precipitate first, a [CrO41...