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Would you expect a precipitate to form in a solution that is 3.2 x 10-4 M...
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) = 1.2×10-12 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...
You have a mixture of three soluble cations with the following concentrations: i. Ag+ with [Ag+]...
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,...
A solution containing a mixture of 0.0441 M 0.0441 M potassium chromate ( K 2 CrO...
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...
Will a precipitate form when 100.0 mL of 6.8 x 10-4 M Mg(NO3)2 is added to...
Will a precipitate form when 100.0 mL of 6.8 x 10-4 M Mg(NO3)2 is added to 100.0 mL of 1.2 x 10-4 M NaOH? The ion product for Mg(OH)2 is 1. Since Q is than Ksp, Mg(OH)2 precipitate from the solution.
12. If a solution is 0.25 Min Ba2+ and 0.50 MPb+ upon addition of Na2CrO4(s) which...
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...
Given: Ksp(Ag2Cro4) = 1.2x10-12 Ksp(BaCro4) 2.1x10-10 For a solution which is initially 0.002 M in Ba2...
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...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and the Cl- ion concentration is 3.2 x 10-4 M. Which of the following statements is true given that the Ksp for AgCl is 1.8 x 10^-10? A)No AgCl(s) will precipitate because Qsp<Ksp. B)No AgCl(s) will precipitate because the Ksp value indicates that AgCl is infinitely soluble in water. C)A precipitate of AgCl(s) will form because Qsp>Ksp. D)Insufficient data is given to make a prediction...
For the reaction Ba(OH)2 (s) -- Ba2+ (aq) + 2 OH (aq) a precipitate will form...
For the reaction Ba(OH)2 (s) -- Ba2+ (aq) + 2 OH (aq) a precipitate will form if Q< K. Select one: True False Into a solution of 0.10 M KBr and 0.10 M KCYOA you add 0.050 M silver nitrate dropwise until a precipitate forms. Ksp for Ag2Cronis 9.0 x 10-12. Ksp for AgBr is 5.0 x 10-13. Which of the following will precipitate first? Select one or more: a. silver chromate b. no precipitate will form C. silver bromide...
Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in...
Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in both Ba2+ and Pb2+ until [SO42-] reaches 1.0 x 10^-4 M. Would either BaSO4 (Ksp = 1.1 x 10^-10) or PbSO4 (Ksp = 1.7 x 10^-8) precipitate under these conditions?
A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+...
A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. 1. What concentration of SO2−4 is necessary to begin precipitation? (Neglect volume changes. BaSO4:Ksp=1.1×10−10; SrSO4:Ksp=3.2×10−7.) 2. What is the concentration of SO2−4 when the second cation begins to precipitate?
Will a precipitate form when 100.0 mL of 6.8 x 10-4 M Mg(NO3)2 is added to 100.0 mL of 1.2 x 10-4 M NaOH? The ion product for Mg(OH)2 is 1. Since Q is than Ksp, Mg(OH)2 precipitate from the solution.
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...
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...
For the reaction Ba(OH)2 (s) -- Ba2+ (aq) + 2 OH (aq) a precipitate will form if Q< K. Select one: True False Into a solution of 0.10 M KBr and 0.10 M KCYOA you add 0.050 M silver nitrate dropwise until a precipitate forms. Ksp for Ag2Cronis 9.0 x 10-12. Ksp for AgBr is 5.0 x 10-13. Which of the following will precipitate first? Select one or more: a. silver chromate b. no precipitate will form C. silver bromide...
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