You have a mixture of three soluble cations with the following concentrations: i. Ag+ with [Ag+]...
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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, Ca2+ second, and Ba2+ last
2. Ag+ first, Ba2+ second, and Ca2+ last
3. Ba2+ first, Ag+ second, and Ca2+ last
4. Ba2+ first, Ca2+ second, and Ag+ last
Homework Answers
![0200 Determine [er Op 20 needed to start precipulate 03.00 Aggero 2 Ag+ Cro 20 Baeroa = Ba2O + Cro 20 - Ksp [Ago] x [ero 20 k](http://img.homeworklib.com/questions/3bc9a550-704a-11ea-aee2-cb49848b3e97.png?x-oss-process=image/resize,w_560)
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You have a mixture of three soluble cations with the following
concentrations:
i. Ag+ with [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) = 1.2×10-12 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...
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 contains 0.10 M concentrations of Ba2+, Ca2+, and Sr2+. Na2CO3 is slowly added to...
A solution contains 0.10 M concentrations of Ba2+, Ca2+, and Sr2+. Na2CO3 is slowly added to the solution. In what order will the ions begin to precipitate? What is the concentration of the first ion when the 2nd begins to precipitate? Ksp for BaCO3 = 2.58 x 10-9, for CaCO3 = 3.36 x 10-9, and for SrCO3 = 5.60 x 10-10.
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From...
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (a) AgBr: [Ag+] = 5.7 × 10^-7 M, [Br–] = 5.7 × 10^-7 M (b) CaCO3: [Ca^2+] = 5.3 × 10^-3 M, [CO3^2−] = 9.0 × 10^-7 M (c) PbF2: [Pb^2+] = 2.1 × 10^-3 M, [F–] = 4.2 × 10^-3 M (d) Ag2CrO4: [Ag+] = 5.3 × 10^-5 M, 3.2...
If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 ( Ksp =...
If a dilute AgNO3 solution is slowly added
to the solution, what is the first compound to precipitate: Ag2CrO4
( Ksp = 1.2×10?12), Ag2CO3 (
Ksp = 8.1×10?12), or AgCl ( Ksp
= 1.8×10?10)?
Problem 17.75 A solution contains three anions with the following concentrations: 0.20 M Cro 0.10 M CO and 0.010 M Cl Part A If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Aga Cro4 Ksp 1.2 x...
Timer Notes Evaluate Feedback Print Inf Course Contents >> ... >> Given: Ksp(Ag Croa) = 41.2x10-12...
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...
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...
Solubility Rules TABLE 1: SOLUBILITY RULES FOR CATIONS Precipitating agent lons that will form a precipitate...
Solubility Rules TABLE 1: SOLUBILITY RULES FOR CATIONS Precipitating agent lons that will form a precipitate Cl", Br", Agt, Pb2+, and Hg22 Ca2+, Sr2+, Ba2+, Agt, and Pb2+ All metal ions (with widely varying Ksp values) except Li, Na+, K+, and NHA All metal ions except Lit, Na, K, NH4+, Ca?, Srl, and Ba? CO32- All metal ions except Lit, Na, K, and NHA PO43- All metal ions except Lit, Na, K, and NH4 50,2- OH S2- Pre-Lab Questions 1....
28. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids....
28. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K for each of the slightly soluble solids indicated: (a) AgBr: [Ag*1 = 5.7 x 10-7M, [Br] =5.7 x 10-'M (b) CaCO3: [Ca?'] = 5.3 x 10-M, [CO,"") = 9.0 x 10-7M (c) PbFy: [Pb²+1 = 2.1 * 10-M, [F] = 4.2 x 10-PM (d) Ag, Cro: [Ag*1 = 5.3 * 10-SM, 3.2 x 10-'M (e) InF,: [In?'] =...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1 M sodium oxalate (Na2C_04) to this solution dropwise, which ion will begin precipitating first? Compound Ksp BaC204 1.6 x 10 CaC204 2.32 x 10 MgC20 4.83 x 10 ZnC2042.7 x 108 Determine the pH required for the onset of the precipitation of Ni(OH)2 from a 0.010-M NISO.(ag) solution at 25° C. At 25°C, K for Ni(OH)2 is 6.5 x 10-18
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...
If a dilute AgNO3 solution is slowly added
to the solution, what is the first compound to precipitate: Ag2CrO4
( Ksp = 1.2×10?12), Ag2CO3 (
Ksp = 8.1×10?12), or AgCl ( Ksp
= 1.8×10?10)?
Problem 17.75 A solution contains three anions with the following concentrations: 0.20 M Cro 0.10 M CO and 0.010 M Cl Part A If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Aga Cro4 Ksp 1.2 x...
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...
Solubility Rules TABLE 1: SOLUBILITY RULES FOR CATIONS Precipitating agent lons that will form a precipitate Cl", Br", Agt, Pb2+, and Hg22 Ca2+, Sr2+, Ba2+, Agt, and Pb2+ All metal ions (with widely varying Ksp values) except Li, Na+, K+, and NHA All metal ions except Lit, Na, K, NH4+, Ca?, Srl, and Ba? CO32- All metal ions except Lit, Na, K, and NHA PO43- All metal ions except Lit, Na, K, and NH4 50,2- OH S2- Pre-Lab Questions 1....
28. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K for each of the slightly soluble solids indicated: (a) AgBr: [Ag*1 = 5.7 x 10-7M, [Br] =5.7 x 10-'M (b) CaCO3: [Ca?'] = 5.3 x 10-M, [CO,"") = 9.0 x 10-7M (c) PbFy: [Pb²+1 = 2.1 * 10-M, [F] = 4.2 x 10-PM (d) Ag, Cro: [Ag*1 = 5.3 * 10-SM, 3.2 x 10-'M (e) InF,: [In?'] =...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1 M sodium oxalate (Na2C_04) to this solution dropwise, which ion will begin precipitating first? Compound Ksp BaC204 1.6 x 10 CaC204 2.32 x 10 MgC20 4.83 x 10 ZnC2042.7 x 108 Determine the pH required for the onset of the precipitation of Ni(OH)2 from a 0.010-M NISO.(ag) solution at 25° C. At 25°C, K for Ni(OH)2 is 6.5 x 10-18
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