The Ksp for BaSO4 is 1.1 x 10^-10 and that for BaSeO4 is 2.8 x 10^-11....
The Ksp for BaSO4 is 1.1 x 10^-10 and that for BaSeO4 is 2.8 x 10^-11. What concentration of [SO4]^-2 and [SeO4]^-2 are needed to precipitate out each salt? Which will precipitate first?
Homework Answers
the concentration of each ion at which salt will be precipitated will depands on the concentration of Ba2+ present in the solution.
since Ksp is less for BaSeO4 than BaSO4, so BaSeO4 will precipitate first.
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The Ksp for BaSO4 is 1.1 x 10^-10 and that for BaSeO4 is 2.8 x
10^-11....
15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a....
15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a. 1.0 x 10-5 b.2.0 x 10-5 c. 4.0 x 10-5 d. 8.0 x 10-5 o o 15b) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4 in 0.10 M Na2SO4? a. 2.8 x 10-10 b.5.5 x 10-10 c. 1.1 x 10-9 d. 2.2 x 10-9
Question 1 1 pts The Ksp value for BaSO4 Ksp = 1.1 x 10 10. If...
Question 1 1 pts The Ksp value for BaSO4 Ksp = 1.1 x 10 10. If 50.0 mL of 2.0 x 10-4 M Ba(NO3)2 is mixed with 350.0 mL of 1.0 x 10-5 M Na2SO4, will a precipitate be observed? A precipitate forms because the ion pair product, Q> Ksp A precipitate forms because the ion pair product, Q< Ksp. No precipitate forms because the ion pair product, Q = Ksp No precipitate forms because the ion pair product, Q<Ksp...
QUESTION 2 Kep(Ag2CrO4) = 9,0 x 10-12, Ksp(BaSO4) = 1.1 x 10-10, Ksp (AgSCN) - 1.2...
QUESTION 2 Kep(Ag2CrO4) = 9,0 x 10-12, Ksp(BaSO4) = 1.1 x 10-10, Ksp (AgSCN) - 1.2 x 10-12 What is the correct order of the solubility of the above ionic compounds? (from smallest to greatest) a. BaSO4 → AgSCN → Ag2C+04 b. AgSCN → Ag2CrO4 → BaSO4 c. AgSCN → BaSO4 → Ag2C104 d. No correct order is found. e. BaSO4 → Ag2Cr04 → AgSCN
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...
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...
(b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, c...
using debye-huckel limiting law
(b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions in aqueous solutions containing 1.2 x 10-3 mol kg of (i) Sucrose (you may assume this mixture is ideal) (ii) potassium nitrate (KNO3) (ii) copper sulphate (CuSO4). A 0.509 mol-1/2 kg 1/2)
(b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions...
Calculate the molar solubility of BaSO4 (Ksp for BaSO4 2.2x10^-10) A) in water B) in a...
Calculate the molar solubility of BaSO4 (Ksp for BaSO4
2.2x10^-10)
A) in water
B) in a solution 4.00M SO4 2-
(Use ICE table when solving)
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?
Given that PbBr2 has a Ksp of 4.0×10−5, PbCrO4 has a Ksp of 2.8×10−13, and Pb(OH)2...
Given that PbBr2 has a Ksp of 4.0×10−5, PbCrO4 has a Ksp of 2.8×10−13, and Pb(OH)2 has a Ksp of 1.2×10−15, which of these salts would precipitate first during selective precipitation?
What concentration of Ba2+ is necessary to begin precipitating BaSO4 if the sulfate concentration is 2.2...
What concentration of Ba2+ is necessary to begin precipitating BaSO4 if the sulfate concentration is 2.2 x 10-4 M? Ksp BaSO4 = 1.1 x 10-10
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M...
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C. 2. Calculate the molar solubility of CaF2 (Ksp = 4.0 x 10-11) in a 0.025 M NaF solution. 3. 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 (Kop -1.7 x 10-8) precipitate under...
15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a. 1.0 x 10-5 b.2.0 x 10-5 c. 4.0 x 10-5 d. 8.0 x 10-5 o o 15b) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4 in 0.10 M Na2SO4? a. 2.8 x 10-10 b.5.5 x 10-10 c. 1.1 x 10-9 d. 2.2 x 10-9
Question 1 1 pts The Ksp value for BaSO4 Ksp = 1.1 x 10 10. If 50.0 mL of 2.0 x 10-4 M Ba(NO3)2 is mixed with 350.0 mL of 1.0 x 10-5 M Na2SO4, will a precipitate be observed? A precipitate forms because the ion pair product, Q> Ksp A precipitate forms because the ion pair product, Q< Ksp. No precipitate forms because the ion pair product, Q = Ksp No precipitate forms because the ion pair product, Q<Ksp...
QUESTION 2 Kep(Ag2CrO4) = 9,0 x 10-12, Ksp(BaSO4) = 1.1 x 10-10, Ksp (AgSCN) - 1.2 x 10-12 What is the correct order of the solubility of the above ionic compounds? (from smallest to greatest) a. BaSO4 → AgSCN → Ag2C+04 b. AgSCN → Ag2CrO4 → BaSO4 c. AgSCN → BaSO4 → Ag2C104 d. No correct order is found. e. BaSO4 → Ag2Cr04 → AgSCN
using debye-huckel limiting law
(b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions in aqueous solutions containing 1.2 x 10-3 mol kg of (i) Sucrose (you may assume this mixture is ideal) (ii) potassium nitrate (KNO3) (ii) copper sulphate (CuSO4). A 0.509 mol-1/2 kg 1/2)
(b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions...
Calculate the molar solubility of BaSO4 (Ksp for BaSO4
2.2x10^-10)
A) in water
B) in a solution 4.00M SO4 2-
(Use ICE table when solving)
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C. 2. Calculate the molar solubility of CaF2 (Ksp = 4.0 x 10-11) in a 0.025 M NaF solution. 3. 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 (Kop -1.7 x 10-8) precipitate under...
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