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![CoS (s) — Cot (aq) + saraz) , Ksp For precipitation to begin Q = [cost] [52] = ksp > 10.0062)(529= 4.0x162=> [S2] = 6.4516x1](http://img.homeworklib.com/questions/dda44c90-72f8-11ea-bea1-d3bf51e8022c.png?x-oss-process=image/resize,w_560)
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Calculate the pH needed to just start preci ue ph needed to just start precipitation of...
What would be the pH needed to initiate precipitation for a solution that contains 4.88 times...
What would be the pH needed to initiate precipitation for a solution that contains 4.88 times 10^-3 M Pb (NO_3)_2? Ksp of Pb(OH)_2 is 1.2 times 10^-15?
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2?...
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
Please help with chemistry 17. Find the new K value for the combined solubility equilibrium and...
Please help with chemistry
17. Find the new K value for the combined solubility equilibrium and formation equilibrium reactions when the Ksp for PbCO, is 7.4x10M and the K, for the [Pb(GOJ2]2-complex ion is 3.5x106. (C2042-?S the bidentate oxalate ligand.) The K, for the complexion Pb(EDTA)2-is 2.0x108. Analysis shows a solution at equilibrium contains [Pb(EDTA?] = 0.0011 M, [EDTA"] = 0.88 M, and [Pb2+]s 6.25×10-22 M. what concentration of sulfide ion will just start the precipitation of PbS(s) from the...
1. Consult an appropriate source and determine the Concentration of each of the following species, when...
1. Consult an appropriate source and determine the Concentration of each of the following species, when in Concentrated form: HCl, H2SO4, and NH3. 2. A 10mL solution of 0.010M HCl is mixed with 20mL of a 0.01M Pb2+ solution, giving a total volume of 30mL. What are the concentrations of Cland Pb2+ after the mixing? Will a precipitate of PbCl2 form? (Ksp = 1.7 x 10-5 for PbCl2 at 25oC.) 3. In the Group 2 precipitations, the Sulfide Ion (S2-...
1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present...
1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present in 2.0 L of a saturated strontium fluoride solution. A.9.0×10-8 B.2.7×10-11 C.6.9×10-9 D.1.1×10-10 E.1.4×10-6 2. Choose the correct equilibrium constant expression (Ksp) for the dissolution of Ag2S . (is the answer D?) A. [ Ag2S ] Ksp = [ Ag+]2 [ S2-] B. Ksp = [ Ag+][ S2-]2 C. [ Ag+] [ S2-] Ka = [ Ag2S ] D. Ksp = [ Ag+]2 [...
A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at...
A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at 0.010 M, was saturated with H2S(g) at room temperature. Assume that the pH of the solution remains constant and that the [H2S]sat = 0.10 M. The Ksp for MnS9S) is 2.5 x 10-13 , Ksp for CdS(s) is 8.0 x 10 -27 and Ksp for FeS(s) is 6.3 x10-18 . For H2S:Ka1=1.3 x 10-7. Ka2=8.5 x 10-14. Calculate the equilibrium concentrations of Mn2+(aq),Cd2+(aq), and...
Hello, I need help with thisquestion (the one that asks for PH) with step explanation. Many...
Hello, I need help with thisquestion (the one that asks for
PH)
with step explanation.
Many thanks!
(awnser is A)
H2S+ S2 What is the pH of a saturated solution of Mg(OH)2 at 25 oC, given that Ksp for Mg(OH)2 8.9 x 10-12 at this temperature? 10.4 10.7 10.1 8.63 none of these hat is the solubility in mol Lt of siver carbonate in pure water? Ksp 8.50 x 10" for Ag2CO3
Calculate the pH of a 0.982 M solution of hydrogen sulfide (H2S) Where: H2S (aq) ->...
Calculate the pH of a 0.982 M solution of hydrogen sulfide (H2S) Where: H2S (aq) -> H+ (aq) + HS- (aq) Ka1 = 1.0 x 10-7 HS- (aq) -> H+ (aq) + S2- (aq) Ka2 = 1.0 x 10-19 Enter your answer with at least 2 sig figs.
Just need the Solubility of SnS2 As discussed in the lab intro, a low concentration of...
Just need the Solubility of SnS2
As discussed in the lab intro, a low concentration of sulfide is needed to precipitate group II ions. This is because the group II sulfides are much less soluble than group III sulfides. Prove this by calculating the molar solubility of SnS2(Sn4+ is a group II ion) and Al2S3 (A1%+ is a group III ion). The Ksp values are given below. Type your answers in the boxes below. SnS2 Ksp = 1 x 10-46...
Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) =...
Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) = 1.1x10-10 solubility = AL The equilibrium concentration of chloride ion in a saturated lead chloride solution is M. In the presence of excess OH, the Ar+ (aq) ion forms a hydroxide complex ion. Al(OH)4 Calculate the concentration of free Ap+ ion when 1.56x10-mol Al(CH2C00)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For Al(OH)4, Ke=...
What would be the pH needed to initiate precipitation for a solution that contains 4.88 times 10^-3 M Pb (NO_3)_2? Ksp of Pb(OH)_2 is 1.2 times 10^-15?
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
Please help with chemistry
17. Find the new K value for the combined solubility equilibrium and formation equilibrium reactions when the Ksp for PbCO, is 7.4x10M and the K, for the [Pb(GOJ2]2-complex ion is 3.5x106. (C2042-?S the bidentate oxalate ligand.) The K, for the complexion Pb(EDTA)2-is 2.0x108. Analysis shows a solution at equilibrium contains [Pb(EDTA?] = 0.0011 M, [EDTA"] = 0.88 M, and [Pb2+]s 6.25×10-22 M. what concentration of sulfide ion will just start the precipitation of PbS(s) from the...
Hello, I need help with thisquestion (the one that asks for
PH)
with step explanation.
Many thanks!
(awnser is A)
H2S+ S2 What is the pH of a saturated solution of Mg(OH)2 at 25 oC, given that Ksp for Mg(OH)2 8.9 x 10-12 at this temperature? 10.4 10.7 10.1 8.63 none of these hat is the solubility in mol Lt of siver carbonate in pure water? Ksp 8.50 x 10" for Ag2CO3
Just need the Solubility of SnS2
As discussed in the lab intro, a low concentration of sulfide is needed to precipitate group II ions. This is because the group II sulfides are much less soluble than group III sulfides. Prove this by calculating the molar solubility of SnS2(Sn4+ is a group II ion) and Al2S3 (A1%+ is a group III ion). The Ksp values are given below. Type your answers in the boxes below. SnS2 Ksp = 1 x 10-46...
Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) = 1.1x10-10 solubility = AL The equilibrium concentration of chloride ion in a saturated lead chloride solution is M. In the presence of excess OH, the Ar+ (aq) ion forms a hydroxide complex ion. Al(OH)4 Calculate the concentration of free Ap+ ion when 1.56x10-mol Al(CH2C00)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For Al(OH)4, Ke=...
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