1.Solid silver sulfide and solid
iron(III) sulfide are in equilibrium with a
solution containing 1.33×10-2 M
iron(III) acetate.
Calculate the concentration of silver ion present
in this solution.
[silver] = M
2.Solid barium sulfite and solid barium
sulfate are in equilibrium with a solution containing
6.16×10-3 M ammonium
sulfite.
Calculate the concentration of sulfate ion present
in this solution.
[sulfate] = M
3.Solid iron(III) hydroxide and solid
chromium(III) hydroxide are in equilibrium with a
solution containing 9.28×10-3 M
chromium(III) acetate.
Calculate the concentration of iron(III) ion
present in this solution.
[iron(III)] = M
PbBr26.3 × 10-6
AgBr3.3 × 10-13CarbonatesBaCO38.1 ×
10-9
CaCO33.8 × 10-9
CoCO38.0 × 10-13
CuCO32.5 × 10-10
FeCO33.5 × 10-11
PbCO31.5 × 10-13
MgCO34.0 × 10-5
MnCO31.8 × 10-11
NiCO36.6 × 10-9
Ag2CO38.1 × 10-12
ZnCO31.5 × 10-11ChloridesPbCl21.7
× 10-5
AgCl1.8 × 10-10ChromatesBaCrO42.0 ×
10-10
CaCrO47.1 × 10-4
PbCrO41.8 × 10-14
Ag2CrO49.0 ×
10-12CyanidesNi(CN)23.0 ×
10-23
AgCN1.2 × 10-16
Zn(CN)28.0 × 10-12FluoridesBaF21.7
× 10-6
CaF23.9 × 10-11
PbF23.7 × 10-8
MgF26.4 × 10-9HydroxidesAgOH2.0 ×
10-8
Al(OH)31.9 × 10-33
Ca(OH)27.9 × 10-6
Cr(OH)36.7 × 10-31
Co(OH)22.5 × 10-16
Cu(OH)21.6 × 10-19
Fe(OH)27.9 × 10-15
Fe(OH)36.3 × 10-38
Pb(OH)22.8 × 10-16
Mg(OH)21.5 × 10-11
Mn(OH)24.6 × 10-14
Ni(OH)22.8 × 10-16
Zn(OH)24.5 × 10-17IodidesPbI28.7 ×
10-9
AgI1.5 × 10-16OxalatesBaC2O41.1 ×
10-7
CaC2O42.3 × 10-9
MgC2O48.6 ×
10-5PhosphatesAlPO41.3 ×
10-20
Ba3(PO4)21.3 ×
10-29
Ca3(PO4)21.0 ×
10-25
CrPO42.4 × 10-23
Pb3(PO4)23.0 ×
10-44
Ag3PO41.3 × 10-20
Zn3(PO4)29.1 ×
10-33SulfatesBaSO41.1 ×
10-10
CaSO42.4 × 10-5
PbSO41.8 × 10-8
Ag2SO41.7 × 10-5 SulfidesCaS 8 ×
10-6
CoS 5.9 × 10-21
CuS 7.9 × 10-37
FeS 4.9 × 10-18
Fe2S31.4 × 10-88
PbS 3.2 × 10-28
MnS 5.1 × 10-15
NiS 3.0 × 10-21
Ag2S 1.0 × 10-49
ZnS 2.0 × 10-25SulfitesBaSO38.0 ×
10-7
CaSO3 1.3 × 10-8
Ag2SO3 1.5 × 10-14
1.Solid silver sulfide and solid iron(III) sulfide are in equilibrium with a solution containing 1.33×10-2 M...
Solid silver sulfide and solid iron(III) sulfide are in equilibrium with a solution containing 1.33×10-2 M iron(III) acetate. Calculate the concentration of silver ion present in this solution. [silver] = M KSPS=AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9 CaCO33.8 × 10-9 CoCO38.0 × 10-13 CuCO32.5 × 10-10 FeCO33.5 × 10-11 PbCO31.5 × 10-13 MgCO34.0 × 10-5 MnCO31.8 × 10-11 NiCO36.6 × 10-9 Ag2CO38.1 × 10-12 ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5 AgCl1.8 × 10-1. BaCrO42.0 × 10-10 CaCrO47.1 × 10-4 PbCrO41.8 × 10-14 Ag2CrO49.0...
Solid barium sulfite and solid barium sulfate are in equilibrium with a solution containing 6.16×10-3 M ammonium sulfite. Calculate the concentration of sulfate ion present in this solution. [sulfate] = M KSPS=AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9 CaCO33.8 × 10-9 CoCO38.0 × 10-13 CuCO32.5 × 10-10 FeCO33.5 × 10-11 PbCO31.5 × 10-13 MgCO34.0 × 10-5 MnCO31.8 × 10-11 NiCO36.6 × 10-9 Ag2CO38.1 × 10-12 ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5 AgCl1.8 × 10-1. BaCrO42.0 × 10-10 CaCrO47.1 × 10-4 PbCrO41.8 × 10-14 Ag2CrO49.0...
1.Solid sodium sulfide is slowly added to 125 mL of a 0.0450 M silver nitrate solution. The concentration of sulfide ion required to just initiate precipitation is M. 2.Solid barium acetate is slowly added to 50.0 mL of a 0.0522 M ammonium sulfite solution. The concentration of barium ion required to just initiate precipitation is M. 3.Solid potassium hydroxide is slowly added to 150 mL of a 0.0329 M iron(III) nitrate solution. The concentration of hydroxide ion required to just initiate precipitation...
A solution contains 9.62×10-3 M silver nitrate and 7.16×10-3 M lead acetate. Solid sodium bromide is added slowly to this mixture. What is the concentration of silver ion when lead ion begins to precipitate? [Ag+] = M ksp=AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9 CaCO33.8 × 10-9 CoCO38.0 × 10-13 CuCO32.5 × 10-10 FeCO33.5 × 10-11 PbCO31.5 × 10-13 MgCO34.0 × 10-5 MnCO31.8 × 10-11 NiCO36.6 × 10-9 Ag2CO38.1 × 10-12 ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5 AgCl1.8 × 10-1. BaCrO42.0 × 10-10 CaCrO47.1...
The equilibrium concentration of iron(III) ion in a saturated iron(III) sulfide solution is ___ M. (the Ksp is given as 1.4 × 10-88)
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Solid copper(II) carbonate and solid copper(II) sulfide are in equilibrium with a solution containing 1.12×10-2 M sodium carbonate. Calculate the concentration of sulfide ion present in this solution. [sulfide] = M
A solution contains 1.31×10-2 M lead nitrate and 1.12×10-2 M iron(III) acetate. Solid potassium sulfide is added slowly to this mixture. What is the concentration of iron(III) ion when lead ion begins to precipitate? [Fe3+] = M
1. Solid barium sulfide is slowly added to 75.0 mL of a 0.178 M sodium sulfite solution until the concentration of barium ion is 0.0288 M. The percent of sulfite ion remaining in solution is %. 2.Solid silver nitrite is slowly added to 125 mL of a potassium carbonate solution until the concentration of silver ion is 0.0134 M. The maximum amount of carbonate remaining in solution is M. 3.Solid sodium chromate is slowly added to 75.0 mL of a silver acetate...
Please help ASAP! 1. Solid iron(II) carbonate and solid iron(II) sulfide are in equilibrium with a solution containing 1.21×10-2 M sodium carbonate. Calculate the concentration of sulfide ion present in this solution. [sulfide] = ________ M 2. Solid manganese(II) sulfide and solid copper(II) sulfide are in equilibrium with a solution containing 1.31×10-2 M manganese(II) nitrate. Calculate the concentration of copper(II) ion present in this solution. [copper(II)] = _______ M 3. Consider these compounds: A. Al(OH)3 B. Cr(OH)3 C. Ag2CrO4 D....