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16 Cards in this Set
- Front
- Back
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What is the equilibrium constant expression for dissolving iron (III) hydroxide in water? |
Ksp = [Fe+3] [OH-]3 |
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The LEAST soluble sulfide is |
CuS; Ksp = 1.0 x 10-36 |
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A flask contains the following chemical system at equilibrium:CuCO3(s) Cu2+(aq) + 2 CO32–(aq)Addition of which of the following substances will increase the solubility of CuCO3(s) in water?(1) aqueous hydrochloric acid(2) aqueous sodium carbonate(3) solid copper(II) carbonate |
(1) only |
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The solubility of lead(II) iodide (FW=461.0 g/mol) is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II) iodide? |
1.1 x 10-8 |
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The molar solubility of magnesium carbonate Mg(CO3) is 1.8 x 10-4 mol/L. What is the Ksp for this compound? |
3.2 x 10-8 |
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Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.1 x 10-12). |
2.5 x 10-4 M |
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The Ksp of BaSO4 is 1.1 x 10–10 at 25 °C. What mass of BaSO4 (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25°C? |
2.4 x 10-3 g |
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What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at 25°C? The Ksp of Mn(OH)2 is 1.9 x 10–13 at 25°C. |
1.9 x 10–1 mol/L |
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At what pH will an aqueous solution of 0.200 M Ni2+ begin to precipitate as Ni(OH)2 at 25°C? The Ksp of Ni(OH)2 is 5.5 x 10–16 at 25°C. |
6.72 |
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What mass of KCl (molar mass = 74.55 g/mol) must be added to 1.0 L of 0.0180 M Pb2+(aq) to initiate precipitation of PbCl2(s)? The Ksp of PbCl2 is 1.7 x 10–5. Assume no volume change occurs upon addition of KCl. |
2.3 g |
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The following anions can be separated by precipitation as silver salts: Cl–, Br–, I–, CrO42–. If Ag+ is added to a solution containing the four anions, each at a concentration of 0.10 M, in what order will they precipitate? Compound Ksp AgCl 1.8 x 10–10 Ag2CrO4 1.1 x 10–12 AgBr 5.4 x 10–13 AgI 8.5 x 10–17 |
AgI à AgBr à AgCl à Ag2CrO4 |
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The molar solubility of silver sulfate Ag2(SO4) is 1.5 x 10-2 mol/L. What is the Ksp for this compound? |
1.4 x 10-5 |
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Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 x 10-6) solution. |
1.5 x 10-2 M |
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The Ksp for silver(I) phosphate is 1.8 x 10-18. Calculate the molar solubility of silver(I) phosphate. |
1.6 x 10-5 M |
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What is the molar solubility of Fe(OH)3(s) in a solution that is buffered at pH 2.50 at 25oC? The Ksp of Fe(OH)3 is 6.3 x 10–38 at 25°C. |
2.0 x 10–3 mol/L |
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Will a precipitate form when 50.0 mL of 1.2 x 10-3 M Pb(NO3)2 are added to 50.0 mL of 2.0 x 10-4 M Na2S? If so, identify the precipitate. |
Yes, the precipitate is PbS. |
