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Questions and Answers
What is the mass in grams of solute in 37.0 mL of 5.75 x 10-4 M benzoic acid?
Why is nitric acid not used in the standardization of potassium permanganate?
What is the pH of 0.1 M nitric acid?
What is the concentration of NaOH after 5ml of 1.5g/ml NaOH is diluted with water to 15ml?
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What is the role of oxalic acid in the standardization of potassium permanganate?
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What is the difference between a solution, suspension, and precipitate?
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What is the solubility product constant (Ksp) of a salt?
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Copper(I) bromide has a measured molar solubility of 2.20x10-4 mol/L at 25°C. What is its Ksp value?
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Will NiCO3 precipitate if a solution is 1.5 x 10–6 M in Ni2+ and 6.0 x 10–4 M in CO32–, given that Ksp(NiCO3) = 6.6 x 10–9?
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A solution contains 0.001 M of KI and 0.10 M of KCl. AgNO3 is gradually added to this solution. Which forms first, solid AgI or solid AgCl?
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The formula of the compound formed by the reaction of lead and phosphate ions is [Pb].[PO4].
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The solubility of Zn(OH)2 in mg/L is 0.45 mg/L.
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The solubility product constant (Ksp) of a salt is directly proportional to the solubility of the substance.
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For a salt AaBb, the solubility product constant (Ksp) is equal to [A+]a.[B-]b.
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Oxalic acid is used as a primary standard in the standardization of potassium permanganate.
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The pOH of ammonium chloride (0.05 M) can be calculated using the formula pOH = -log[OH-].
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The reaction quotient Q is always equal to the solubility product constant (Ksp) at equilibrium.
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If the reaction quotient Q is greater than the solubility product constant (Ksp), a precipitate will always form.
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The final concentration of NaOH after dilution is 0.5 g/ml.
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For a solution containing 0.001 M of KI and 0.10 M of KCl, AgI will form first when AgNO3 is gradually added.
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Study Notes
Solution, Suspension, and Precipitate
- Solution: a homogeneous mixture where one substance is dissolved in another
- Suspension: a heterogeneous mixture where one substance is dispersed in another
- Precipitate: a solid that forms from a solution when the concentration of ions exceeds the solubility product
Solubility Product Constant (Ksp)
- Ksp: the product of the concentration of ions present in a saturated solution of an ionic compound
- For a salt AaBb: Ksp = [A+]a.[B-]b
- Ksp represents the level at which a solute dissolves in a solution
- Higher Ksp value indicates higher solubility
Examples of Ksp Calculations
- For AgCl: Ksp = [Ag+].[Cl-]
- For Pb3(PO4)2: Ksp = [Pb2+]3.[PO43-]2
- For CuBr: Ksp = [Cu+].[Br-] = 4.0x10-8 mol2/L2
- For Bi2S3: Ksp = [2X]2.[3X]3 = 1.1 x 10-73
Precipitation Reaction
- NiCO3: will not precipitate if Q < Ksp
- Reaction quotient Q = [Ni2+][CO32-]
- NiCO3 → Ni2+ + CO32-
Comparison of Ksp Values
- AgCl: Ksp = 1.6×10−10
- AgI: Ksp = 1.5×10−16
- AgI will form first in a solution with KI and KCl
Standardization of Potassium Permanganate
- Procedure: titrate oxalic acid or iron solution with potassium permanganate to the faint pink color end-point
- Standardization equation: (MV)oxalic = (MV)KMnO4 or (MV)Iron = (MV)KMnO4
Solution, Suspension, and Precipitate
- Solution: a homogeneous mixture where one substance is dissolved in another
- Suspension: a heterogeneous mixture where one substance is dispersed in another
- Precipitate: a solid that forms from a solution when the concentration of ions exceeds the solubility product
Solubility Product Constant (Ksp)
- Ksp: the product of the concentration of ions present in a saturated solution of an ionic compound
- For a salt AaBb: Ksp = [A+]a.[B-]b
- Ksp represents the level at which a solute dissolves in a solution
- Higher Ksp value indicates higher solubility
Examples of Ksp Calculations
- For AgCl: Ksp = [Ag+].[Cl-]
- For Pb3(PO4)2: Ksp = [Pb2+]3.[PO43-]2
- For CuBr: Ksp = [Cu+].[Br-] = 4.0x10-8 mol2/L2
- For Bi2S3: Ksp = [2X]2.[3X]3 = 1.1 x 10-73
Precipitation Reaction
- NiCO3: will not precipitate if Q < Ksp
- Reaction quotient Q = [Ni2+][CO32-]
- NiCO3 → Ni2+ + CO32-
Comparison of Ksp Values
- AgCl: Ksp = 1.6×10−10
- AgI: Ksp = 1.5×10−16
- AgI will form first in a solution with KI and KCl
Standardization of Potassium Permanganate
- Procedure: titrate oxalic acid or iron solution with potassium permanganate to the faint pink color end-point
- Standardization equation: (MV)oxalic = (MV)KMnO4 or (MV)Iron = (MV)KMnO4
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Description
Learn about the differences between solution, suspension, and precipitate. Understand the concept of solubility product constant (Ksp) and its calculation for ionic compounds.
