Precipitation Titration and Solubility Product Constant
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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?

  • 0.0675 g
  • 0.0875 g
  • 0.0495 g
  • 0.04335 g (correct)

Why is nitric acid not used in the standardization of potassium permanganate?

  • It is not a suitable indicator
  • It is a weak acid
  • It reacts with potassium permanganate
  • It is a strong oxidizing agent (correct)

What is the pH of 0.1 M nitric acid?

  • 1.3
  • 1.7
  • 1 (correct)
  • 2.1

What is the concentration of NaOH after 5ml of 1.5g/ml NaOH is diluted with water to 15ml?

<p>0.5 g/ml (C)</p> Signup and view all the answers

What is the role of oxalic acid in the standardization of potassium permanganate?

<p>It is a reducing agent (B)</p> Signup and view all the answers

What is the difference between a solution, suspension, and precipitate?

<p>A solution is a homogeneous mixture, a suspension is a heterogeneous mixture, and a precipitate is a solid formed from a solution. (A)</p> Signup and view all the answers

What is the solubility product constant (Ksp) of a salt?

<p>The product of the concentration of the ions that are present in a saturated solution of an ionic compound. (D)</p> Signup and view all the answers

Copper(I) bromide has a measured molar solubility of 2.20x10-4 mol/L at 25°C. What is its Ksp value?

<p>4.0x10-8 mol2/L2 (B)</p> Signup and view all the answers

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?

<p>No, because the reaction quotient Q is less than Ksp. (A)</p> Signup and view all the answers

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?

<p>Solid AgI, because Ksp(AgI) is less than Ksp(AgCl). (C)</p> Signup and view all the answers

The formula of the compound formed by the reaction of lead and phosphate ions is [Pb].[PO4].

<p>True (A)</p> Signup and view all the answers

The solubility of Zn(OH)2 in mg/L is 0.45 mg/L.

<p>False (B)</p> Signup and view all the answers

The solubility product constant (Ksp) of a salt is directly proportional to the solubility of the substance.

<p>True (A)</p> Signup and view all the answers

For a salt AaBb, the solubility product constant (Ksp) is equal to [A+]a.[B-]b.

<p>True (A)</p> Signup and view all the answers

Oxalic acid is used as a primary standard in the standardization of potassium permanganate.

<p>True (A)</p> Signup and view all the answers

The pOH of ammonium chloride (0.05 M) can be calculated using the formula pOH = -log[OH-].

<p>True (A)</p> Signup and view all the answers

The reaction quotient Q is always equal to the solubility product constant (Ksp) at equilibrium.

<p>False (B)</p> Signup and view all the answers

If the reaction quotient Q is greater than the solubility product constant (Ksp), a precipitate will always form.

<p>True (A)</p> Signup and view all the answers

The final concentration of NaOH after dilution is 0.5 g/ml.

<p>True (A)</p> Signup and view all the answers

For a solution containing 0.001 M of KI and 0.10 M of KCl, AgI will form first when AgNO3 is gradually added.

<p>False (B)</p> Signup and view all the answers

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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Learn about the differences between solution, suspension, and precipitate. Understand the concept of solubility product constant (Ksp) and its calculation for ionic compounds.

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