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• Solubility product constant, Ksp


  The product of the molar concentrations of its ions in a saturated solution, each raised to the power that is the coefficient of that ion in the balanced chemical equation

  
• The more soluble a substance is, the higher the value of Ksp
• Solubility equilibrium


  When a slightly soluble ionic compound is added to water, some of it dissolves to form a solution, establishing an equilibrium between the pure solid and a solution of its ions

  
• The equilibrium expression is written without including the solid species
• Solving for Ksp


  1. Take the molarities of the products and multiply them

  2. If there are coefficients in front of any of the products, raise the product to that coefficient power (and multiply the concentration by that coefficient)

  
• Factors affecting Solubility and Ksp

  • Temperature effect: Endothermic reaction - temperature ↑, solubility ↑, Ksp ↑
  • Exothermic reaction - temperature ↑, solubility ↓, Ksp ↓
• Calculating molar solubility of BaSO4


  Given Ksp = 1.07*10-10

  
• Common ion effect


  • Addition of common ion at constant temperature:
  • Concentration of products ↑
  • Reaction shifts backward (toward reactants) to get rid of excess products
  • Reaction returns to first equilibrium state
  • Ksp remains constant

  
• Experimental work to determine Ksp of potassium acid tartrate (KHT)

  1. Aim: Determine Ksp of KHT and study effect of common ion

  2. Procedure: Prepare KCl solutions of different concentrations, add to KHT, filter, titrate filtrate with NaOH, calculate Ksp

  
• Preparation of 0.01 M KCl solution from 0.1 M KCl stock solution
• Calculating Ksp of KHT

  1. In absence of common ion: Ksp = [HT⁻] [K⁺]

  2. In presence of common ion: Ksp = [HT⁻] [K⁺ KHT + K⁺ KCl]

  
• Calculation of [K⁺]KCl
• Chemical factor


  g. of [HT⁻] ≡ 1 ml of 0.02 M of NaOH Solution