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TITRIMETRY ANALYSIS - Coggle Diagram
TITRIMETRY ANALYSIS
Water Dissociation and pH
Kw = [H+][OH-] = 1 x 10^-14 at 25 °C
pH = -log[H+]
pOH = -log[OH-]
pH + pOH = 14 at 25 °C
pKa = -log Ka
pKb = -log Kb
Ka x Kb = Kw
Titration Calculations
Write balanced chemical equation
Calculate moles: n = MV (V in litres)
Use stoichiometric mole ratio
Determine limiting and excess reagents
Identify products and remaining substances
Calculate pH of the resulting solution
Titrimetry
Quantitative analytical technique
Determines concentration using a known-concentration solution and measured volume
Titrant: known concentration
Analyte: substance being analysed
Equivalence point: reactants have reacted according to stoichiometric ratio
Types of Titration
Strong acid + strong base
Weak acid + strong base
Equivalence point
Reactants match the stoichiometric ratio
After equivalence point
Check excess reagent before calculating pH
Main Purposes
Determine analyte concentration
Determine pH after titrant is added
Identify limiting reagent, excess reagent and products
Acid-Base Theories
Arrhenius
Acid produces H+ / H3O+ in water
Base produces OH- in water
Bronsted-Lowry
Acid donates H+
Base accepts H+
Conjugate acid-base pairs
Lewis
Acid accepts an electron pair
Base donates an electron pair
Types of Acids and Bases
Strong acid/base: completely dissociate
Weak acid/base: partially dissociate
pH of Acids and Bases
Strong acids/bases
Completely dissociate
Determine pH from [H+] or [OH-]
Weak acids/bases
Partially dissociate
Use equilibrium concentrations / ICE table