Slide 1 : Acid-Base Titration and pH
Self-Ionization of Water : Self-Ionization of Water H2O + H2O H3O+ + OH- Though pure water is considered a non-conductor, there is a slight, but measurable conductivity due to “self-ionization”
Ion Concentration in Solutions : Ion Concentration in Solutions
Kw – Ionization Constant for Water : Kw – Ionization Constant for Water In pure water at 25 C: [H3O+] = 1 x 10-7 mol/L [OH-] = 1 x 10-7 mol/L Kw is a constant at 25 C: Kw = [H3O+][OH-] Kw = (1 x 10-7)(1 x 10-7) = 1 x 10-14
H+, OH-, and pH : H+, OH-, and pH
pH Scale : pH Scale
Calculating pH, pOH : Calculating pH, pOH pH = -log10(H3O+) pOH = -log10(OH-) Relationship between pH and pOH pH + pOH = 14 Finding [H3O+], [OH-] from pH, pOH [H3O+] = 10-pH [OH-] = 10-pOH
pH Calculations : pH Calculations
Measuring pH with wide-range paper : Measuring pH with wide-range paper
Narrow-Range pH Paper : Narrow-Range pH Paper
pH Indicators and theirranges : pH Indicators and theirranges
Some Acid-Base Indicators : Some Acid-Base Indicators
Weak Acid/Strong Base Titration : Weak Acid/Strong Base Titration A solution that is
0.10 M CH3COOH
is titrated with
0.10 M NaOH Endpoint is above pH 7
Strong Acid/Strong Base Titration : Strong Acid/Strong Base Titration A solution that is
0.10 M HCl is titrated with
0.10 M NaOH Endpoint is at
pH 7
Strong Acid/Strong Base Titration : Strong Acid/Strong Base Titration A solution that is
0.10 M NaOH is titrated with
0.10 M HCl Endpoint is at
pH 7 It is important to recognize that titration curves are not always increasing from left to right.
Strong Acid/Weak Base Titration : Strong Acid/Weak Base Titration A solution that is
0.10 M HCl is titrated with
0.10 M NH3 Endpoint is below
pH 7