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Explore the vocab, types of reactions, titration equations, and important points in titration involving strong/weak acids and bases. Learn to calculate concentrations and sketch titration curves effectively.
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Vocab • Titrant • Analyte • Endpoint/Equivalence point • Indicators
PhenolphthaleinFormal name: 3,3-bis(4-hydroxyphenyl)-1(3H)-isobenzofuranone, 3,3-bis(4-hydroxyphenyl)phthalide) Bronsted Acid Conj. Base (colorless, in acid) (pink, in base)
Types of Reactions • Strong Acid - Strong Base • Weak Acid - Strong Base • Strong Acid - Weak Base
1. Strong Acid - Strong Base • Example: HCl + NaOH --> • Titration Equation: Ma • Va = Mb •Vb Equivalence Pt pH = ____ If 50. mL of HCl was titrated with 0.050 M NaOH, what is the [HCl]
A 25. mL sample of HCl titrated using 50 mL of 0.050 M NaOH. Sketch this curve. pH Volume of Base Added
2. Weak Acid - Strong Base • Example: CH3COOH + NaOH --> • MV=MV pH
2. Weak Acid - Strong Base Important Points • pH = pKa when halfway to equivalence point • The formation of a conjugate base A- will make the solution BASIC at equivalence, so pH > 7
3. Weak Base - Strong Acid • Example: NH3 + HCl --> • MV=MV pH = pKb pH 12.5
3. Weak Base - Strong Acid Important Points • pH = pKb at halfway to equivalence point • The formation of a conjugate acid BH+ will make the solution ACIDIC at equivalence, so pH < 7
Titration of Diprotic Acids 2 equivalence pts