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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 83
Capitolo 17, Problema 83

Referring to Table 17.1, pick an indicator for use in the titration of each acid with a strong base. a. HFColor chart showing pH ranges for various acid-base indicators.

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Determine the pH range at the equivalence point for the titration of HF with a strong base. HF is a weak acid, and its titration with a strong base will result in a slightly basic equivalence point, typically around pH 8-9.
Refer to the provided color chart to identify indicators that change color in the pH range of 8-9.
From the chart, identify the indicators that have a color change range that includes pH 8-9. These indicators are Phenolphthalein and Thymolphthalein.
Select an indicator that has a clear and distinct color change within the pH range of 8-9. Phenolphthalein changes from colorless to pink in the pH range of approximately 8.2 to 10, making it a suitable choice.
Confirm that the chosen indicator (Phenolphthalein) will provide a clear endpoint for the titration of HF with a strong base by ensuring its color change range aligns with the expected pH at the equivalence point.

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Acid-Base Titration

Acid-base titration is a quantitative analytical method used to determine the concentration of an acid or base in a solution. It involves the gradual addition of a titrant (strong base) to a solution of analyte (weak acid) until the reaction reaches the equivalence point, where the amount of acid equals the amount of base. The endpoint is often indicated by a color change, which is facilitated by an appropriate pH indicator.
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Acid-Base Titration

pH Indicators

pH indicators are substances that change color in response to changes in pH, allowing for the visual determination of acidity or alkalinity in a solution. Each indicator has a specific pH range over which it changes color, making it suitable for different types of titrations. Selecting the right indicator is crucial for accurately identifying the endpoint of a titration, especially when titrating weak acids with strong bases.
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Acid-Base Indicators

Weak Acids vs. Strong Bases

Weak acids, like hydrofluoric acid (HF), do not completely dissociate in solution, resulting in a higher pH at the equivalence point compared to strong acids. When titrating a weak acid with a strong base, the pH at the equivalence point will be greater than 7, necessitating the use of a pH indicator that changes color in this range. Understanding the behavior of weak acids in titrations is essential for selecting the appropriate indicator from the provided table.
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Strong vs Weak Bases
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