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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.18 - Aqueous Ionic EquilibriumProblema 75a
Capitolo 18, Problema 75a

Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.
(i) Which acid solution is more concentrated?

Guida verificata passo dopo passo
1
Step 1: Understand that a titration curve shows the pH of a solution as a function of the amount of titrant (in this case, NaOH) added. The shape of the curve can provide information about the acid being titrated.
Step 2: The initial pH of the solution before any NaOH is added is determined by the concentration and strength of the acid. A higher initial pH indicates a weaker acid or a less concentrated solution.
Step 3: The point at which the pH starts to rise significantly is called the equivalence point. This is when all the acid has reacted with the NaOH. The volume of NaOH needed to reach the equivalence point is directly related to the concentration of the acid.
Step 4: Compare the two titration curves. The curve that reaches the equivalence point with a smaller volume of NaOH corresponds to a less concentrated acid solution.
Step 5: Therefore, the acid solution that requires a larger volume of NaOH to reach the equivalence point is more concentrated.

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Titration Curves

Titration curves graphically represent the pH of a solution as a function of the volume of titrant added. For weak acids, the curve typically shows a gradual increase in pH, followed by a steep rise at the equivalence point. The shape and position of the curve can provide insights into the concentration and strength of the acids being titrated.
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Acid-Base Titration Curves

Weak Acids and Their Concentration

Weak acids partially dissociate in solution, meaning that not all acid molecules release protons (H+). The concentration of a weak acid affects the initial pH and the steepness of the titration curve. A more concentrated weak acid will generally have a lower initial pH and a more pronounced change in pH near the equivalence point compared to a less concentrated solution.
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Calculating Percent Ionization of Weak Acids

Equivalence Point

The equivalence point in a titration is reached when the amount of titrant added is stoichiometrically equivalent to the amount of substance in the solution being titrated. For weak acids titrated with a strong base like NaOH, the equivalence point is characterized by a rapid increase in pH. Analyzing the position of this point on the titration curve can help determine the concentration of the acid.
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At the Equivalence Point
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A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence point, 40 mL, 50 mL. Sketch the titration curve.

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A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 40 mL.

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A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl. Calculate the pH at each volume of added acid: 50 mL.

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Consider the titration curves (labeled a and b) for two weak bases, both titrated with 0.100 M HCl. (a)


(b)

(ii) Which base has the larger Kb?

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Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.

(ii) Which acid has the larger Ka?

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