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Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblema 95b,c
Capitolo 17, Problema 95b,c

Consider the titration of 50.0 mL of a 0.100 M solution of the protonated form of the amino acid alanine (H2A+: Ka1 = 4.6 × 10–3, Ka2 = 2.0 × 10–10) with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of base. (b) 25.0 mL (c) 50.0 mL

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1
Determine the initial moles of H2A+ in the solution by multiplying the volume (50.0 mL) by the concentration (0.100 M). Convert the volume to liters before multiplying.
Calculate the moles of NaOH added by multiplying the volume of NaOH added (25.0 mL for part b and 50.0 mL for part c) by its concentration (0.100 M). Convert the volume to liters before multiplying.
For part (b), compare the moles of NaOH added to the initial moles of H2A+. Since 25.0 mL of NaOH is added, it is half the equivalence point, and the solution is a buffer. Use the Henderson-Hasselbalch equation to find the pH, considering the first dissociation (Ka1).
For part (c), since 50.0 mL of NaOH is added, it reaches the first equivalence point where all H2A+ is converted to HA. Calculate the pH by considering the hydrolysis of HA using the second dissociation constant (Ka2) and the concentration of HA at this point.
Use the appropriate equilibrium expressions and assumptions to solve for the pH in each case, ensuring to check if any simplifications can be made based on the relative magnitudes of Ka1 and Ka2.

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Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (a solution of known concentration) to a sample until a reaction is complete, indicated by a color change or a pH change. In this case, the titration of alanine with NaOH will help determine the pH at specific volumes of base added.
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Acid-Base Titration

Acid-Base Equilibria

Acid-base equilibria involve the balance between proton donors (acids) and proton acceptors (bases) in a solution. The dissociation constants (Ka) of the amino acid alanine indicate its ability to donate protons at different pH levels. Understanding these equilibria is crucial for calculating the pH during titration, especially when determining the point at which the amino acid transitions from its protonated to deprotonated forms.
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Arrhenius Acids and Bases

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution based on the concentration of the acid and its conjugate base. It is expressed as pH = pKa + log([A-]/[HA]). This equation is particularly useful in titration problems involving weak acids and their conjugate bases, such as alanine, as it allows for the determination of pH at various stages of the titration process.
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Henderson-Hasselbalch Equation
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Domanda del libro di testo

Consider the titration of 50.0 mL of a 0.100 M solution of the protonated form of the amino acid alanine (H2A+: Ka1 = 4.6 × 10–3, Ka2 = 2.0 × 10–10) with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of base. (e) 100.0 mL

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Domanda del libro di testo

Consider the titration of 50.0 mL of a 0.100 M solution of the protonated form of the amino acid alanine (H2A+: Ka1 = 4.6 × 10–3, Ka2 = 2.0 × 10–10) with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of base. (a) 10.0 mL

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What is the pH at the equivalence point for the titration of 0.20 M solutions of the following acids and bases? Which of the indicators in Figure 17.5 would be suitable for each titration? (c) Ba(OH)2 and HBr

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Domanda del libro di testo

Consider the titration of 50.0 mL of a 0.100 M solution of the protonated form of the amino acid alanine (H2A+: Ka1 = 4.6 × 10–3, Ka2 = 2.0 × 10–10) with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of base. (d) 75.0 mL

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What is the pH at the equivalence point for the titration of 0.10 M solutions of the following acids and bases, and which of the indicators in Figure 17.5 would be suitable for each titration? (c) CH3NH2 (methylamine) and HCl

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