Skip to main content
Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblema 95d
Capitolo 17, Problema 95d

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

Guida verificata passo dopo passo
1
Determine the initial moles of the protonated form of alanine (H2A+) using the initial concentration and volume: \( \text{moles of } H_2A^+ = 0.100 \text{ M} \times 0.050 \text{ L} \).
Calculate the moles of NaOH added using its concentration and the volume added: \( \text{moles of NaOH} = 0.100 \text{ M} \times 0.075 \text{ L} \).
Determine the limiting reactant by comparing the initial moles of H2A+ and the moles of NaOH added.
Identify the species present after the reaction and their concentrations. If NaOH is in excess, calculate the concentration of OH- ions.
Use the concentration of OH- ions to calculate the pOH, and then find the pH using the relation \( \text{pH} = 14 - \text{pOH} \).

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
8m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

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 (in this case, NaOH) to a solution containing the analyte (the protonated form of alanine) until the reaction reaches its equivalence point. The pH changes during this process can be monitored to understand the acid-base behavior of the solution.
Video consigliato:
Percorso guidato
03:04
Acid-Base Titration

Acid-Base Equilibria

Acid-base equilibria describe the balance between protonated and deprotonated forms of a substance in solution. For alanine, the two dissociation constants (Ka1 and Ka2) indicate how readily it donates protons. Understanding these constants is crucial for calculating the pH at various stages of the titration, especially when determining the pH after adding specific volumes of NaOH.
Video consigliato:
Percorso guidato
02:00
Arrhenius Acids and Bases

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a way to calculate the pH of a buffer solution based on the concentrations of the acid and its conjugate base. It is expressed as pH = pKa + log([A-]/[HA]). This equation is particularly useful in titration scenarios, as it allows for the determination of pH at points where the solution contains both the protonated and deprotonated forms of the amino acid.
Video consigliato:
Percorso guidato
02:40
Henderson-Hasselbalch Equation
Pratica correlata
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

486
views
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

889
views
Domanda del libro di testo
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

380
views
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. (b) 25.0 mL (c) 50.0 mL

Domanda del libro di testo

Consider the titration of 50.0 mL of 1.00 M H3PO4 with 1.00 M KOH. Calculate the pH after the addition of each of the following volumes of base. (a) 25.0 mL (c) 75.0 mL

286
views