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Titration Calculations: Strong Acid - Strong Base02:28

Titration Calculations: Strong Acid - Strong Base

29.6K
Calculating pH for Titration Solutions: Strong Acid/Strong Base
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:
29.6K
pH Scale02:41

pH Scale

68.9K
Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes. Two different solutions can differ in their hydronium or hydroxide ion concentrations by a million, billion, or even trillion times. A common means of...
68.9K
Calculating pH Changes in a Buffer Solution02:45

Calculating pH Changes in a Buffer Solution

53.3K
A buffer can prevent a sudden drop or increase in the pH of a solution after the addition of a strong acid or base up to its buffering capacity; however, such addition of a strong acid or base does result in the slight pH change of the solution. The small pH change can be calculated by determining the resulting change in the concentration of buffer components, i.e., a weak acid and its conjugate base or vice versa. The concentrations obtained using these stoichiometric calculations can be used...
53.3K
Titration of a Weak Base with a Strong Acid01:20

Titration of a Weak Base with a Strong Acid

5.2K
The titration curve of a weak base like ammonia with a strong acid like hydrochloric acid is the mirror image of the titration curve of a weak acid with a strong base.
Using the ICE table and substituting the Kb value, we calculate the initial pH of 50 mL of 0.1 M ammonia to be 11.11. Addition of 25 mL of 0.1 M hydrochloric acid to this solution of ammonia results in a buffer with an equal concentration of ammonia and ammonium ions. The pH of this buffer can be calculated by substituting these...
5.2K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

44.3K
Calculating pH for Titration Solutions: Weak Acid/Strong Base
For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as:
44.3K
Buffer Effectiveness02:19

Buffer Effectiveness

49.0K
Buffer solutions do not have an unlimited capacity to keep the pH relatively constant . Instead, the ability of a buffer solution to resist changes in pH relies on the presence of appreciable amounts of its conjugate weak acid-base pair. When enough strong acid or base is added to substantially lower the concentration of either member of the buffer pair, the buffering action within the solution is compromised.
The buffer capacity is the amount of acid or base that can be added to a given volume...
49.0K

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Simultaneous pH Measurement in Endocytic and Cytosolic Compartments in Living Cells using Confocal Microscopy
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On the Validity of Constant pH Simulations.

Amin Bakhshandeh1, Yan Levin1

  • 1Instituto de Física, Universidade Federal do Rio Grande do Sul, Caixa P.O. Box 15051, 91501-970 Porto Alegre, Rio Grande do Sul, Brazil.

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Constant pH (cpH) simulations require careful charge neutrality management. This study reveals significant differences in polyelectrolyte titration curves between standard and canonical simulation methods, highlighting the importance of the correct approach.

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Area of Science:

  • Computational chemistry
  • Physical chemistry
  • Materials science

Background:

  • Constant pH (cpH) simulations are widely used for charge regulation in polyelectrolyte and colloidal systems.
  • Extending cpH methods to explicit ion/solvent systems presents challenges, particularly ensuring charge neutrality during ion exchange.
  • Existing literature often overlooks the synchronization of titration and ion insertion/deletion moves.

Purpose of the Study:

  • To investigate the challenges of constant pH (cpH) simulations in systems with explicit ions or solvents.
  • To compare titration curves obtained from standard cpH algorithms with those from exact canonical simulations.
  • To emphasize the importance of correct simulation methodologies for accurate charge regulation studies.

Main Methods:

  • Comparison of standard cpH simulation algorithms with an exact canonical simulation algorithm.
  • Implementation of synchronized titration and ion insertion/deletion moves for charge neutrality.
  • Utilizing the surface Widom insertion algorithm for pH calculation in canonical simulations.

Main Results:

  • Standard cpH simulations are inherently grand-canonical, with controlled pH reflecting the reservoir.
  • The Donnan potential significantly impacts titration curves, creating discrepancies between open and closed systems.
  • A substantial difference was observed between titration isotherms from standard cpH and canonical titration algorithms.

Conclusions:

  • The choice of simulation algorithm critically affects the accuracy of charge regulation studies.
  • Canonical simulations with correct detailed balance conditions provide a more accurate representation of titration behavior.
  • Researchers must carefully select simulation methods to correctly model polyelectrolytes, proteins, and colloidal particles.