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Related Concept Videos

Phosphate Buffer01:22

Phosphate Buffer

636
The phosphate buffer system is a critical biological mechanism for maintaining pH stability in the body. This system operates primarily through two components: sodium dihydrogen phosphate (NaH2PO4), which acts as a weak acid, and sodium hydrogen phosphate (Na2HPO4), which serves as a weak base.
Sodium dihydrogen phosphate does not fully dissociate in neutral or acidic solutions. When a strong base, such as sodium hydroxide (NaOH), is introduced into the solution, sodium dihydrogen phosphate...
636
Factors Affecting Solubility04:01

Factors Affecting Solubility

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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
32.9K
Calculating pH Changes in a Buffer Solution02:45

Calculating pH Changes in a Buffer Solution

52.3K
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...
52.3K
Titration of Polyprotic Base with a Strong Acid01:18

Titration of Polyprotic Base with a Strong Acid

706
The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...
706
Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

1.7K
Titration of a polyprotic acid, which contains multiple ionizable protons, involves distinct dissociation steps, each with its own dissociation constant (Ka). Each successive Ka is weaker than the previous one. In the titration of a polyprotic acid like sulfurous acid with a strong base such as sodium hydroxide, the base first neutralizes the initial ionizable proton, forming an intermediate species (e.g., hydrogen sulfite ions). This step's titration curve resembles that of a weak...
1.7K
Buffer Effectiveness02:19

Buffer Effectiveness

48.3K
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...
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Simultaneous pH Measurement in Endocytic and Cytosolic Compartments in Living Cells using Confocal Microscopy
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Acidification of phosphate buffered saline.

Lukáš Veselý1, Behera Susrisweta1, Radim Štůsek1

  • 1Department of Chemistry, Faculty of Science, Masaryk University, Kamenice 5, 625 00 Brno, Czech Republic.

International Journal of Pharmaceutics
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Freezing significantly alters the acidity of phosphate buffered saline (PBS), impacting product stability. Understanding these pH changes is crucial for preserving frozen foods and pharmaceuticals.

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Area of Science:

  • Physical Chemistry
  • Biochemistry
  • Materials Science

Background:

  • Freezing causes acidity changes affecting frozen product stability.
  • Standard buffers are often unsuitable for freezing due to pH alterations.
  • Phosphate buffered saline (PBS) is widely used but its freezing behavior is not fully understood.

Purpose of the Study:

  • To investigate freezing-induced acidity changes in PBS.
  • To determine the influence of initial pH, concentration, and cooling rate on these changes.
  • To elucidate the mechanisms behind acidity shifts in frozen PBS.

Main Methods:

  • UV-VIS spectroscopy was employed to measure acidity in frozen PBS.
  • Experiments varied initial pH, buffer concentration, and cooling rates.
  • The impact of individual salts within PBS was assessed.

Main Results:

  • Freezing significantly alters the acidity of PBS.
  • Initial pH, concentration, and cooling rate were found to influence the extent of these changes.
  • Specific salt contributions to the observed acidity shifts were identified.

Conclusions:

  • Freezing-induced acidity changes in PBS are complex and dependent on multiple factors.
  • These findings are critical for optimizing buffer selection and formulation for frozen applications.
  • Further research into buffer mechanisms under freezing conditions is warranted.