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Related Concept Videos

Buffers: Buffer Capacity01:09

Buffers: Buffer Capacity

2.1K
Buffer capacity is the quantitative measure of a buffer to resist the change in pH. As shown in the following equation, the buffer capacity, denoted by 'beta', is expressed as the number of moles of acid or base needed to change the pH of a one-liter buffer solution by 1 unit. Here, Ca and Cb indicate the number of moles of acid and base, respectively. Note that dpH represents the change in pH.
In the graph, pH is plotted as a function of the number of moles of base (Cb) added to a weak...
2.1K
Buffers02:56

Buffers

171.8K
A solution containing appreciable amounts of a weak conjugate acid-base pair is called a buffer solution, or a buffer. Buffer solutions resist a change in pH when small amounts of a strong acid or a strong base are added. A solution of acetic acid and sodium acetate is an example of a buffer that consists of a weak acid and its salt: CH3COOH (aq) + CH3COONa (aq). An example of a buffer that consists of a weak base and its salt is a solution of ammonia and ammonium chloride: NH3 (aq) + NH4Cl...
171.8K
Buffer Effectiveness02:19

Buffer Effectiveness

54.7K
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...
54.7K
Buffer Systems in the Body01:19

Buffer Systems in the Body

3.5K
Chemical buffers play a critical role in the body's regulation of pH levels. These systems contain one or more compounds that stabilize pH changes by neutralizing strong acids or bases. When pH levels drop, hydrogen ions bind to a weak base; when pH levels rise, hydrogen ions are released. This dynamic process helps maintain pH within a narrow and stable range essential for normal physiological function.
A typical buffer system in bodily fluids includes a weak acid and its corresponding...
3.5K
Protein Buffers in Blood Plasma and Cells01:20

Protein Buffers in Blood Plasma and Cells

3.5K
The human body utilizes protein buffer systems to maintain a stable pH. These systems capitalize on the dual role of amino acids, which can act as acids or bases by accepting or releasing hydrogen ions in response to pH changes. Protein buffer systems are particularly significant in the extracellular fluid (ECF) and intracellular fluid (ICF) of active cells, where structural and functional proteins provide substantial buffering capacity.
Certain amino acids can exist in a zwitterion state at a...
3.5K
Phosphate Buffer01:22

Phosphate Buffer

4.6K
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...
4.6K

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Surface ocean pH and buffer capacity: past, present and future.

Li-Qing Jiang1,2, Brendan R Carter3,4, Richard A Feely4

  • 1Earth System Science Interdisciplinary Center, University of Maryland, College Park, Maryland, USA. Liqing.Jiang@noaa.gov.

Scientific Reports
|December 11, 2019
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Summary
This summary is machine-generated.

Ocean acidification, driven by carbon dioxide (CO2) absorption, threatens marine life. This study combines observational data and Earth System Models to map global ocean pH and Revelle Factor changes, aiding adaptation strategies.

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Area of Science:

  • Oceanography
  • Climate Science
  • Marine Chemistry

Background:

  • The ocean absorbs anthropogenic carbon dioxide (CO2), altering its chemistry.
  • This process, known as ocean acidification, poses a significant threat to marine ecosystems, including coral reefs.

Purpose of the Study:

  • To provide a high-resolution, regionally varying view of global surface ocean pH and Revelle Factor.
  • To project future ocean acidification trajectories from the pre-Industrial era to the end of the century.

Main Methods:

  • Combined the 6th version of the Surface Ocean CO2 Atlas (1991-2018) with an Earth System Model.
  • Utilized historical atmospheric CO2 concentrations and IPCC Representative Concentration Pathways.
  • Linked modeled pH trends with observed modern pH distribution for improved regional accuracy.

Main Results:

  • Developed a global climatology of surface ocean pH and Revelle Factor from 1750 to 2100.
  • Demonstrated that air-sea CO2 disequilibrium is the primary driver of spatial variability in surface ocean pH.
  • Highlighted contrasting spatial variability between pH and calcium carbonate saturation states.

Conclusions:

  • The integrated approach offers improved regional ocean acidification trajectories.
  • Findings will assist in developing targeted regional adaptation strategies for ocean acidification.
  • Understanding spatial variability is crucial for predicting ecosystem impacts and informing conservation efforts.