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Related Concept Videos

Ions as Acids and Bases02:54

Ions as Acids and Bases

26.2K
Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
26.2K
Acidity and Basicity of Carboxylic Acid Derivatives01:25

Acidity and Basicity of Carboxylic Acid Derivatives

4.2K
Carboxylic acids are the strongest among organic acids, as they readily lose the hydroxyl proton to form a resonance-stabilized carboxylate ion. In comparison, the acid derivatives lack acidic hydrogens directly attached to a functional group. In these compounds, the acidic nature arises from their ability to lose α hydrogens, making them weakly acidic.
The relative acidic strength of the derivatives can be explained based on the extent of resonance stabilization of the conjugate base. The...
4.2K
Acidity and Basicity of Alcohols and Phenols02:36

Acidity and Basicity of Alcohols and Phenols

22.1K
Like water, alcohols are weak acids and bases. This is attributed to the polarization of the O–H bond making the hydrogen partially positive. Moreover, the electron pairs on the oxygen atom of alcohol make it both basic and nucleophilic. Protonation of an alcohol converts hydroxide, a poor leaving group, into water—a good one. The two acid–base equilibria corresponding to ethanol are depicted below.
22.1K
Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

57.9K
The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
57.9K
Lewis Acids and Bases02:33

Lewis Acids and Bases

48.2K
In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.
A coordinate covalent bond (or dative bond) occurs when one of the atoms in the bond provides both bonding electrons. For example, a coordinate covalent bond occurs when a water molecule combines with a hydrogen ion to form a hydronium ion. A coordinate covalent bond also results when...
48.2K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

49.1K
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:
49.1K

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A Polyaniline-based Sensor of Nucleic Acids
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Acid-Base Basics.

Michael F Romero1, Adam J Rossano1

  • 1Physiology and Biomedical Engineering, Nephrology and Hypertension, Mayo Clinic College of Medicine and Science, Rochester, MN.

Seminars in Nephrology
|July 14, 2019
PubMed
Summary
This summary is machine-generated.

This study reviews fundamental concepts of biological buffering and acid-base balance, crucial for understanding physiological processes and medical treatments. It highlights new genetically encoded pH indicators for advanced research applications.

Keywords:
CO(2)/HCO(3)(-) bufferingGEpHIIntracellular pHammonium pulsegenetically encoded pH indicatorpH buffering

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Area of Science:

  • Physiology
  • Biochemistry
  • Medical Science

Background:

  • Buffering and acid-base transport are fundamental in biology but often underemphasized.
  • These principles are critical for understanding physiology, nephrology, pulmonology, and anesthesiology.
  • Mechanistic understanding, medical treatments, and therapy assessment rely on these concepts.

Purpose of the Study:

  • To provide an overview of basic science acid-base concepts and buffer transport.
  • To introduce tools for monitoring intracellular pH and modeling cellular responses to pH changes.
  • To discuss the development and application of genetically encoded pH indicators.

Main Methods:

  • Review of basic chemistry and transport of buffers and acid-base equivalents.
  • Outline of fundamental acid-base concepts.
  • Description of tools for intracellular pH monitoring and cellular response modeling.
  • Introduction to genetically encoded pH indicators (pHerry, pHire).

Main Results:

  • Genetically encoded pH indicators offer new avenues for research.
  • These indicators have demonstrated utility in in vitro, ex vivo, and in vivo experiments.
  • Continued development enhances opportunities for basic and clinical investigations.

Conclusions:

  • Understanding biological buffering and acid-base balance is essential for various medical fields.
  • Genetically encoded pH indicators represent a significant advancement in pH monitoring technology.
  • These tools facilitate deeper insights into physiological processes and potential clinical applications.