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Acid/Base Strengths and Dissociation Constants03:02

Acid/Base Strengths and Dissociation Constants

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The relative strength of an acid or base is the extent to which it ionizes when dissolved in water. If the ionization reaction is essentially complete, the acid or base is termed strong; if relatively little ionization occurs, the acid or base is weak. There are many more weak acids and bases than strong ones. The most common strong acids and bases are listed below:
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Strong Acid and Base Solutions03:22

Strong Acid and Base Solutions

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A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
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The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution...
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Brønsted-Lowry acid-base chemistry is the transfer of protons; thus, logic suggests a relation between the relative strengths of conjugate acid-base pairs. The strength of an acid or base is quantified in its ionization constant, Ka or Kb, which represents the extent of the acid or base ionization reaction. For the conjugate acid-base pair HA / A−, the ionization equilibrium equations and ionization constant expressions are
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Ions as Acids and Bases02:54

Ions as Acids and Bases

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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:
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Ionic Association01:28

Ionic Association

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The ionic association is the association of oppositely charged ions in an electrolyte solution to form ion pairs. Bjerrum defined ion pairs as two oppositely charged ions whose electrostatic attraction exceeds the thermal energy of the system, typically expressed as 2kT. Electrostatic attraction depends on ionic charge, separation distance, and the dielectric constant of the medium. Thermal energy, represented by kT, reflects the tendency of ions to move independently due to molecular motion.
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Base excess, strong ion difference, and expected compensations: as simple as it is.

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Summary

This review compares three methods for interpreting acid-base disorders. The anion gap and expected compensation approach is most practical for clinicians at the bedside.

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Area of Science:

  • Clinical Chemistry
  • Internal Medicine
  • Critical Care Medicine

Background:

  • Blood gas analysis has evolved from a purely chemical measurement to a clinically applicable tool.
  • Understanding acid-base disorders is crucial for patient management.

Purpose of the Study:

  • To compare the three most common diagnostic approaches for interpreting acid-base disorders.
  • To provide practical insights for clinicians.

Main Methods:

  • Literature review of key publications on acid-base disorder interpretation.
  • Comparative analysis of diagnostic methodologies: base-excess, Stewart approach, and anion gap/expected compensation.

Main Results:

  • All three diagnostic strategies are deemed acceptable.
  • Base-excess calculation may be too simplistic for mixed disorders.
  • The Stewart approach, while chemically sound, is complex for emergency physicians.
  • The anion gap and expected compensation method is comprehensive and bedside-feasible.

Conclusions:

  • The anion gap and expected compensation approach offers a practical and comprehensive method for bedside interpretation of acid-base disorders.
  • Clinicians should be aware of the strengths and limitations of each diagnostic strategy.