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Related Concept Videos

Determining the pH of Salt Solutions04:08

Determining the pH of Salt Solutions

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The pH of a salt solution is determined by its component anions and cations. Salts that contain pH-neutral anions and the hydronium ion-producing cations form a solution with a pH less than 7. For example, in ammonium nitrate (NH4NO3) solution, NO3− ions do not react with water whereas NH4+ ions produce the hydronium ions resulting in the acidic solution. In contrast, salts that contain pH-neutral cations and the hydroxide ion-producing anions form a solution with a pH greater than 7.
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The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
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Ionic Strength: Overview01:12

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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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Ions as Acids and Bases02:54

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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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Electrolytes: van't Hoff Factor03:08

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Colligative Properties of ElectrolytesThe colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one dissolved...
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Buffers02:56

Buffers

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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...
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Balanced versus unbalanced salt solutions: what difference does it make?

Sheldon Magder1

  • 1Departments of Critical Care, Medicine and Physiology, McGill University Health Centre, 687 Pine Av W, Montreal, Quebec H3A 1A1, Canada.

Best Practice & Research. Clinical Anaesthesiology
|September 12, 2014
PubMed
Summary

Using balanced crystalloid solutions, rather than 0.9% saline, may reduce complications in critically ill patients. Further large-scale trials are needed to confirm if lower chloride concentrations improve outcomes.

Keywords:
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Area of Science:

  • Critical Care Medicine
  • Intravenous Fluid Therapy
  • Electrolyte Balance

Background:

  • Crystalloid solutions are vital for critically ill patients, maintaining fluid and electrolyte balance.
  • 0.9% saline, a common fluid, has equal sodium (Na+) and chloride (Cl-) concentrations, unlike plasma.
  • This imbalance can cause hyperchloremic acidosis, but its clinical significance is unclear.

Purpose of the Study:

  • To explore the physiological roles of Na+ and Cl- in maintaining normal body function.
  • To investigate how the gastrointestinal tract and kidneys regulate Na+ and Cl-.
  • To examine evidence supporting the use of 'balanced' crystalloid solutions over high-chloride fluids.

Main Methods:

  • Review of normal physiology concerning Na+ and Cl- roles in osmolality and acid-base balance.
  • Analysis of renal and gastrointestinal regulation of Na+ and Cl- concentrations.
  • Examination of existing evidence on the clinical impact of different crystalloid solutions.

Main Results:

  • Observational data suggest that avoiding elevated Cl- concentrations may reduce renal dysfunction, infections, and mortality.
  • Current evidence is primarily observational, indicating association rather than causation.
  • Randomized trials are limited and insufficient to establish causality.

Conclusions:

  • Avoiding high Cl- concentrations in intravenous fluids shows potential benefits in critically ill patients.
  • Large-scale randomized trials are necessary to confirm causality and clinical significance.
  • Further research is needed to determine if Cl- concentration, Na+-Cl- difference, or total Cl- mass is the key variable.