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Related Concept Videos

Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

1.8K
Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
1.8K
Calculating Equilibrium Concentrations02:05

Calculating Equilibrium Concentrations

55.6K
Being able to calculate equilibrium concentrations is essential to many areas of science and technology—for example, in the formulation and dosing of pharmaceutical products. After a drug is ingested or injected, it is typically involved in several chemical equilibria that affect its ultimate concentration in the body system of interest. Knowledge of the quantitative aspects of these equilibria is required to compute a dosage amount that will solicit the desired therapeutic effect.
A more...
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Homogeneous Equilibria for Gaseous Reactions02:15

Homogeneous Equilibria for Gaseous Reactions

30.1K
Homogeneous Equilibria for Gaseous Reactions
For gas-phase reactions, the equilibrium constant may be expressed in terms of either the molar concentrations (Kc) or partial pressures (Kp) of the reactants and products. A relation between these two K values may be simply derived from the ideal gas equation and the definition of molarity. According to the ideal gas equation:
30.1K
Calculating the Equilibrium Constant02:46

Calculating the Equilibrium Constant

39.7K
The equilibrium constant for a reaction is calculated from the equilibrium concentrations (or pressures) of its reactants and products. If these concentrations are known, the calculation simply involves their substitution into the Kc expression.
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
39.7K
Constant Pressure Calorimetry03:02

Constant Pressure Calorimetry

99.6K
Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a substance. The heat is exchanged with a calibrated and insulated device called the calorimeter. Calorimetry experiments are based on the assumption that there is no heat exchange between the insulated calorimeter and the external environment. The well-insulated calorimeters prevent the transfer of heat between the calorimeter and its external...
99.6K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

49.9K
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:
49.9K

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Updated: Mar 11, 2026

Computation of Atmospheric Concentrations of Molecular Clusters from ab initio Thermochemistry
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Computation of Atmospheric Concentrations of Molecular Clusters from ab initio Thermochemistry

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Calculated Chemistry Parameters - do they need to be harmonised?

David Hughes1, James Cg Doery2, Kay Weng Choy3

  • 1ACT Pathology, Canberra, ACT, Australia.

The Clinical Biochemist. Reviews
|November 23, 2016
PubMed
Summary
This summary is machine-generated.

Harmonizing calculated clinical chemistry parameters like osmolality, anion gap, and albumin-adjusted calcium is crucial for patient safety and data integration. Addressing terminology, formulas, and reference intervals is key to achieving this harmonization.

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Area of Science:

  • Clinical Chemistry
  • Laboratory Medicine
  • Health Informatics

Background:

  • Global initiative to harmonize clinical chemistry testing improves patient safety and data integration.
  • Harmonization efforts in Australia have primarily focused on measured analytes.
  • Calculated parameters, derived from measured analytes, also require harmonization for clinical decision-making.

Conclusions:

  • Harmonization of calculated clinical chemistry parameters is essential for robust clinical decision-making.
  • A tailored approach is necessary for each calculated parameter due to varying complexities.
  • Further investigation into specific pathways for harmonizing osmolality, anion gap, and albumin-adjusted calcium is warranted.