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  2. Sodium nitrate - Wikipedia

    en.wikipedia.org/wiki/Sodium_nitrate

    Sodium nitrate is the chemical compound with the formula Na N O 3.This alkali metal nitrate salt is also known as Chile saltpeter (large deposits of which were historically mined in Chile) [4] [5] to distinguish it from ordinary saltpeter, potassium nitrate.

  3. Dissociation (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Dissociation_(chemistry)

    The higher the percentage, the stronger the electrolyte. Thus, even if a substance is not very soluble, but does dissociate completely into ions, the substance is defined as a strong electrolyte. Similar logic applies to a weak electrolyte. Strong acids and bases are good examples, such as HCl and H 2 SO 4. These will all exist as ions in an ...

  4. Aqueous solution - Wikipedia

    en.wikipedia.org/wiki/Aqueous_solution

    The ability for ions to move freely through the solvent is a characteristic of an aqueous strong electrolyte solution. The solutes in a weak electrolyte solution are present as ions, but only in a small amount. [3] Nonelectrolytes are substances that dissolve in water yet maintain their molecular integrity (do not dissociate into ions).

  5. Electrolyte - Wikipedia

    en.wikipedia.org/wiki/Electrolyte

    An electrolyte in a solution may be described as "concentrated" if it has a high concentration of ions, or "dilute" if it has a low concentration. If a high proportion of the solute dissociates to form free ions, the electrolyte is strong; if most of the solute does not dissociate, the electrolyte is weak.

  6. Supporting electrolyte - Wikipedia

    en.wikipedia.org/wiki/Supporting_electrolyte

    A supporting electrolyte, in electrochemistry, according to an IUPAC definition, [1] is an electrolyte containing chemical species that are not electroactive (within the range of potentials used) and which has an ionic strength and conductivity much larger than those due to the electroactive species added to the electrolyte.

  7. Ionic strength - Wikipedia

    en.wikipedia.org/wiki/Ionic_strength

    The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.

  8. ‘A minefield of its own making’: New investigation of USAA ...

    www.aol.com/finance/minefield-own-making...

    Starting in 2019, USAA has also faced a number of fines — $3.5 million over customer-related violations, $85 million over compliance and management issues and $140 million over weak protections ...

  9. Molar conductivity - Wikipedia

    en.wikipedia.org/wiki/Molar_conductivity

    The limiting molar conductivity of a weak electrolyte cannot be determined reliably by extrapolation. Instead it can be expressed as a sum of ionic contributions, which can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. For aqueous acetic acid as an example, [4]