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  1. Nov 2025
  2. chem.libretexts.org chem.libretexts.org
    19.5: Standard Electrochemical Potentials
    1
    1. claytonw 17 Nov 2025
      Figure 19.5.3: he Standard Hydrogen Electrode. The SHE consists of platinum wire that is connected to a Pt surface in contact with an aqueous solution containing 1 M H+ in equilibrium with H2 gas at a pressure of 1 atm. Note, the SHE can act as either an Anode or Cathode.

      Note that Pt is absent from the full redox rxn and the resulting half rxn. Don't accidentally get confused Pt is just the surface the redox rxn is occurring on (its interion differentiates its status as not being apart of the "reactants" or "productions").

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    chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1403:_General_Chemistry_2/Text/19:_Electron_Transfer_Reactions/19.05:_Standard_Electrochemical_Potentials
  3. chem.libretexts.org chem.libretexts.org
    19.3: Electrochemical Cells
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    1. claytonw 17 Nov 2025
      The moment current flows [Zn+2] increases while the [Cu+2] decreases and this can be seen by the images in part (b) of figure 19.2.3 as the Zinc anode dissolves and copper ions attach themselves to the electrode and become reduced to neutral copper.

      The moment current flows [Zn+2] increases while the [Cu+2] decreases and this can be seen by the images in part (b) of figure 19.2.3 as the Zinc anode dissolves and copper ions attach themselves to the electrode and become reduced to neutral copper.

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    2. claytonw 17 Nov 2025
      he moment current flows [Zn+2] increases while the [Cu+2] decreases and this can be seen by the images in part (b) of figure 19.2.3 as the Zinc anode dissolves and copper ions attach themselves to the electrode and become reduced to neutral copper.

      Not sure if this is clear to all but in the case it is not the resulting image on the right (b) shows the anode, or Zn, thinning down as ions enter the solution. The reason for the "fuzziness" or "spikeyness" on the Cu cathode is due to the formation of Copper crystals from electrons in solution.

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  4. chem.libretexts.org chem.libretexts.org
    19.1: Electrical Fundamentals
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    1. claytonw 14 Nov 2025
      Note: E is not energy but electric potential. (19.1.7)W=q⋅Δ⁢E

      The reasoning behind this is because it represents the amount of energy per given unit charge (In this case Coulombs, but Joule / Volt could work too). A great analogy I saw online because this topic can be confusing for intro to electrochemistry is the height analogy. That is an object on a high ledge does not have any kinetic energy but rather potential energy (the unit here being per g or lb that increases with increased potential energy).

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  5. Oct 2025
  6. chem.libretexts.org chem.libretexts.org
    17.2: Controlling pH- Buffer Solutions
    2
    1. claytonw 22 Oct 2025
      Note, like any logarithm, you can write this in the log form, on in the power form (17.2.15)[A−][H⁡A]=10p⁢H−p⁢K⁢A

      Notice that the way the equation solves that with the solved value. If 10^pH-pKA is greater than 1, the Conjugate Base or [A-] is in higher concentration than the lewis acid [HA], alternatively an increased HA concentration means a larger denominator --> 10^pH-pKA closer to 0; Conjugate Acid is higher in concentration.

    2. claytonw 22 Oct 2025
      Mix a weak acid (or base) with a soluble salt of its conjugate.

      In order to obtain a buffer, the complete neutralization of either the acid or the base must be avoided. Thus weak acids are used (and my guess no strong bases as well) because the complete dissociation of its ions would prevent the suspension of the pH.

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    chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1403:_General_Chemistry_2/Text/17:_Aqueous_Equilibria/17.02:__Controlling_pH-_Buffer_Solutions
  7. chem.libretexts.org chem.libretexts.org
    16.3: Equilibrium Constants for Acids and Bases
    2
    1. claytonw 10 Oct 2025
      and we can calculate pOH for a weak acid

      This formula is similar to the pH formula of a weak acid given its H+ concentration. This likely means due to the logarithmic nature that a hypothetical titration curve could be plotted with similarly its H+ concentration to that of its OH- concentration (logarithmic relationship).

    2. claytonw 10 Oct 2025
      So we can define the percent ionization of a weak acid as (16.3.36)%I=[A−][H⁡A]i⁢(100)

      This formula will tell you the amount of A- Ions in solution, note that this formula is for a monoprotic weak acid (less it also applies to di+)?

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    chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1403:_General_Chemistry_2/Text/16:_Acids_and_Bases/16.03:_Equilibrium_Constants_for_Acids_and_Bases