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24 Cards in this Set
- Front
- Back
Galvani potential
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Ionic strength
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Electrochemical potential
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Debye huckel limiting law
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Mean activity coefficient
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Nernst equation
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Equilibrium constant
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Gibbs energy
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Natural log of equilibrium constant
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Standard potential (anode and cathode)
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Mean activity coefficient for any salt
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Activity
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Redox electrode
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Pt (s) with aqueous ions of differing charge
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Stern model
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Series combination of helmholtz and diffuse layers.
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As the concentration of the electrolyte increases:
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Thickness of the diffuse layer decreases
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Metal/insoluble salt electrode
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Solid metal coated in soluble salt in aqueous solution
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Metal/metal ion electrode
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Solid metal in aqueous solution of ions
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Gas electrodes
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Solid platinum in aqueous acid solution with hydrogen gas
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Galvanic cell
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Spontaneous reaction at electrodes
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How do pH meters work?
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Higher conc of H+ in the analyte and therefore the hydrated glass causes Na+ ions to diffuse across the glass and push H+ ions from the hydrated glass into the buffer - increasing the activity of the buffer and causing a lower pH
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Example of a pH electrode
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Ag (s) |AgCl (s) | KCl (aq) || analyte | glass | buffer | NaCl (aq) | AgCl (s) | Ag (s)
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How do pH meters work?
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Higher conc of H+ in the analyte and therefore the hydrated glass causes Na+ ions to diffuse across the glass and push H+ ions from the hydrated glass into the buffer - increasing the activity of the buffer and causing a lower pH
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Helmholtz layer model
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Surface charge compensated by a fixed sheet of ions at the outer helmholtz layer
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Gouy-Chapman model
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Surface charge counterbalanced by a dynamic ionic atmosphere - diffuse layer
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