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| in an aqueous environment (solvent is water), H+ increases, pH decreases, acid gets stronger |
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| H3O+, generated by dissociated acids |
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| Electron pair acceptor, contains an empty orbital, metals, decreases pH |
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| A species of an anion and cation which completely dissociates in water to form electrolytes |
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| Gaines electrons and generates OH-, increasing the pH |
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| A species that can BOTH accept/give a proton (can become an acid and a base) (BOTH directions) |
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| A species that can EITHER give/accept multiple protons (many steps in ONE direction) |
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| Strong acids; HBr, HI, HCl, excluding HF |
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| at 25 deg celsius, Kw=1x10^-14, Kw=[H+][OH-] |
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| Ka=[A-][H+]/[HA], increase in Ka=incr. strength |
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| Kb=[BH+][OH-]/[B], increase in Kb=incr. strength |
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| increase in Ka, decrease in pKa as pKa=-log(Ka) |
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| The identity of the acid (Ka) and the ratio of acid to conj base (works best at a 1:1) |
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| a weak acid and its conjugate base |
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| Shifts toward the side with the weaker equilibrium constant (Ka or Kb) (aka weaker acid or base) |
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| What does a 1:1 concentration ratio in a buffer indicate? |
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| In an amphiprotic/polyprotic reaction... |
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