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| Ratio of ([products]/[reactants]) = a constant at a given T |
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Kp=Kc(RT)Δn(gas)
Δn(gas)=mol gaseous products- mol gaseous reactants |
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A ratio of terms for a given reation conststing of product concentration multiplied together and divided by reatant concentrations multiplied together, each raised to the power of their balancing coefficient
=([C]c X [D]d)/([A]a x[B]b) for aA+bB→cC+dD |
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| For nonequilibrium conditions, the expression having the same form as Kc or Kp is called the |
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| Reaction proceeds to tright as written to achieve equilibrium |
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| Reaction proceeds to left as written to achieve eqilibrium |
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| A substance that has H in its formula and dissociates in water to yield H3O+ |
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| A substance that has OH in its fomula and dissociates in water to yield OH- |
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| Acid dissociation constant (Ka) |
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Definition
An equilibrium constant for the dissociation of an acid (HA) in H2O to yield the conjgate base (A-) and H3O+
Ka=[H3O+][A-]/[HA] |
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| A disturbed system undergoes a net reaction to reattain equilibrium |
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| A proton donor, any species that donates an H+ ion |
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| A proton acceptor, any species that accepts the H+ ion |
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| formed when a base accepts a H+ from an acid |
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| of an acid is the acid minus the proton it has donated |
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| The pH range over which a buffer acts effectively; related to the relative component concentrations |
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| A measure of the ability of a buffer to resist a change in pH; related to the total concentrations and relative proportiond of buffer components |
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| A species whose color is different in acid and in base, which is used to monitor the equivalence point of a titration or the pH of a solution |
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| Kw= [H3O+][OH-]=1.0x10-14 |
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| a substance that could act as both an acid and a base |
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| The shift in the position of an ionic equilbirium away from formation of an ion that is caused by the addition (or prescence) of that ion. |
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| Kf (metal-ligand complex) |
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| Kf= [MLN]/([M][L]N) usually >>1 |
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| Henderson-Hasselbalch Equation |
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