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| claculating concentrations when given the starting amounts of products and 1 ending amount |
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Definition
step 1 ice table
step 2 get rid of solids and liquids
step 3 solve for concentrations using ending amounts as x |
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Definition
| Kc=([C]^c[D]^d)/([A]^a[B]^b) |
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| find Kc using the sum of 2 reactions |
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Definition
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Definition
| partial pressure constant(Kc(RT)^change n) |
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Definition
| is an equilibrium involving reactants and products in more than one phase ex gas+liquid--->gas+solid(liquids and solids get negated when solving for equilibrium) |
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Definition
| Products are favoured in reaction |
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Definition
| Reactants are favoured in the reaction |
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Definition
| neither products or reactants are favoured |
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Definition
[Ci]^c[Di]^d)/([Ai]^a[Bi]^b)
Qc concentrations at a particular time in the reaction |
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Definition
| Reactions moves to left to reach equilibirum |
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Term
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Definition
| reaction is at equalibirum |
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Term
| find concentrations when given conc at a particular time and Kc |
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Definition
Step 1 determine Qc
step 2 form ice table based on shift of equation
step 3 solve for x with ice table |
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Term
| 3 steps to solve for equilbrium concentrations |
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Definition
step 1 set up ice table(exclude liquids and solids)
step 2 substitue the expression in x for equalibrium cncentrations into Kc
step 3 solve the equilbrium constant equation for the values needed |
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Term
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Definition
| effects concentrations, doesnt change Kc, reaction shifts to the side with less moles of gas |
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Term
| increase in temperature(T) |
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Definition
| Kc changes depending on reaction |
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Term
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Definition
| K doesnt change, reaction reaches equilbrium faster |
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Term
| solve: you are at equilbrium and add more of product/reactant |
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Definition
step 1 calculate Qc and compare to Kc
step 2 use shift for ice table
step 3 solve for concentrations |
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Definition
| substance that increase the concentration of H+ ion(H3O+) |
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Term
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Definition
| substance that increases OH- ion |
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Term
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Definition
completely ionizes in water to give OH- and cation
ex NaOH |
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Term
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Definition
completely ionizes to creat H+ and anion
ex HCl |
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Term
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Definition
| is the species donating a proton |
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Term
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Definition
| species accepting a proton |
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Definition
| 2 species that differ only by the amount of H+ ions NH3 NH4+ |
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Definition
| species that can act as an acid or a base H2O |
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Definition
| is a species that can form a covelant bond by accepting an electron pair from another species ex H+ |
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Term
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Definition
| is a species that can form a covalent bond by donating an electron pair to another species NH3 |
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Term
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Definition
acid-loses proton easily
base- holds proton strongly(creates strong bond) |
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Term
| conjugate strength of strong acid/base |
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Definition
| strength of acid/base is weak |
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Term
| determine strength of H bonded acids |
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Definition
| as you move across the periodic table electronegativity increases, H-x bond polarity increases, and the acid strength increases |
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Term
| Oxic acids(H-O-Y) determine strength? |
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Definition
| as electronegativity of Y increases strength increases |
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Term
| for and (OH)mYOn strength? |
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Definition
| the highe n(number of oxygen molecules not bonded to OH) increases strength increases |
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Term
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Definition
| ion product constant for water (1.0*10^-14=[H3O][OH-]) |
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Term
| calculate concentrations of hydronium and hydroxide ions when given acid/base concentration |
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Definition
step 1 substitue for H3O or OH
step 2 solve using Kw forumla using 1.0*10^-14 |
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Definition
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Definition
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| find PH given POH or vice versa |
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