Term
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Definition
| once reaction has reached equalibrium, the greater concentration is on the product side |
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Term
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Definition
| once the reaction has reached equalibrium the concentration is on the reaction side |
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Term
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Definition
- changes with temperiture
- changes when stoichiometric coefficients change
- changes when reaction is reversed
- Remains the same when different concentrations are used.
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Term
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Definition
| used to determine concentrations |
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Term
| equalibrium consintration expression |
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Definition
- all concentrations are at equlibrium values
- product concentrations appear in the numerator, and the reactant concentrations appear in the denominator
- each concentration is reised to the power of it's stoichiometric coefficient in the balanced chemical equation
- the value of the contant K depends on the particular reaction and the temperature
- units are never given with K
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Term
| never included in equilibirum expression? |
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Definition
- solid reactants and products
- molar concentration of water
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Term
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Definition
Product favored at equalibirum.
strong acid/bases
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Term
| completion in regards to a reaction |
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Definition
| essentially all have been converted to water it was sapouse to. |
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Term
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Definition
| reaction is reactant- favored at equilibrium |
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Term
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Definition
| at an point as the reaction proceeds from the reactants to an equailibrium mixtrue. |
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Term
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Definition
| reactants must be converted to products for equilibruim |
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Term
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Definition
| some products must be converted to reactants for equilibrium |
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Term
| short cut to solving equalibrium concentration equation |
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Definition
if 100 * K < 2 order of magnetude than initial product [A], then the denominator x can be removed.
k = [B][C]/[A]
K = xx/A-x
K= xx/A |
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Term
| what is the equilibrium constant for the new K when there are new stoichiometirc ratio's? |
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Definition
| it is the old K raised to the power of the miltiplication factor of the stoichiometric number |
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Term
| what happens to K when the chemical equation is revervsed? |
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Definition
| the new K is the reciprocal of the old K |
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Term
| how is the new K found when adding two reactions together? |
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Definition
| The two K's are multiplied to find the new K |
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Term
| how is the equalibrium constant disturbed? |
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Definition
- temperature
- change in concentration
- change in volume
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Term
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Definition
| how reaction will adjust to the quantities of reactants and products so that equilibtium is restored |
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Term
| what side will equilibrim favor of a gass reaction when volume is increased? |
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Definition
| the side with more molecules |
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Term
| what side will an equilibrium favor of a gass reaction when volem is decreesed? |
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Definition
| the side with the smallest number of gass molecules |
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Term
| what happens to the energy flow when the reaction is heated |
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Definition
| the energy is obsorbed meaning it is endothermic |
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Term
| Arrhenius definition of an acid and base |
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Definition
| any substance that when dissolved in water increases the concentration of H+ ions is an acid. any substance that increases the concentration of hydroxid ion is a base |
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Term
| Bronsted - Lowery definition of acid and base |
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Definition
| acid is a proton donar and a base is a proton acceptor |
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Term
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Definition
| capable of donation one proton |
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Term
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Definition
| capable of donating many protons |
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Term
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Definition
| ions that can behave either as bronsted acids ro bases |
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Term
| all polyatomic ions are ....... when it comes to donating hydtrgen ions |
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Definition
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Term
| conjugate acide base pair |
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Definition
| consits of two species that differ from each other by the presence of one hydrogen ion |
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Term
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Definition
| water is composed of some H3O and some OH, it is never not conducting electricity |
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Term
| what is the equalibrium constant for water at 25 degrees C |
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Definition
| Kw = [H3O+][OH-] = 1 * 10-14 |
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Term
| autoionization constant for water |
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Definition
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Term
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Definition
[H3O+] = [HO-]
both are equal to 1 * 10-7 |
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Definition
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| the some of pH and pOH must be equal to 14 at 25 degrees C |
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Term
| why is the some of pH and pOH always equal to 14? |
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Definition
| Adding acid reaises the concentration of the H3O+ ions so the solution is acidic. to oppose this increase, Le Chatelier's principle predicts that a small fraction of the H3O+ ions will react with OH- ions from whater autoionization to form water, lowering OH until the product of H3O and OH is again eqaul |
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Term
| how do you define relative strengths of acids? |
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Definition
| measure the oH of soutions of acids of equal concentrations, the lower the pH the greater the concentration of hydronium ions |
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Term
| what does a large Ka mean? |
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Definition
- ionization products strongly favored
- strongest acids
- small Kb
- all of these aplly to basses
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Term
| what happens to the stregnth of Ka and conjuagate Kb when the molicule has a big organic tail? |
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Definition
the Ka ( acidity ) decreases
the conjugate Kb increases |
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Term
| how do polyprotic acids ionize? |
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Definition
| they are broken down into steps |
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Term
| what happens to the K aspolyprotic acids are ionzed? |
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Definition
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Term
| why does k become smaller as more H+ are being pulled off? |
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Definition
| Because it is getting harder and harder to remove H+ ions. the larger the negative chager the more difficult it is to remove H+ |
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Term
| anions that are conjugate bases of strong acids have what kind of effect on the pH |
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Definition
| they are such weak bases that they have no effect on pH solution |
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Term
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Definition
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Term
| how do alkali metal and alaline earth cations effect pH of solution? |
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Definition
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Term
| what are acidic cations limited to? |
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Definition
| metal ations with 2+ or 3+ charges and to ammonium ions |
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Term
| all metal ions are what in water |
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Definition
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Term
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Definition
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Term
| relationship among pK values |
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Definition
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Term
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Definition
| the product of Ka for an acie and Kb for its conjugate base is euql to the constant specifically Kw |
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Term
| what side does the equalibrium fall on? |
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Definition
| the side with the weeker base or acid |
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Term
| how do all proton transfer reactions proceed? |
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Definition
| from the stronger acid and base to the weaker acid and base |
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Term
| what is the net ionic equation for strong base and acid? |
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Definition
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Term
| what are the products of a hydrolsys reaction? |
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Definition
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Term
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Definition
| the cantstant for finding the parsail pressures |
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Term
| Is a conj. acid/base considered to be an acid or a base when looking it up in table 17.4? |
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Definition
| is it is a conj. acid it is considered to be an acid when looking at table 17.4. |
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Term
| what happens when equal number of moles of a strong base is mixed with an equal number of a weak acid? |
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Definition
| The solution is basic with the pH depending on Kb |
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Term
| mixing strong acid and strong base? |
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Definition
| produces a neutroal solution |
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Term
| mixing equal number of moles of strong acid with weak base ? |
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Definition
| produces an acidic solution with pH depending on Ka |
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Term
| what happens when acetic acid (CH3CO2H) a weak acid is mixed with ammonia (NH3)? and why |
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Definition
The solution is neutraul because the pH depends both of the products formed and both products have a Ka and a Kb That are equal. |
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Term
| what happens when mixing weak ka and kb values? |
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Definition
| the pH depends on the relative Ka and Kb values |
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Term
| how is the pH effected by the inorganic polyptotic acids/bases? |
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Definition
| the pH is many effected by the release of the first H+ ion and not so much by the second |
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Term
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Definition
| is a substance that can accept a pair of electrons from another atom to form a new bond |
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Term
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Definition
| is a substance that can donate a pair of electrons to another atom to form a new bond |
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Term
| acid-base adduct (coordinate covalent bond) |
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Definition
| the product of a lewis acid base reaction |
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Term
| list some moecules that have both strong acid and strong base |
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Definition
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Term
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Definition
has a lot of atoms attached to it with a charge
[Co(H20)4Cl2]+ |
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Term
| when given two Ka's for a reactions how is the equalibrium constant found? |
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Definition
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Term
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Definition
| condition in which forward rate of reaction equals reverse rate |
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Term
| at equilibirum was does the forward and the reverse rate of the reaction equal? what is that called? |
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Definition
| the forward rate equals the reverse rate. that is where we get the equilibrium constant from? |
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Term
Typical steps to this cacluation:
what are the equilbirum concentrations give the about of reactant formed and what is the equilibirum constant? |
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Definition
1:set up ICE table
2: solve for x
3: caclulate K by the equilbrium constant equation |
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Term
| What happens to K when T increases? |
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Definition
| The K increases when T increases. When K increases that means that it favors the products. |
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Term
| what constitutes a strong acid? |
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Definition
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Term
strong or week acid/ base
acetic acid |
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Definition
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Term
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Definition
buffers always consist of weak acid and conjugate base
or
weak base and conjugate acid |
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Term
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Definition
| example of LaChatelier's Principle: a perturbation to a system at equilibirum leads to achisft in the equilibrium that offsets, or minimizes the effect of the perturbation. |
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Term
| what is the buffer or HF? |
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Definition
| hydrofluoric acid (weak acid HF) and sodium flouride (conj. base F-) |
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Term
| what is the buffer system for acetic acid? |
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Definition
| acetic acid (CH3COOH week acid) and sodium acetate ( CH3COO conj. bAse) |
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Term
| equivalence point of strong acid/ base? |
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Definition
| is always going to be at 7 pH |
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Term
| the equivalence point of a weak acid with a strong base? |
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Definition
| the ph is controlled by the conjugate base of the acid. |
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Term
| weak acid and strong base have the same consentration |
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Definition
| means the pka is = to the ph in a titration |
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Term
| what is the ph of a weak acid and a strong base at the equivalancy point? |
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Definition
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Term
| whem is a substance predicted to be more soluble then ksp value? |
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Definition
| when a salt is the conj. baske of weak acd is there and an |
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Term
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Definition
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Term
| will a small or large Ksp precipitate first? |
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Definition
| a small Ksp will presipitate first because it has a larger Kf value. |
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Term
| how would you calculate the Knet for the disosiation of a solid and an acid? |
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Definition
| you would findthe Ksp and Kform and multiply them |
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Term
| when are kc and Kp the same? |
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Definition
when the number of moles of a gaseous reactiant and product are the same
number of moles = (molicules or prodcuts - products) |
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Term
What is the pH have the falloing buffer solutions
NH4/NH3
CH3CO2H/CH3CO2
HCO3-/CO32-
H3PO4/H2PO4- |
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Definition
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