Chem 106 – Chemistry – Flashcards
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| product favored |
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| once reaction has reached equalibrium, the greater concentration is on the product side |
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| reactant favored |
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| once the reaction has reached equalibrium the concentration is on the reaction side |
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| equalibirum constant (K) |
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| ICE table |
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| used to determine concentrations |
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| equalibrium consintration expression |
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| ;never included in equilibirum expression? |
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K;1 Ka/b;1 |
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Product favored at equalibirum. strong acid/bases ; |
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| completion in regards to a reaction |
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| essentially all have been converted to water it was sapouse to.; |
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| K;1 |
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| reaction is reactant- favored at equilibrium |
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| reaction quotiant q |
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| at an point as the reaction proceeds from the reactants to an equailibrium mixtrue.; |
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| Q;K |
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| reactants must be converted to products for equilibruim |
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| Q;K |
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| some products must be converted to reactants for equilibrium |
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| short cut to solving equalibrium concentration equation |
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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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| what is the equilibrium constant for the new K when there are new stoichiometirc ratio's? |
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| it is the old K raised to the power of the miltiplication factor of the stoichiometric number |
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| what happens to K when the chemical equation is revervsed? |
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| the new K is the reciprocal of the old K |
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| how is the new K found when adding two reactions together? |
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| The two K's are multiplied to find the new K |
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| how is the equalibrium constant disturbed? |
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| Le Chateleir's principle |
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| how reaction will adjust to the quantities of reactants and products so that equilibtium is restored |
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| what side will equilibrim favor of a gass reaction when volume is increased? |
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| the side with more molecules |
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| what side will an equilibrium favor of a gass reaction when volem is decreesed? |
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| the side with the smallest number of gass molecules |
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| what happens to the energy flow when the reaction is heated |
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| the energy is obsorbed meaning it is endothermic |
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| Arrhenius definition of an acid and base |
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| 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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| Bronsted - Lowery definition of acid and base |
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| acid is a proton donar and a base is a proton acceptor |
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| monoprotic acids |
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| capable of donation one proton |
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| polyprotic acids |
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| capable of donating many protons |
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| amphiprotic |
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| ions that can behave either as bronsted acids ro bases |
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| all polyatomic ions are ....... when it comes to donating hydtrgen ions |
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| amphiprotic |
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| conjugate acide base pair |
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| consits of two species that differ from each other by the presence of one hydrogen ion |
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| autoionization |
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| water is composed of some H3O and some OH, it is never not conducting electricity |
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| what is the equalibrium constant for water at 25 degrees C |
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| Kw = [H3O+][OH-] = 1 * 10-14 |
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| autoionization constant for water |
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| Kw |
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| neutral solution |
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[H3O+] = [HO-] both are equal to 1 * 10-7 |
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| acidic solution |
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[H3O+] > [OH-]
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| basic solution |
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| [H3O+] < [OH-] |
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| what is pH |
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| pH = -log[H3O+] |
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| what is pOH |
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| pOH = -log[OH-] |
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| sum of pH and pOH |
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| the some of pH and pOH must be equal to 14 at 25 degrees C |
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| why is the some of pH and pOH always equal to 14? |
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| 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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| how do you define relative strengths of acids? |
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| 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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| what does a large Ka mean? |
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| what happens to the stregnth of Ka;and conjuagate Kb when the molicule has a big organic tail? |
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the Ka ( acidity ) decreases the conjugate Kb increases |
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| how do polyprotic acids ionize? |
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| they are broken down into steps |
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| what happens to the K aspolyprotic acids are ionzed? |
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| the K ;become smaller |
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| why does k become smaller as more H+ are being pulled off? |
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| 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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| anions that are conjugate bases of strong acids have what kind of effect on the pH |
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| they are such weak bases that they have no effect on pH solution |
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| deprotonation |
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| removal of H+ ions |
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| how do alkali metal and alaline earth cations effect pH of solution? |
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| they have no effect |
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| what are acidic cations limited to? |
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| metal ations with 2+ or 3+ charges and to ammonium ions |
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| all metal ions are what in water |
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| hydrated |
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| pKa ? |
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| pKa;= - log (Ka) |
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| relationship among pK values |
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| pKa +;pKb;=pKw |
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| Ka *Kb;= Kw |
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| the product of Ka for an acie and Kb;for its conjugate base is euql to the constant specifically Kw |
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| what side does the equalibrium fall on? |
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| the side with the weeker base or acid |
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| how do all proton transfer reactions proceed? |
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| from the stronger acid and base to the weaker acid and base |
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| what is the net ionic equation for strong base and acid? |
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| OH + H = H2O |
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| what are the products of a hydrolsys reaction? |
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| Kp |
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| the cantstant for finding the parsail pressures |
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| 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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| is it is a conj. acid it is considered to be an acid when looking at table 17.4.; |
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| 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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| ;The solution is basic with the pH depending on Kb |
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| mixing strong acid and strong base? |
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| produces a neutroal solution |
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| mixing equal number of moles of strong acid with weak base ? |
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| produces an acidic solution with pH depending on Ka |
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| what happens when acetic acid (CH3CO2H) a weak acid is mixed with ammonia (NH3)? and why |
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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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| what happens when mixing weak ka and kb values? |
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| the pH depends on the relative Ka and Kb values |
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| how is the pH effected by the inorganic polyptotic acids/bases? |
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| the pH is many effected by the release of the first H+ ion and not so much by the second |
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| lewus acid |
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| is a substance that can accept a pair of electrons from another atom to form a new bond |
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| lewis base |
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| is a substance that can donate a pair of electrons to another atom to form a new bond |
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| acid-base adduct (coordinate covalent bond) |
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| the product of a lewis acid base reaction |
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| list some moecules that have both strong acid and strong base |
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NaHSO4 KClO4 NaNO3 LiBr |
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| complex ion |
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has a lot of atoms attached to it with a charge; [Co(H20)4Cl2]+ |
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| when given two Ka's for a reactions how is the equalibrium constant found? |
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| multiply Ka1 times ka2 |
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| dynamic equilibrium |
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| condition in which forward rate of reaction equals reverse rate |
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| at equilibirum was does the forward and the reverse rate of the reaction equal? what is that called? |
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| the forward rate equals the reverse rate. that is where we get the equilibrium constant from? |
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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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1:set up ICE table 2: solve for x 3: caclulate K by the equilbrium constant equation |
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| What happens to K when T increases? |
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| The K increases when T increases. When K increases that means that it favors the products. |
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| what constitutes a strong acid? |
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| stronger than water |
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strong or week acid/ base
acetic acid |
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CH3co2H
weak acid |
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| what is a buffer? |
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buffers always consist of weak acid and conjugate base
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weak base and conjugate acid |
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| the comon ion effect |
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| 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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| what is the buffer or HF? |
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| hydrofluoric acid (weak acid HF) and sodium flouride (conj. base F-) |
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| what is the buffer system for acetic acid?; |
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| acetic acid (CH3COOH week acid) and sodium acetate ( CH3COO conj. bAse) |
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| equivalence point of strong acid/ base? |
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| is always going to be at 7 pH |
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| the equivalence point of a weak acid with a strong base? |
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| the ph is controlled by the conjugate base of the acid.; |
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| weak acid and strong base have the same consentration |
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| means the pka is = to the ph in a titration |
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| what is the ph of a weak acid and a strong base at the equivalancy point? |
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| greater than 7!; |
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| whem is a substance predicted to be more soluble then ksp value? |
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| when a salt is the conj. baske of weak acd is there and an |
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| Kf |
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| formation constant.; |
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| will a small or large Ksp precipitate first? |
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| a small Ksp will presipitate first because it has a larger Kf value. |
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| how would you calculate the Knet for the disosiation of a solid and an acid? |
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| you would findthe Ksp and Kform and multiply them |
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| when are kc and Kp the same? |
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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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What is the pH have the falloing buffer solutions ; NH4/NH3 CH3CO2H/CH3CO2 HCO3-/CO32- H3PO4/H2PO4- |
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9 4.7 10 2 |
