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Arrhenius acid
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Arrhenius base
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EK Chem 6
Acids and bases
| Question | Answer |
|---|---|
| Arrhenius acid | anything that produces hydrogen ions in aqueous soln |
| Arrhenius base | anything that produces hydroxide ions in aqueous soln |
| Bronsted and Lowry acids | anything that donates a proton |
| Bronsted and Lowry base | anything that accepts a proton |
| Lewis acid | anything that accepts a pair of e's |
| Lewis base | anything that donates a pair of e's |
| the stronger the acid, the _____ the conjugate base | weaker |
| the stronger the base, the _____ the conjugate acid | stronger |
| amphoteric | a substance that can act as either an acid or base |
| strong acids | HI, HBr, HCl, HNO3, HClO4, HClO3, H2SO4 |
| strong bases | NaOH, KOH, NH2-, H-, Ca(OH)2, Na2O, CaO |
| polyprotic acid | acids that can donate more than 1 proton |
| diprotic acid | acids that can donate 2 protons, the second proton is usually so weak and often negligible |
| acid dissociation____ with acid concentration, but acid strength ____ with an acid concentration | decreases, increases |
| 3 factors determining whether H containing molecule will release its H and act as an acid | (1) strength of bond holding H (2) polarity of the bond (3) stability of the conjugate base |
| ___ conjugate base stability will increase acidity | increasing |
| ___ polarity will increase acidity | decreasing |
| ___ bond strength will increase acidity | decreasing |
| in a series of oxyacids, more oxygens means a __ acid | stronger (hypochlorous acid < chlorous acid < chloric acid < perchloric acid) |
| hydride | cmpd with only 2 elements and 1 being hydrogen; can be acidic, basic, or neutral (where acidity increases down and to the right of the periodic table) |
| metal hydrides are ____ | basic or neutral |
| nonmetal hydrides are ___ | neutral or acidic |
| acidity of nonmetal hydrides tends to ___ going down the table | increase (H2O < H2S < H2Se < H2Te |
| autoionization of water | H2O + H2O --> H3O+ + OH-, equilibrium constant Kw |
| Kw | [H+][OH-] = Ka*Kb = 10^-14 |
| pKw | =pH + pOH = 14 |
| acid dissociation constant | Ka, equilibrium constant for acid dissociating in water, = [H+][A-]/[HA] |
| Kb | equilibrium constant for the reaction of the conjugate base with water, =[OH-][HA]/[A-] |
| salts | ionic cmpd's that dissociate in water and often create acidic or basic conditions; pH of such son can be predicted qualitatively by comparing conjugates of the respective ions |
| titration | drop-by-drop mixing of an acid and a base |
| equivalence point | for a monoprotic acid, is the point in the titration when there are equal equivalents of acid and base in solution |
| equivalence point for equally strong acid-base titrations | pH= 7 |
| half equivalence point | point where we could add the largest mat of acid or base w/ the least amt of change in pH (most well buffered); where there is 50% A- and 50%HA; point where half of the acid has been neutralized by the base |
| Henderson-Hasselbach eqn | pH = pKa + log([A-]/HA]); when at the half equivalence point, the pH = pKa |
| indicator | usually a weak acid whose conjugate base is a different color |
| endpoint of indicator | point where the indicator changes color, but it is not the same as the equivalence point |
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miniangel918
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