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Chem 106 Assessment4
| Term | Definition |
|---|---|
| Arrhenius acid | increases H+ when dissolved in water |
| Arrhenius base | increases OH - when dissolved in water |
| Bronsted-Lowry acid | H+ donor |
| Bronsted-Lowry base | H+ acceptor |
| conjugate acid | what's left of a base after it accepts a proton/H+ |
| conjugate base | what's left of an acid after it donates its H+ |
| the stronger the acid/base the _______ its conjuagte | the weaker it's conjugate |
| Kw = | 1x10^-14 [OH-][H+] |
| neutral | [H+]=[OH-] = 1x10^-7 |
| basic | [OH-] > 1x10^-7 |
| acidic | [H+] . 1x10^-7 |
| strong acids and bases ______ dissociate weak acids and bases ______ dissociate | strong - completely weak - partially |
| strong acids | HCl HBr HI HNO3 NClO4 H2SO4 |
| strong bases | LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2 |
| p means | -log (better way to measure it, log makes the numbers all close to each other) |
| pH + pOH = | 14 |
| Ka * Kb = | Kw |
| more polyproptic acids, the ____ proton has tendency to dissolve more | first |
| pKa | measure how strong an acid is measures how easily the acid gives up H+ |
| pH | measure of the acidity of a solution (measure concentration of H+) |
| protonated | has an H+ on it |
| pH=pKa when | the acid is half dissociated |
| pH > pKa | mostly depronated |
| pH < pKa | mostly protonated |
| with salts you must consider 2 steps | dissociation hydrolysis |
| lower pKa/pKb | higher the strength of acid/base (-log flips scale) |
| SA/SB | no hydrolysis ions completely dissociate neutral solution |
| SA/WB | hydrolysis of cation (that came from the weak base) acid anion completely dissociates acidic |
| WA/SB | hydrolysis of anion (that came from the weak acid) base cation completely dissociates basic solution |
| WA/WB | both ions react with water compare Ka to Kb to see if solution is acidic or basic |
| spectator ions | do not react with water, do not chnage pH stays the same before and after a reaction |
| cations of strong bases ______ change the pH | do not ex: Na+ |
| anions of strong acids _____ change the pH | do not ex: Cl- |
| positively charged cations ____ pH | lower (NH4+, H3O+) |
| metal ions _____ pH | decrease |
| general acid and base equations | HA + H2O --> H3O+ + A- B + H2O --> HB + OH- |
| buffer | resists pH change 1) weak acid/base and conjugate 2) same common ion 3) in water |
| RICE tables | M or atm equilibrium |
| BCA table | mols completion |
| titration | adding a titrant into an analyte to figure out its concentration |
| what do you need for a titration | analyte indicator titrant |
| equivalence point | analyte and titrant are at exact equal stoichiometric amount |
| end point | indicate color change, stop adding titrant (very close to equivalence point if done correctly) |
| saturated | max amount of solute has dissolved in the solvent |
| always soluble | group 1A: Li, Na, K, Rb, Cs NH4+ NO3- CH3COO- |
| Ca, Sr, Ba are soluble with and limited soluble with | Cl, Br, I, OH, S2 SO4, F, O2, PO4, Cr2O4 |
| Cu+ is soluble with and limited soluble with | SO4 Cl, Br, I, OH, S2 SO4, F, O2, PO4, Cr2O4 |
| Hg 2+ and Pb 2+ are limited soluble with | SO4 Cl, Br, I, OH, S2 SO4, F, O2, PO4, Cr2O4 |
| SA/SB titration curve | starts at a very low pH (complete dissociation) no buffer, sharp spike equivalence point at 7 |
| WA/SB | starts at a higher pH (partial dissociation) buffer region equivalence point above 7 (strong base wins against weak acid) |
| SA/WB | starts a very high pH (basic) buffer region equivalence point lower than 7 (acid wins) |
| Lewis acid | accept electron pairs |
| Lewis base | donate electron pairs and accept protons |
| ligands | aka Lewis bases |
| complex ion | metal complexes form as ligands share electrons with vacant orbitals on a metal |
| complex ion formation is highly | product favored |
| Kf | formation constant very big - product favored |
| coordination number | number of ligand atoms attached to the central atom |
| coordination sphere | [in brackets] counter ion is outside |
| coordination number is always ___ for Cr (III) and Co (III) | 6 |
| coordination number is always ___ for Pb (II) | 4 |
| larger ligands | lower coordination number |
| negatively charged ligands | lower coordination number |
| Ksp | solubility-product constant measures how much salt can dissolve in water |
| molar solubility | mol/L |
| mass solubility | g/L |
| solubility | g/100 mL or g/L |
| slightly soluble salts partially dissolve creating an equilibrium | with a saturated solution of ions solid --> ion + ion |
| ksp - kf - | ksp - precipiate (small, goes to reactants) kf - dissolving of ions (large, goes to products) |
| solubility of slightly soluble salts _______ in presence of common ion | decrease |
| solubility of slightly soluble salts _____ with an increase of H+ | increase |
| Ksp < Q Ksp = Q Ksp > Q | Ksp < Q precipitate forms Ksp = Q saturated solution Ksp > Q no precipitate, solid dissolves |
Created by:
anyasalmon