| Term | Definition |
|---|
| Tastes Sour | Acid |
| Litmus Red | Acid |
| Phenolphthalein turns clear | Acid |
| has a HIGH H+ concentration | Acid |
| tastes bitter | Base |
| Turns litmus blue | Base |
| has a LOW H+ concentration | base |
| Arrhenius Acid | produces H+ |
| Arrhenius Base | produces -OH |
| Bronsted Acid | proton donor |
| Bronsted Base | proton acceptor |
| Conjugate Base | Acid - proton |
| Conjugate Acid | Base + proton |
| Strong Acid turns to--> | Conjugate Base |
| Strong Base turns to--> | Conjugate Acid |
| Amphiprotic | substance that can act as a base or acid; can loose or gain a proton |
| Example of Amphiprotic | water |
| As Acid Strength increases, the conjugate base | gets weaker |
| Weaker the Acid | Stronger the conjugate base |
| The more an acid wants to release its proton | the less its conjugate base wants to pick it up |
| Acid Strength increases (periodic table) | across the period and down the group |
| Leveling | strong acid + strong base = weak base + weak acid |
| Lower the pKa | stronger the acid |
| larger the pKa value | stronger the base |
| Reactions Always Favor the Direction of | strong to weak |
| As oxygens increase, acid strength | increases |
| Larger the ion | stronger the acid |
| EN | the tendency to attract electrons |
| Higher the EN of the bond with H | the stronger the acid |
| Formula for Oxoacids | HnEOm |
| "E" in an Oxoacid | nonmetal |
| In oxoacids oxygen bonds to | E |
| If EN of the nonmetal in an oxoacid is great | the weaker the bond between O and H, and stronger the acid |
| Acidity is really just the | strength or weakness of the H bond to the molecule |
| In all water solutions, the water is mostly molecular but a | small amount ionizes |
| [H+][-OH]= (Kw) | 1 x 10^-14 |
| Kc of water | 1.8 x 10^-16 |
| Formula for pH | -log[H+] |
| Formula for pOH | -log[-OH] |
| pH+pOH | 14 |
| Kw= | Ka x Kb |
| HA <-----> | H+ +-A |
| pKa= | -log [Ka] |
| pKb= | -log [Kb] |
| H2O is a ____ base or acid. | weak |
| Polyprotic Acids | substances that can release more than one H+ |
| How many H+ can a polyprotic ion loose at a time? | one |
| First loss of H+ of a polyprotic ion will act as a | strong acid |
| Second, third, fourth loss of a polyprotic ion will act as | a weaker acid than first loss |
| In polyprotic ions, Ka1 ___ Ka2 ... | greater than |
| Stong acids and bases __________ in water solution | Totally dissociate |
| In polyprotic ions, the 2nd ionization is always ____________ than the first. | smaller |
| Salts of Strong Acids and Strong Bases | form neutral solutions |
| salts of weak acids and strong bases | form basic solutions |
| salts of strong acids and weak bases | form acidic solutions |
| salts of weak acids and weak basics form solutions that are | acid, basic, neutral |
| If a salt dissolves in water, the Acid-Base properties of the solution depends | on how the dissolves ions react with water |
| hydrolysis | is a chemical reaction during which one or more water molecules are split into hydrogen and hydroxide ions |
| ionization | when dissolved ions interact with water |
| Ions that are ______________________ hydrolyze appreciably. | conjugates of weak acids or weak bases |
| anions or cations of weak acid/base | can form the acid/base |
| anions or cations of strong acid/base | cannot form acid/base |
| The largest K value will determine | the expected acidity |
| The pH is determined by using the Ka/ Kb of | the ion that reacts with the H2O |
| When a salt of a strong acid and strong base is dissolved in water, the solution becomes | neutral |
| Common Ion Effect | the shift in equilibrium caused by addition of a "common" ion to the solution |
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