Term
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Definition
The lower (higher) the pH of equimolar acids (bases) the stronger the acide (base)
acids= pH<7
bases= pH>7 |
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Term
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Definition
| Strong (weak) acids (bases) ionize 100% |
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Term
| Acid-base proportions of compounds w/ elements X & O & H |
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Definition
If:
X = metal, compound is a base (NaOH)
X = nonmetal, compound is an acid (HNO3) |
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Term
| Acid-base proportions of compounds w/ elements X & O & H |
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Definition
| The higher (lower) the electronegativity of X the more acidic (more basic) the compound. |
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Term
| Acid-base proportions of compounds w/ elements X & O & H |
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Definition
The greater # of H's in a coumpound where H is the only variable the more acidic the compound.
Ex:
Na2HPO4 over NaH2PO4 |
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Term
| Acid-base proportions of compounds w/ elements X & O & H |
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Definition
The greater # of O's in a compound where O is the only variable the more acidic the compound.
Ex:
H2SO4 over H2SO3 |
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Term
| Conjugate Acids and Bases |
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Definition
Strengths of acids (bases) and their conjugate bases (acids) are inverse
Ex:
Acid strength: HCl>HCN
Base strength of conjugate: CN->Cl- |
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Term
| Acid-Base Neutralization and Indicators |
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Definition
| the salt product of acid-base neutralization is not necessarily neutral. |
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Term
| Acid-Base Neutralization and Indicators |
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Definition
Salt properties can be predicted from strengths of reacting acid and base:
1. Strong acid + strong base = neutral salt
2. Weak acid + strong base = basic salt
3. Strong acid + weak base = acidic salt |
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Term
| Equivalent Weight Titrations |
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Definition
Experimental Equivalent Weight =
g sample
mol of OH- |
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Term
| Equivalent Weight Titrations |
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Definition
Theoretical Equivalent Weight =
Molecular wt
# ionizable H |
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Term
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Definition
Metal ions are Lewis acids and exist as aquo complex ions in aqueous solution.
Ex:
[Al(H2O)6]3+ |
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Term
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Definition
Aquo Complex metal ions react w/ water molecules. During reaction proton(s) is(are) released from the aquo complex metal ion and bond to outside water molecules(s) to form Hydronium ions.
Ex:
[Cu(H2O)4]2+ + H2O = [Cu(H2O)4(OH)]+ + H3O |
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Term
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Definition
| Post transition > transition > alkaline earth > alkali |
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Term
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Definition
| Mg2+ has a greater charge density than Ca2+ since the ionic radius of Mg is smaller than Ca and thus Mg2+ is more acidic than Ca2+. |
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Term
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Definition
increases as period # decreases within a family
Ex:
Mg2+ is more acidic than Ca2+ |
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Term
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Definition
| = electron pair seekers (cations) |
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Term
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Definition
= electron pair donor
also called ligands |
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Term
| Lewis acid-base reactions (another name) |
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Definition
| are also called complexation reactions |
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Term
| Lewis acid-base reactions |
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Definition
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Term
| Lewis acid-base reaction (what happens when a new base is added?) |
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Definition
A lewis acid (base) reacts w/ the BEST Lewis base (acid)
Ex:
Therefore if a new Lewis base is added to a reaction mixture, ligand/base exchange will occur if the added base is better |
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Term
| What cations react with NH3 |
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Definition
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Term
| Which cation's react with OH- |
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Definition
| Only post-transition cation's |
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Term
| Dissolving of precipitates and position of cation on periodic table |
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Definition
Transition metal ion preipitates dissolved upon addition of NH3.
Post-transition and pre-transition metal ion precipitates did not dissolve |
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Term
| Dissolving of precipitates |
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Definition
| Precipitate will dissolve upon addition of OH- or NH3 if the cation comprising the ppt. reacts with the added base to form a soluble complex ion |
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