Term
Arrhenius Acid
Arrhenius Base |
|
Definition
Anything that produces hydrogen ions in an aqueous solution.
Anything that produces hydroxide ions in an aqueous solution. |
|
|
Term
Bronsted and Lowry Acid
Bronsted and Lowry Base |
|
Definition
Anything that donates a proton
Anything that accepts a proton |
|
|
Term
|
Definition
Anything that accepts a pair of electrons.
Anything that donates a pair of electrons. |
|
|
Term
|
Definition
|
|
Term
|
Definition
The resultant product of a base in a reaction.
|
|
|
Term
|
Definition
| The resultant product of a acid in a reaction. |
|
|
Term
|
Definition
| Substance that act as an acid or base dependent on the environment. |
|
|
Term
|
Definition
Hydroidic acid, HI
Hydrobromic acid, HBr
Hydrochloric acid, HCl
Nitric acid, HNO3
Perchloric acid, HClO4
Chloric acid, HClO3
Sulfuric acid, H2SO4 |
|
|
Term
|
Definition
Sodium Hydroxide, NaOH
Potassium Hydroxide, KOH
Amide Ion, NH2-
Hydride Ion, H-
Calcium Hydroxide, Ca(OH)2
Sodium Oxide, Na2O
Calcum Oxide, CaO |
|
|
Term
|
Definition
| Can donate more than one proton |
|
|
Term
| How Molecular Structure Affects Acid Strength |
|
Definition
1. Strength of the bond holding the hydrogen to the molecule
2. the polarity of the bond
3. the stability of the conjugate base |
|
|
Term
|
Definition
| Binary compounds that contain hydrogen |
|
|
Term
|
Definition
Pure water reacting with itself to form hydronium and hydroxide ions.
H20 + H20 --> H- + H30+ |
|
|
Term
|
Definition
Kw = [H+][OH-]
Kw =10-14
KaKb=Kw |
|
|
Term
|
Definition
|
|
Term
| Acid Dissociation Constant, Ka |
|
Definition
|
|
Term
| Base Dissociation Constant, Kb |
|
Definition
|
|
Term
|
Definition
Ka = [H+][A-]/[HA]
If we know Ka and molar concentration of the acid, and need to find the pH, we can solve for
x*x/.01-x = Ka which reduces to
x2/.01=Ka |
|
|
Term
|
Definition
Ionic compounds that dissociate in water.
When salts dissociate they often create acidic and basic conditions. |
|
|
Term
|
Definition
Drop by drop mixing of an acid and a base.
Performed to find the concentration of some unknown by comparing it with the concentration of the titrant. |
|
|
Term
| Equivalence Point (Stoichiometric point) |
|
Definition
| Point for a monoprotic acid in titration when there are equal equivalents of acid and base in a solution. |
|
|
Term
| Titration with a base stronger than the acid: |
|
Definition
| Equivalence point is above 7 |
|
|
Term
| Titration with the acid stronger than the base. |
|
Definition
| Equivalence point below 7 |
|
|
Term
|
Definition
Point where one half of the acid has been neutralized by the base.
Concentrations of the acid equal to the concentration of the conjugate base.
This shows the point where the solution is the most well buffered.
pH of the solution = pKa of the acid. |
|
|
Term
|
Definition
| We can add the largest amount of base or acid with the least amount of change in pH. |
|
|
Term
| Henderson-Hasselbalch Equation |
|
Definition
pH = pKa + log([A-]/[HA])
When [A-]=[HA], pH=pKa because log(1) = 0 |
|
|
Term
|
Definition
| A weak acid whose conjugate base is a different color. |
|
|
Term
|
Definition
| The pH values of the two points of color change. Can be predicted by the HH Equation |
|
|
Term
|
Definition
| The point where an indicator changes color. |
|
|
