ACIDS AND BASES Flashcards
These are substances that had a sour taste were corrosive and reacted with substance called bases
Acids
These are substances that had a bitter taste made skin slippery on contact and reacted with acids
Bases
Under Arrhenius theory it ionizes to form hydrogen ions in aqueous solution
Arrhenius acids
Under arrhenius theory if ionizes to form hydroxide ions in aqueous solution
Arrhenius base
A base which ionizes almost completely in solution is said to be__ whereas one which has a small degree of ionization is a__
Strong base
Weak base
In this theory and acid ionizes in water much as an ionic substance and equilibrium constant for the reaction is called acid ionization constant
Arrhenius theory
It is the reaction of an acid and a base to produce water and a salt
Neutralization
It is the proton donor to the lone pair due to electronegativity
Bronsted lowry acid
It is the proton acceptor from the acid under bronsted lowry theory
Bronsted lowry base
The product resulting from the addition of a proton to the base
Conjugate acid
The product formed after the proton is lost from the acid
Conjugate base
It is the acceptor electron such as metal group 3A elements and transition metals
Lewis acids
It is the donor electrons or the lone pairs
Lewis base
The donated electron pair is shared between an acid and a base in a covalent bond which results to a
Coordinate covalent bond
Refers to its ability or tendency to lose a proton
Acid strength
It completely ionizes or dissociates in a solution
Strong acid
It partially dissociates in a solution
Weak acid
It measures the strength of an acidic molecule
Acid dissociation constant (ka)
Measures the strength of an aqueous acid solution
pH
Strong acids have large_and _ conjugate base
Ka & weak
Weak acids have small_ and _ conjugate base
Ka & strong
It indicates the relative strength of the acid or base
Ionization constant (Ka)
Negative log of the ionization constant
pKa
The negative logarithm of water ion constant
pKw
The negative logarithm of acid dissociation constant
pKa
The negative logarithm of base dissociation constant
pKb
Characterized by the presence of a positively polarized hydrogen atom
Organic acids
Hydrogen atom bonded to an electronegative oxygen atom (O-H)
Organic acids
Hydrogen atom bonded to a carbon next to a carbonyl carbon
Organic acids
Examples of organic acids
Methanol
acetone
acetic acid
It contains one or more of the following functional groups
Carboxylic acid group
Phenolic group
Sulfonic acid group
Sulfonamide group
Imide group
Organic acids
Functional groups under organic acids
Carboxylic acid group
Phenolic group
Sulfonic acid group
Sulfonamide group
Imide group
Characterized by the presence of an atom with lone pair of electrons that can bond to a hydrogen ion
Organic bases
These are nitrogen containing compounds and oxygen containing compounds that can act both as an acid or base depending on the circumstances
Organic bases
Organic bases example
Methylamine
Methanol
Acetone
Contain one or more of the following functional groups
-Primary secondary tertiary aliphatic or alicyclic amino groups
-most aromatic or unsaturated heterocyclic nitrogen
Organic bases
Use to calculate the pH of solutions of weak acids weak bases and buffers consisting of weak acids and their conjugate bases or weak bases and their conjugate acids
Henderson hasselbalch equation
Henderson hasselbalch equations
pH= pKa + log (A/HA)
pH= pKw - pKb + log (B/HB)
It is the base dissociation constant
kb
It is the water dissociation constant
Kw
Molecule that acts both acid and base
Amphoteric
Increase Ka will _ ph
Decrease
Decrease Ka will _ ph
Increase
Increase Ka will _ acidity
Increase
Decrease Ka will _ acidity
Decrease
Increase Ka will _ basicity
Decrease
Decrease Ka will _ basicity
Increase
pH+pOH=
14
pKw=
14
