-
Acid - Arrhenius theory
- a substance that dissolves in water and produces hydrogen ions (H+)
- all start with H and end in -ide
- ionizes in water
-
Acid - Bronsted-Lowry theory
proton donor
-
Acidosis
a physiological condition in which the blood pH is lower than 7.35
-
Alkalosis
a physiological condition in which the blood pH is higher than 7.45
-
Base - Arrhenius theory
- a substance that dissolves in water and produces hydroxide ions (OH-)
- metal + hydroxide (OH-)
- dissociates in water
-
Base - Bronsted-Lowry theory
proton acceptors
-
Bronsted-Lowry acids and bases
- an acid is a proton donor
- a base is a proton acceptor
- water (H2O) can be considered and acid or base in this theory
-
Buffer
- a solution of a weak acid and its conjugate base (the salt of the weak acid) or a weak base and its conjugate acid (the salt of the weak base) that maintains the pH by neutralizing an added acid or base
- resists pH change to a degree
-
Conjugate acid-base pair
- an acid and base that differ by one H+
- when an acid donates a proton, the product is its conjugate base, which is capable of accepting a proton in the reverse reaction
- the stronger the acid, the weaker its conjugate base & vice versa
- 1st the salt of the buffer totally dissociates, 2nd the weak acid/base stays pretty much a molecular substance
- all group 1 salts (including NH4+) are very soluble
- all nitrates are very soluble
-
Hydronium ion
the ion formed by the attraction of a proton (H+) to a water (H2O) molecule written as H3O+
-
Ion product constant of water (Kw)
- the product of [H30+] and [OH-] in solution
- Kw = [H3O+] * [OH-] = 1 * 10**-14
-
Neutral
the term that describes a solution with equal concentration of H3O+ and OH-
-
Neutralization
a reaction between an acid and a base to form a salt and water
-
pH
- a measure of the [H3o+] in a solution
- pH = - log [H3O+]
-
-
-
Reaction of acids & bases
- acid + metal => salt + hydrogen gas (H2)
- acid + carbonate (MCO3, where M is a metal) => metal salt + water (H2O) + carbon dioxide (CO2)
- acid + bicarbonate (MHCO3, where M is a metal) => metal salt + water (H2O) + carbon dioxide (CO2)
- acid + hydroxide => water (H20) + salt
- acid + base => water (H2O) + salt
-
Strong acid
- an acid that completely ionizes in water
- properties:
- - single headed arrow
- - strong electrolyte
- - all products and very little reactants at equilibrium
-
Strong base
- a base that completely ionizes in water
- all metal hydroxides are strong bases
-
Titration
- the addition of a base to an acid sample to determine the concentration of the acid
- a neutralization reaction using an indicator to determine when the end point (when acid & base is equal) is reached
-
Weak acid
- an acid that is a poor donor of H+ and dissociates only slightly in water
- properties:
- - double headed arrow
- - weak electrolyte
- - many reactants and very little products at equilibrium
-
Weak base
a base that is a poor acceptor of H+ and dissociates only slightly in water
|
|
