acid and base equilibria Flashcards
(22 cards)
theory of ionization / electrolytes
- electrolytes exist in the form of ions
- an ion is an atom or group of atoms with an electric charge
- in electrolyte solutions, total pos ion charge = total neg ion charge
strong electrolyte
- ionic compounds
- dissociate 100%
- produce many ions
weak electrolyte
- partially dissociates
- polar covalent molecules
- weak conductors of electricity
arrhenius acid
acid that releases H+ ions in water
bronsted-lowry acid
proton / H+ ion donor
- has H3O as products
arrhenius base
substance that releases OH- ions in water
bronsted-lowry base
proton acceptor
: has OH- in products
conjugate acid
received H
conjugate base
whats left after donating H
adding a strong acid…
⬆️H3O
⬇️OH
adding a strong base…
⬇️H3O
⬆️OH
strong acids…
- have large Ka, more H+
- easily donates protons
- strong electrolytes
- easily dissociates ~95%
weak acids
- weak electrolytes
- dont ionize (5%)
- equilibrium between ions and molecules (double arrows)
- less H+
strong base
- easily accepts H
- strong electrolytes
- completely dissociates to OH or O2
weak bases
- poor proton acceptors
- equilibrium between molecule and ions
salt hydrolysis
Salt reacting with water to produce acidic or basic solutions
strong acid + strong base
neutral salt
weak acid + strong base
basic salt
strong acid + weak base
acidic salt
amphoteric
can act as an acid or base
pH
concentration of H3O or H in a solution
salt
compound composed of the negative ion of an acid and the positive ion of the base
