Exam 2 Flashcards
polyprotic acids (definition)
capable of losing more than 2 proton per molecule
relationship between Ka and pKa and acidity
high Ka = low pKa
as Ka increases, acidity increases
arrhenius acid/base definition
acid – forms H+ or H3O+ ions in water
base – forms OH- ions in water
lewis acid/base definition
acid – accepts a pair of electrons
base – donate a pair of electrons
most weak acids have Ka values ranging from
~10^-2 to 10^-10
autoionization (self-ionization) of water
water dissociates very slightly into ions in an equilibrium
amphiprotic (definition)
acts as a base (accepts an H+) in one case and as an acid (donates an H+) in the other
calibration plot/standard curve
used to find unknown concentrations of a substance in solution
absorption spectra
find wavelength where Abs. is at max
monoprotic (definition)
acid capable of only donating 1 H+ per molecule
strong acids (name the acids)
hydrochloric acid -- HCl hydrobromic acid -- HBr hydriodic acid -- HI nitric acid -- HNO3 sulfuric acid -- H2SO4 perchloric acid -- HClO4
weak acids
hydrofluoric acid – HF
phosphoric acid – H3PO4
carbonic acid – H2CO3
acetic acid – CH3COOH (HC2H3O2)
strong bases
Group 1A(1) hydroxides Heavy Group 2A(2) hydroxides
weak bases
ammonia – NH3
changes in pressure:
equilibrium position changes?
K changes?
equilibrium position may be changed
K unchanged (don’t include pressure of solids or liquids)
