Acids and Bases Ch 16 Flashcards
Common acids
HCl, H2SO4, HNO3, HC2H3O2, H3C6H5O7, H2CO3, HF, H3PO4
HCl facts
used to clean metals, process foods, refine metal ores, in stomach acid
H2SO4 (sulfuric acid) and HNO3 (nitric acid) facts
used in fertilizers, explosives, dyes, glues, sulfuric acid is in car batteries
HC2H3O2 facts and carboxylic acids
acetic acid is in vinegar, carboxylic acid is in foods ~citric acid and malic acid
properties of acids
sour taste, can dissolve metals, turn blue litmus paper red, neutralize bases
properties of bases
bitter taste, slippery, turn red litmus paper blue, neutralize acids, often poisonous in plants
NaOH and KOH facts
used in petroleum and cotton processing, soap and plastic making, unclog drains, in antacids, baking soda
Common bases
NaOH, KOH, NaHCO3, Na2CO3, NH3
Arrhenius acids and bases
acid = makes H+ ions in aqueous solution, base = makes OH- in aqueous solution
Bronsted Lowry acids and bases
acid = proton donor, base = proton acceptor, H+ is basically a proton
acid strengths (binary)
weaker bond = stronger acid so HCl is more acidic than HF, bond polarity is also important, must be have negative dipole away from hydrogen - going over a row with electronegativity has greater effect than going down a row
oxoacids and bond strength
more electronegative the Y is, the more acidic because HO is more polarized, with more O, is more acidic
6 strong acids
HCl, HBr, HI, HNO3, HClO4, H2SO4
6 weak acids
HF, HC2H3O2, HCHO2, H2SO4, H2CO3, H3PO4
what is diprotic and triprotic
diprotic means that there are 2 ionizable protons and triprotic means there are 3
amphoteric
can act as acid or base, so can donate or accept an H+
logarithms and decimal places
only the numbers to the right of the decimal point are significant in logarithms, so if the concentration has 2 sig figs then report to 2 decimal places
pKa scale?
a way to quantify strength, smaller pKa means stronger acid
mixtures of acids
strong acid + weak acid = ignore weak acid, so [acid] = [H3O+], with weak acids if one is 10^3 times larger than the other then can ignore weaker acid
Le Chatelier and acid mixtures
the stronger acid will suppress the ionization of the weaker acid
6 strong bases
LiOH, NaOH, KOH, Sr(OH)2, Ca(OH)2, Ba(OH)2, note that some of these are metal hydroxides and make 2 mol of OH- when dissolved in water
common weak bases
CO3^2-, CH3NH2, C2H5NH2, NH3, HCO3^-, C5H5N, C6H5NH2
strong and weak bases with water
in strong base [base] = [OH-], take into account if it makes 2 moles of OH- so would need to multiply by 2, for weak base with water use ICE table
anions in salts
an anion that is a conj. base of a weak acid is a weak base, an anion that is a conj. base of a strong acid is neutral
cations in salts
cations that are counterions of strong bases are neutral, cation that is conj acid of weak base is a weak acid, small highly charged metal cations make weakly acidic solutions
cation or anion don’t act as acid or base
pH neutral
salt where cation = counterion of strong base, anion is conj. base of weak acid
basic solution (because neutral + basic)
salt where cation is conj. acid of weak base or small highly charged metal and anion is conj. base of strong acid
acidic solution (because weak acid + neutral)
salt where cation is conj. acid of weak base or small highly charged metal ion and anion is conj. base of weak acid
pH depends on relative strength (because acid + base) ~ can determine using Ka and Kb, whichever is larger number will dominate whether basic or acidic
polyprotic acid
has more than 1 ionizable proton, and is ionized in steps, x found in 2nd step = Ka2, for pH the Ka1 is what matters
Lewis acids and bases
acid = electron pair acceptor, base = electron pair donor, expands options for acids but not really for bases
