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CH 102 > Acids and Bases Ch 16 > Flashcards

Acids and Bases Ch 16 Flashcards

1
Q

Common acids

A

HCl, H2SO4, HNO3, HC2H3O2, H3C6H5O7, H2CO3, HF, H3PO4

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2
Q

HCl facts

A

used to clean metals, process foods, refine metal ores, in stomach acid

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3
Q

H2SO4 (sulfuric acid) and HNO3 (nitric acid) facts

A

used in fertilizers, explosives, dyes, glues, sulfuric acid is in car batteries

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4
Q

HC2H3O2 facts and carboxylic acids

A

acetic acid is in vinegar, carboxylic acid is in foods ~citric acid and malic acid

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5
Q

properties of acids

A

sour taste, can dissolve metals, turn blue litmus paper red, neutralize bases

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6
Q

properties of bases

A

bitter taste, slippery, turn red litmus paper blue, neutralize acids, often poisonous in plants

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7
Q

NaOH and KOH facts

A

used in petroleum and cotton processing, soap and plastic making, unclog drains, in antacids, baking soda

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8
Q

Common bases

A

NaOH, KOH, NaHCO3, Na2CO3, NH3

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9
Q

Arrhenius acids and bases

A

acid = makes H+ ions in aqueous solution, base = makes OH- in aqueous solution

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10
Q

Bronsted Lowry acids and bases

A

acid = proton donor, base = proton acceptor, H+ is basically a proton

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11
Q

acid strengths (binary)

A

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

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12
Q

oxoacids and bond strength

A

more electronegative the Y is, the more acidic because HO is more polarized, with more O, is more acidic

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13
Q

6 strong acids

A

HCl, HBr, HI, HNO3, HClO4, H2SO4

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14
Q

6 weak acids

A

HF, HC2H3O2, HCHO2, H2SO4, H2CO3, H3PO4

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15
Q

what is diprotic and triprotic

A

diprotic means that there are 2 ionizable protons and triprotic means there are 3

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16
Q

amphoteric

A

can act as acid or base, so can donate or accept an H+

17
Q

logarithms and decimal places

A

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

18
Q

pKa scale?

A

a way to quantify strength, smaller pKa means stronger acid

19
Q

mixtures of acids

A

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

20
Q

Le Chatelier and acid mixtures

A

the stronger acid will suppress the ionization of the weaker acid

21
Q

6 strong bases

A

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

22
Q

common weak bases

A

CO3^2-, CH3NH2, C2H5NH2, NH3, HCO3^-, C5H5N, C6H5NH2

23
Q

strong and weak bases with water

A

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

24
Q

anions in salts

A

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

25
Q

cations in salts

A

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

26
Q

cation or anion don’t act as acid or base

A

pH neutral

27
Q

salt where cation = counterion of strong base, anion is conj. base of weak acid

A

basic solution (because neutral + basic)

28
Q

salt where cation is conj. acid of weak base or small highly charged metal and anion is conj. base of strong acid

A

acidic solution (because weak acid + neutral)

29
Q

salt where cation is conj. acid of weak base or small highly charged metal ion and anion is conj. base of weak acid

A

pH depends on relative strength (because acid + base) ~ can determine using Ka and Kb, whichever is larger number will dominate whether basic or acidic

30
Q

polyprotic acid

A

has more than 1 ionizable proton, and is ionized in steps, x found in 2nd step = Ka2, for pH the Ka1 is what matters

31
Q

Lewis acids and bases

A

acid = electron pair acceptor, base = electron pair donor, expands options for acids but not really for bases

CH 102 (2 decks)

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