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Chemistry H > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

acids examples

A
  • hydrochloric acid.
  • sulfuric acid.
  • nitric acid.
  • carbonic acid.
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2
Q

bases examples

A
  • lithium hydroxide
  • sodium hydroxide
  • potassium hydroxide
  • magnesium hydroxide
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3
Q

properties of acids

A
  • react with bases to form water & a salt (neutralizations)
  • change color of acid base indicators to litmus red
  • reacts with some metals to product H2 gas
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4
Q

dilute acids

A

have a sour taste

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5
Q

aqueous solutions of are

A

electrolytes (strong or weak)

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6
Q

properties of bases

A
  • react with acids to form water & a salt (neutralization)
  • change color of acid-base indicators to litmus blue
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7
Q

aqueous solutions of bases

A

taste bitter & feel slippery

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8
Q

acid formula

A
  • acids are a compound that products hydrogen ions (H+) when dissolved in water
  • no oxygen present

so formulas of acids usually are in “HX”
- x can be monatomic or polyatomic

  • focuses on naming the anion
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9
Q

naming acids

A
  1. if anion ends in ide-, acid becomes with hydro-.
    suffix of anion changes to -ic and ends with acid
  2. if anion ends in -ite, suffix of anion changes to -ous
    ends with acid
  3. if anion ends in -ate, suffix of anion is -ic
    ends with acid
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10
Q

name of HBr

A

hydrobromic acid

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11
Q

name of H2S

A

hydrosulfuric acid

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12
Q

name of HNO2

A

nitrous acid

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13
Q

name of H2SO3

A

sulfurous acid

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14
Q

name of H3PO3

A

phosphorous acid

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15
Q

name of HNO3

A

nitric acid

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16
Q

name of H2CO3

A

carbonic acid

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17
Q

name of H3PO4

A

phosphoric acid

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18
Q

base formula

A
  • base produces hydroxide ions when dissolved in OH
    = if the base is an ionic compound (cation+anion), it is named like any ionic compound
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18
Q

dissociation of water

A
  • “pure” h2o is not really pure
  • h2o can disassociate just like ionic compounds in water into H+ and OH-

because water can do this, it plays a large role in acid base reactions

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19
Q

rate of water disassociation

A

only 1-2 water molecules out of 10 million are disassociated

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20
Q

hydrogen ions in water

A
  • attracted to partial negative charge on oxygen
  • form the ion hydronium H3O+
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21
Q

H3O+

A

H+

(they’re the same)

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22
Q

2 water molecules colliding

A

H2O+H2O –> H3O+ + OH-

H2O –> H+ +
OH-

self ionization of water

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23
Q

self ionization of water

A

within liquid water there is ac chemical reaction of water disassociating into H3O+ and OH-

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24
Q

ion-product constant for water (Kw)

A

Kw = [H+] x [OH-] = 1.0 x 10^14

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25
Q

Kw

A

KW ALWAYS EQUALS 1.0 x 10^14

the equilibrium constant when water goes through self-ionization

[H3O+][OH-] or Kw = [H+][OH-]

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26
Q

acidic solution example

A

HCl(g) → H+(aq) + Cl-(aq)

always:
[H+] is greater than 1.0*10^-7

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27
Q

basic solutions example

A

NaOH(s) → Na+(aq) + OH-(aq)

always:
[H+] is less than 1.0 x 10-7 M
[OH-] is greater than 1.0 x 10-7 M

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28
Q

pH

A

tells us about [H+] in a solution

ranges from 0-14

29
Q

pH<7

A

acidic solution

30
Q

pH=7

A

natural solution

31
Q

pH>7

A

basic solution

32
Q

pH formual

A

-log[H+]

33
Q

[H+] formula

A

10^-ph

34
Q

pOH

A

-log [OH-]
tells us about [OH-]

pH + pOH = 14

35
Q

arrhenius acid

A

substance that yields H+ when dissolved in water

HCl(g) → H+(aq) + Cl-(aq)

35
Q

OH-

A

-10^-pOH

35
Q

tripotic acids

A

3 ionizable hydrogens (H3PO4)

35
Q

arrhenius base

A

substance that yields OH- when dissolved in water

KOH(s) → K+(aq) + OH-(aq)

35
Q

monoprotic acids

A

1 ionizable hydrogen (HNO3)

35
Q

diprotic acids

A

2 ionizable hydrogens (H2CO3)

36
Q

hydrogen ionizing

A

not all hydrogens ionize

CH3COOH(aq) → CH3COO-(aq)+ H+(aq)

36
Q

brønsted-lowry

A

acids: H+ donor
base: H+ acceptor

37
Q

amphoteric

A
  • (water) can act as an acid and a base
37
Q

conjugate pairs

A

2 substances that differ by 1 H+

each pair has one acid and one base

acids have the additional H+

37
Q

lewis base

A

substance that can donate a pair of electron to form a covalent bond

37
Q

6 strong acids

A
  • HClO4
  • HCl
  • HBr
  • HI
  • HNO37
  • H2SO4
38
Q

lewis acid

A

substance that can accept a pair of electrons to form a covalent bond

38
Q

identify parts

NH3 + H2O —> NH4+ + OH-

A

NH3 base
H2O acid

NH4+ conjugate acid
OH- base

NH3 NH4+ conjugate pair
H2O OH- conjugate pair

38
Q

lewis acids need

A

dot structures to see electron pairs

38
Q

strong acids

A

completely disassociate in water

HCl(g) → H+(aq) + Cl-(aq)

39
Q

weak acids

A

only partially ionize

CH3COOH(aq) → CH3COO-(aq)+ H+(aq)

40
Q

6 strong bases

A
  • LiOH
  • NaOH
  • KOH
  • CA(OH)2
  • SR(OH)2
  • BA(OH)2
41
Q
A
42
Q

salt

A

an ionic compound formed from an acid (anion) & a base (cation)

43
Q

all neutralization rxns

A

double replacement rxns

44
Q

acid base titrations

A

a method used to determine the concentration of a solution

makes use of neutralization reactions

  • an indicator is added to signal when the neutralization has occurred
45
Q

standard solution

A

the solution of known concentration

46
Q

acid base titrations indicators

A
  • the point when it changes colors is the end point
  • end point / equivalence point is when neutralization has been reached
47
Q

normality

A

(N) a unit of concentration used mainly in acid-base titration
- considers # of H+ or OH- ions in solition

48
Q

titration formula

A

N1V1 = N2V2

49
Q

titration for acids

A
  • monoprotic: N=M
  • diprotic: N=2M
  • triprotic: N=3M
50
Q

titration for bases

A
  • for 1 OH- ion N=M
  • for 2 OH- ion N=2M
  • for 3 OH- ion N=3M
51
Q

normality

A

20.0 g NaOH in 1.0 L of solution

20g * (1mol/40g) = 0.5 mol
0.5mol=1L=0.5M

1 OH so, 0.5N

52
Q

hydrolysis

A

a reaction of a substance with water

53
Q

salt hydrolysis

A

salts that react with water to form H+ or OH-

54
Q

weak acids, strong bases

A

weak acids neutralized by strong bases produce basic salt solutions

K3PO4

55
Q

strong acids, weak bases

A

strong acids neutralized by weak bases produce acidic salt solutions

NH4NO3

56
Q

strong acids, strong bases

A

strong acids neutralized by strong bases produce neutral salt solutions

NaCL

57
Q

buffers

A
  • solutions that actively resist changes in pH
  • remain constant when small amounts of acid or base are added
  • a solution of a weak acid and one of its salts, or a solution of a weak base and one of its salts
  • made of conjugate acid-base pairs
58
Q

buffer, pH

A

buffer cannot control pH when too much acid or base is added

Chemistry H (11 decks)

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