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Chem > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Arrhenius Theory

A

Acid - substance that forms the hydronium ion in water.
Base - substance that forms the hydroxide ion in water.
Pros - Easy to sort a + b
Cons - Many bases don’t contain hydroxides

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2
Q

Bronsted Lowry Theory

A

Acid - donates a proton, becomes conjugate base
Base - accepts a proton, becomes a conjugate acid

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3
Q

Lewis Theory

A

Acid - accepts an electron pair around central atom
Base - donates an electron pair from around central atom

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4
Q

Polyprotic

A

2+ protons

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5
Q

coordinate covalent bond

A

both electrons donated by a single substance

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6
Q

How much is ionized in a strong rxn?

A

100%

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7
Q

How much is ionized in a weak rxn?

A

> 100%

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8
Q

Binary Acids vs Tertiary Acids

A

Binary - 2 elements
Tertiary - 3 elements

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9
Q

Per _ ate —>

A

Per _ ic acid

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10
Q

_ate —>

A

_ic

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11
Q

_ite —>

A

___ous

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12
Q

Hypo_ite —>

A

Hypo _ ous

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13
Q

_ide

A

Hydro_ic

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14
Q

Strong Acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

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15
Q

Strong Bases

A

OH- with a metal from Group 1 or 2, except Be & Mg

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16
Q

Strong acids and bases are ___ conductors

A

good

17
Q

How many arrows to use for strong and weak?

A

strong = 1
weak = 2

18
Q

H+ > OH-

A

acidic

19
Q

H+ < OH-

A

basic

20
Q

H+ = OH-

A

neutral

21
Q

pH —> pOH

A

pH + pOH = 14

22
Q

pOH to OH-

A

10 ^-pOH

23
Q

OH - to pOH

A

-log (OH-)

24
Q

H+ to OH - and vice versa

A

H+ x OH- = 1 x 10^-14

25
Q

H+ to pH

A

-log H+

26
Q

pH to H+

A

10^-pH

27
Q

You must show ___ in a weak acid dissosciation equation

A

Water

28
Q

You must show ___ in a weak acid dissociation equation

A

Water

29
Q

How do conjugate acids/bases differ from their OGs?

A

By one proton

30
Q

Amphiprotic

A

Can donate or accept a proton (act as acid or base)

31
Q

Most common amphiprotic substance

A

water

32
Q

Amphoteric

A

Can react with both acids and bases

33
Q

Polyprotic Acids

A

Can give more than one H+ ion away. H2S, H2CO3

34
Q

What is titration

A

A technique used to determine the unknown molarity of an acid or base. Solution of known molarity is dropped to the other solution until a neutralization rxn takes place

35
Q

Equivalence Point

A

When all of the acid is neutralized by the base - end of titration

36
Q

Indicators

A

show when the equivalence point is used. Most common indicator is phenophaletin.

37
Q

Buffers

A

Solutions that resist changes in pH / keep it constant. Usually weak acid + conjugate base / vice versa.

Chem (15 decks)

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