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AP Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Arrhenius Theory of Acids and Bases

A

a substance that donates a H+ is an acid and a substance that donates a OH- is a base

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2
Q

neutralization reaction

A

when an acid is mixed with a base, a salt and water forms

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3
Q

Bronsted-Lowry Acid

A

substance that donates a H+

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4
Q

Bronsted-Lowry Base

A

substance that accepts a H+

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5
Q

hydronium is a

A

pronated water molecule

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6
Q

conjugate acid/base pair

A

two substances that differ by 1 H+

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7
Q

amphiprotic substance

A

species that can act as an acid or a base

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8
Q

most common amphiprotic substance

A

water

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9
Q

titration

A

types of volumetric analysis where the concentration of a solution can be determined through stoichiometry using a standard solution

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10
Q

titrant

A

solution that is standardized of known concentration

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11
Q

analyte

A

solution tested of unknown concentration

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12
Q

equivalence point

A

point in the titration where the moles of the titrant are equal to the moles of the analyte

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13
Q

acid/base indicators

A

complex molecules that change in the presence of an acid or a base

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14
Q

bromothymol blue

A

green when neutral, blue when basic, yellow when acidic

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15
Q

phenolphthalein

A

turns pink in the presence of a base

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16
Q

What is the difference between a concentrated acid and a strong acid?

A

concentration refers to the amount of molecules in a solvent and strength refers to the extent of ionization

17
Q

strong acid

A

acid that ionizes completely

18
Q

6 strong acids

A

perchloric, hydroiodic, hydrobromic, hydrochloric, nitric, sulfuric

19
Q

weak acid

A

acid that only partially ionizes in water

20
Q

acid ionization constant

A

Ka; equilibrium constant for weak acids

21
Q

all weak acids have a

A

ka<1

22
Q

strong base

A

base that ionizes completely

23
Q

strong bases include the OH- bound to a

A

group 1A or 2A element

24
Q

weak base

A

base that partially ionizes in water

25
Q

base ionization constant

A

Kb; equilibrium constant for weak bases

26
Q

binary acid(Hx)

A

the strength of a binary acid is determined by bond length

27
Q

bond length

A

the distance between the H and its anion

28
Q

binary acids: the larger the anion,

A

the longer the bond, the longer the bond the weaker the bond, the weaker the bond, the easier the H+ ionizes(stronger acid)

29
Q

the more H+ on the binary acids,

A

the weaker the acid

30
Q

hydrohalic acids are

A

the strongest acids

31
Q

hydrohalic acids

A

acids made with halogens

32
Q

ternary acids(oxo-acids, oxy-acids)

A

the strength of ternary acids are determined by the number of oxygens and the electronegativity of the center atom

33
Q

ternary acids: the stronger acid has

A

more oxygens; if oxygens are the same, the acid with the more electronegative center atom is stronger

34
Q

carboxyllic acids

A

the strength of a carboxyllic acid is determined by the polarization of the -O-H- bond

35
Q

carboxyllic acid: the fewer carbons in the base chain

A

causes increased polarization, making a stronger acid

36
Q

the substance that has the higher Ka value will

A

act as the acid, the proton donor

37
Q

shifts in equilibria for acid-base systems

A

the direction of strong acid and strong base forming the weak acid and base is favored

38
Q

the strong acid and the strong base are

A

always on the same side of the equation

39
Q

leveling effect

A

the effect that all strong acids ionize completely in water gives the impression that they are all the same strength

AP Chemistry (16 decks)

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