LO 42 - 46

Question 1

What is a neutralization reaction?

Answer 1

acids react with bases and produce H2O or sometimes a weak electrolyte

Question 2

Weak acids do not _________ so they are notated by ↔ reaction arrows

Answer 2

fully ionize

Question 3

________ acids contain more than one ionizable proton and release them _________

Answer 3

polyprotic
sequentially

Question 4

_______ acids have one, first strongly ionizable proton and then a second weaker one

Answer 4

diprotic

Question 5

________ acids contain only two elements

Answer 5

binary

Question 6

How are binary acids named?

Answer 6

hydro + base name of nonmetal (-ic) + acid

Question 7

________ contain H and an oxyanion which is a nonmetal + oxygen

Answer 7

oxyacid

Question 8

How are oxyacids named when the oxyanion ends in -ate?

Answer 8

base name of oxyanion + -ic + acid

Question 9

How are oxyacids named when the oxyanion ends in -ite?

Answer 9

base name of oxyanion + -ous + acid

Question 10

Describe acid-base titrations

Answer 10

a substance in solution of known concentration is reacted with another solution of unknown concentration. an indicator such as dye is used to signal the equivalence point

Question 11

What is the titration equivalence point

Answer 11

when the # of mols OH- equals the number of mols H+ in solution

Question 12

Neutralization reactions between concentrated acids and bases are highly __________

Answer 12

exothermic

Question 13

What are the 4 distinct characteristics of acids

Answer 13

1. sour taste
2. dissolve many metals
3. turn litmas paper blue → red
4. neutralize bases

Question 14

What are the four distinct characteristics of bases

Answer 14

1. bitter taste
2. slippery feeling
3. turn litmas paper red → blue
4. neutralize acids

Question 15

What is the Arrhenius definition of an acid

Answer 15

a substance that produces H+ ions in aqueous solution

Question 16

What is the Arrhenius definition of a base

Answer 16

a substance that produces OH- ions in aqueous solution

Question 17

Weakness or strength of an acid/base is determined by __________ according to Arrhenius

Answer 17

amount that dissociates into ions

Question 18

What is the Bronsted-Lowry definition of an acid

Answer 18

a proton donor

Question 19

What is the Bronsted-Lowry definition of a base

Answer 19

a proton acceptor

Question 20

__________ substances such as H2O can act as an acid or a base

Answer 20

amphoteric

Question 21

____________ acid-base pairs are two substances related to each other by the transfer of a proton

Answer 21

conjugate

Question 22

Base + H+ → ______

Answer 22

conjugate acid

Question 23

Acid - H+ → ________

Answer 23

conjugate base

Question 24

What two factors affect the strength of a binary acid

Answer 24

1. bond polarity
2. bond strength

Question 25

How does bond polarity impact the strength of a binary acid

Answer 25

Increasing the polarity of an "H-X" bond increases the strength of the acid. When shared electrons in an "H-X" bond spend most of their time close to "X" atom, the bond becomes polar. It also becomes weaker.

Question 26

How does bond strength impact the strength of binary acids

Answer 26

the stronger the bond the **weaker** the acid because the H atom will be held more tightly

Question 27

What two factors affect the strength of an oxyacid (HYOx)

Answer 27

1. electronegativity of "Y" 2. number of oxygens bonded to "Y"

Question 28

How does the electronegativity of "Y" in an oxyacid (HYOx) impact strength of the acid

Answer 28

the more electronegative Y, the more it weakens and polarizes the H-O bond and thus the **more acidic**

Question 29

How does the number of oxygens bonded to "Y" in an oxyacid (HYOx) impact strength of the acid

Answer 29

additional O atoms are electronegative and thus draw e- density away from the bonds to Y and H, weaking the bonds and **increasing acidity**

Question 30

The ______ ________ constant (Ka) quantifies the relative strength of a weak acid based on the law of mass action

Answer 30

acid ionization

Question 31

The smaller Ka is, the _______ the acid ionizes thus indicating it as _______

Answer 31

less weaker

Question 32

Because water is amphoteric, it acts as an acid or base with itself in a process known as ________

Answer 32

autoionization

Question 33

The ______________ of water (Kw) represents H2O at equilibrium

Answer 33

ion product constant

Question 34

Kw = ____________ (concentration terms) @ 25°C

Answer 34

[H3O+] · [OH-]

Question 35

Kw = ____________ (numeric) @ 25°C

Answer 35

1.0 · 10^-14

Question 36

A neutral solution contains [H3O+] = [OH-] = ____________ @ 25°C

Answer 36

1.0 · 10^-14

Question 37

An acidic solution contains [H3O+] _____ [OH-]

Answer 37

>

Question 38

A basic solution contains [H3O+] _____ [OH-]

Answer 38

<

Question 39

In **aqueous** solutions both [H3O+] and [OH-] are present and _________ holds true

Answer 39

[H3O+] · [OH-] = 1.0 · 10^-14

Question 40

A "p" scale of any kind indicates the _________ of a value

Answer 40

-log (x)

Question 41

The pH scale specifics the _______ of a solution as given by pH = _______

Answer 41

acidity -log [H3O+]

Question 42

pH + pOH = ______

Answer 42

14

Question 43

The numbers to the right of the decimal place in a pH or pOH value correspond to the number of ________________

Answer 43

significant figures in the negative log ex. -log (1.0 · 10^-3) = 3.00 pH 2 sig figs 2 decimal places

Question 44

pKa = _________ where the smaller the pKa value, the _________ the associated acid

Answer 44

-log(Ka) stronger

Question 45

For oxyacids (H-X-O): more electronegative X = _________ more O atoms = ___________

Answer 45

stronger, stronger

Question 46

For binary acids (H-A): larger the atom = ____________

Answer 46

stronger

Question 47

Strong acids and strong bases do **not** ____________________. As such, when you get the conjugates of a SA or SB in the products side of a reaction . . .

Answer 47

reform in solution they will be neutral