Unit 10- Acids & Bases Section

Question 1

What model is used for acid/base identification?

Answer 1

Bronsted-Lowry Model

Question 2

According to the Bronsted-Lowry model, acids are proton _____ and bases are proton _____.

Answer 2

Donors- Acceptors ADBA (Acids donate, Bases accept)

Question 3

Acids will always turn into a ______.

Answer 3

Conjugate Base

Question 4

Bases will always turn into a ______.

Answer 4

Conjugate Acid

Question 5

Write an equilibrium expression that represents the autoionization of water.

Answer 5

Kw= [H+][OH-]= 1.00x10^-14

Question 6

pH= _____

Answer 6

-log[H+]

Question 7

pOH= _____

Answer 7

-log[OH-]

Question 8

pH+pOH=

Answer 8

14

Question 9

[H+]=

Answer 9

10^-pH

Question 10

[OH-]=

Answer 10

10^-pOH

Question 11

When determining the number of significant figures of pH and pOH, it’s the _____.

Answer 11

Numbers after the decimal point that matter.

Question 12

If the pH of what we’re adding to water is smaller than it, the pH is _____.

Answer 12

7

Question 13

The difference between strong acids/bases and weak acids/bases is the _____.

Answer 13

% ionization

Question 14

What are the strong acids?

Answer 14

HClO4, HI, HBr, HCl, H2SO4, HNO3

Question 15

Strong acids ionize _____.

Answer 15

Completely

Question 16

Weak Acids are only partially _____.

Answer 16

Ionized

Question 17

The stronger the acid, the weaker the corresponding conjugate _____.

Answer 17

Base

Question 18

The equilibrium always lies to the side of the _____ acid and _____ base.

Answer 18

Weaker-Weaker

Question 19

The strongest acid that can exist in aqueous solution is _____.

Answer 19

H3O+

Question 20

The strongest base that can exist in aqueous solution is _____.

Answer 20

OH-

Question 21

What are the strong bases?

Answer 21

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Question 22

Polyprotic Acids are acids with _____

Answer 22

Multiple ACIDIC hydrogens

Question 23

Give some examples of monoprotic acids.

Answer 23

HC2H3OH-HCl-HF-HNO3

Question 24

Give some examples of diprotic acids.

Answer 24

H2SO4-H2CO3-H2CrO4

Question 25

Give some examples of triprotic acids

Answer 25

H3PO4-H3PO3

Question 26

What do the prefixes of the acids tell us?

Answer 26

It tells us how many hydrogens are coming off

Question 27

For every reaction of polyprotic acids we have, we have a different _____

Answer 27

Equilibrium Constant

Question 28

For monoprotic acids, we can write _____ equation, for diprotic acids, we can write _____ equations, for triprotic acids, we can write _____ equations.

Answer 28

1-2-3

Question 29

If you have a polyprotic acid and you’re asked about the pH, you only need _____.

Answer 29

One ICE Chart

Question 30

For polyprotic acids, the x is the second equation will always be equivalent to the _____.

Answer 30

Second Equilibrium Constant

Question 31

% Dissociated=

Answer 31

Amount Dissociated (M)/ Initial Concentration (M) x100

Question 32

For a weak acid, the percent dissociation _____ as the acid becomes more dilute.

Answer 32

Increases

Question 33

When electrons are localized, the bases will be _____

Answer 33

Stronger

Question 34

If you have a conjugate of a _____ substance, the thing can go back.

Answer 34

Weak

Question 35

What are the steps in determining whether salts are acidic, basic, or neutral?

Answer 35

First, you separate the two ions and add/subtract a hydrogen depending on the ion. Then, depending on which substance is a strong acid or a base, you determine it.

Question 36

Kw=

Answer 36

Ka.Kb

Question 37

When thinking about the strength of acids, it is important to look at two factors:

Answer 37

The strength of the H-X bond and the polarity of the H-X bond.

Question 38

When electrons are localized, the acids will be _____.

Answer 38

Weaker; so, for example, in HClO4, since the electrons are going to be around all of the oxygens as opposed to HClO in which all the electrons are going to be around 1 oxygen, the Ka value of HClO4 will be significantly larger than that of HClO’s