Acids, Bases and Salts

Question 1

Basic is where on the pH scale?

Answer 1

GREATER than 7

Question 2

Acidic is where on the pH scale?

Answer 2

LESS than 7

Question 3

What are Arrhenius Acids?

Answer 3

Compounds that produce H+ ions in a solution.

Question 4

What is a monoprotic acid?

Answer 4

An acid that produces 1 H+ ion

Question 5

What is a diprotic acid?

Answer 5

An acid that produces 2 H+ ions

Question 6

What is a triprotic acid?

Answer 6

An acid that produces 3 H+ ions

Question 7

What are Arrhenius Bases?

Answer 7

Bases that produce OH- ions in a solution

Question 8

How to write Sulfate

Answer 8

SO4 2-

4 is a subscript, -2 is a superscript

Question 9

How to write Sulfite

Answer 9

SO3 2-

3 is a subscript, -2 is a superscript

Question 10

How to write Phosphate

Answer 10

PO4 3-

4 is a subscript, -3 is a superscript

Question 11

How to write Phosphite

Answer 11

PO3 3-

3 is subscript, -3 is superscript

Question 12

How to write Nitrite

Answer 12

NO2 -

2 is subscript, (-) is superscript

Question 13

How to write Nitrate

Answer 13

NO3 -

3 is subscript, (-) is superscript

Question 14

What is a Brønsted-Lowry Base?

Answer 14

They are bases that serve as proton (H+) acceptors

Question 15

What is a Brønsted-Lowry Acid?

Answer 15

They are acids that serve as proton (H+) donors

Question 16

What are Conjugate Acids?

Answer 16

An acid formed when a base gains a Hydrogen

Acid formed from a base

Question 17

What are Conjugate Bases?

Answer 17

A base formed from an acid that loses a Hydrogen

Question 18

What does Amphoteric mean?

Answer 18

A substance that can act as an acid or a base

H2O is the most common

Question 19

Lewis acids are electron pair _________

Answer 19

acceptors

Question 20

Lewis bases are electron pair _______

Answer 20

donors

Question 21

In an aqueous solution, when [H+] _______, the [OH-] _________.

Answer 21

increases, decreases

and vice versa

Question 22

The total product of concentrations of [H+] and [OH-] in water always equal…

Answer 22

1 * 10^-14, aka Kw

Question 23

What are K values measured in?

Answer 23

Nothing, K values have no units

Question 24

Mathematically, what is neutral?

Answer 24

[H+] = [OH-] = 1 * 10^-7 M

M stands for Molarity

Question 25

Mathematically, what is acidic?

Answer 25

[H+] is greater than [OH-]

Question 26

Mathematically, what is basic?

Answer 26

[OH-] is greater than [H+]

Question 27

What is the equation for pH?

Answer 27

pH = -log[H+]

Question 28

What is the equation for pOH?

Answer 28

pOH = -log[OH-]

Question 29

How is pOH different from pH?

Answer 29

The scale is reversed

Question 30

Convert pH to pOH

Answer 30

[H+] = 10^-pH

Question 31

Convert pOH to pH

Answer 31

[OH-] = 10^-pOH

Question 32

Strong acids and bases _______ dissociate in aqueous solution

Answer 32

completely

Question 33

A weak acid/base has a _____ Ka/Kb value, and a strong acid/base has a _____ Ka/Kb value.

Answer 33

small, large

Question 34

Generic Ka formula

Answer 34

HA <--> H+ + A- Ka= [H+][A-] [HA]

Question 35

Generic Kb formula

Answer 35

B + H2O <--> BH+ + OH- Kb= [BH+][OH-] [B]

Question 36

A neutralization reaction between an acid and a base forms what?

Answer 36

Water and a salt

Question 37

How is a salt formed?

Answer 37

Substance formed from cation of a base and the anion of an acid.

Question 38

What is titration?

Answer 38

Using a buret, adding a certain amount of acid/base to a certain amount of **unkown** base/acid until neutralization

Question 39

What is equivalence point of titration?

Answer 39

When moles of hydrogen ions equal moles of hydroxide ions