Test 3: Chapters 15 and 16

Question 1

Arrhenius Acid

Answer 1

any substance that produces H+ ions once dissolved

Question 2

Arrhenius Base

Answer 2

any substance that produces OH- ions once dissolved

Question 3

What happens when acids and base combine?

Answer 3

They neutralize each other.

H+(aq) + OH-(aq) —> H20(g)

Question 4

What does the Bronsted-Lowry acid-base theory focus on?

Answer 4

It focuses on the transfer of H+ ions, which are called protons

Question 5

Define Brownstead-Lowry Acid

Answer 5

proton(H+) donor

Question 6

Define Brownstead-Lowry Base

Answer 6

proton(H+) acceptor

Question 7

What is the intention of the B-L theory?

Answer 7

To help identify bases that don’t essentially contain OH- ions but still produces them in solution

Question 8

Define Amphoteric

Answer 8

substances that can be both an acid and a base

Question 9

Define Conjugate acid-base pair

Answer 9

two substances that are related to each other by the transfer of a proton

Question 10

Define Strong Acid

Answer 10

substance that completely ionizes in solution

Question 11

What are the Strong Acids?

Answer 11

Nitric Acid- HNO3
Sulfuric Acid- H2SO4
Chloric Acid- HClO3
Perchloric Acid- HClO4
Hydrochloric Acid- HCl
Bromic Acid- HBr
Hydroiodic Acid- HI

Question 12

Define Weak Acid

Answer 12

substance that doesn’t completely ionize in solution

Question 13

What are some weak acids?

Answer 13

Hydrofluoric acid- HF
Acetic acid- HC2H3O2
Formic acid- HCHO2
Sulfurous acid- H2SO3
Carbonic acid-H2CO3
Phosphoric acid- H3PO4

Question 14

What does the acid ionization constant (Ka) do?

Answer 14

Quantifies the relative strength of acids. The smaller the Ka value, the less the acid ionizes and the weaker the acid will be

Question 15

Ka constant

Answer 15

Ka= [H+][A-]/[HA]

Question 16

What is the autoionization of water?

Answer 16

when water reacts with itself.

H20(l) + H20(l) H30+(aq) + OH-(aq)

Question 17

What is the equilibrium constant of water?

Answer 17

Kw= [H+][OH-] also…

At 25 degrees Celcius: Kw= 1.0 x 10^-14

Question 18

How to tell the types of solutions?

Answer 18

Neutral solution: [H30+] = [OH-]

Basic solution: [H30+] [Oh-]

Question 19

How to find pH?

Answer 19

pH= -log(H30+)

Question 20

How to find pH of a strong acid?

Answer 20

Since strong acids by definition completely ionize in water and because we can ignore the autoionization of water, the concentration of [H30+] in a strong acid is equal to the M of the strong acid.
Ex: .10 M HCl
pH= -log(.10)
pH= 1.00

Question 21

How to find pH of a weak acid?

Answer 21

Since weak acids don’t equal the concentration of [H30+], we have to use two equilibrium methods (either small x or quadratic formula)

Question 22

What is the percent ionization of a weak acid?

Answer 22

[H3O]/[HA]intital times 100%

Question 23

What is another type of p scale?

Answer 23

pOH scale

Question 24

What’s it used for?

Answer 24

The pOH scale is similar to the pH scale but is defined with [OH] instead of [H3O+]
- pOH= -log[OH-]

Question 25

How to read a pOH scale?

Answer 25

Basic: pOH > 7
Acid: pOH