Test 3: Chapters 15 and 16 Flashcards Preview

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Flashcards in Test 3: Chapters 15 and 16 Deck (25)
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1
Q

Arrhenius Acid

A

any substance that produces H+ ions once dissolved

2
Q

Arrhenius Base

A

any substance that produces OH- ions once dissolved

3
Q

What happens when acids and base combine?

A

They neutralize each other.

H+(aq) + OH-(aq) —> H20(g)

4
Q

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

A

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

5
Q

Define Brownstead-Lowry Acid

A

proton(H+) donor

6
Q

Define Brownstead-Lowry Base

A

proton(H+) acceptor

7
Q

What is the intention of the B-L theory?

A

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

8
Q

Define Amphoteric

A

substances that can be both an acid and a base

9
Q

Define Conjugate acid-base pair

A

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

10
Q

Define Strong Acid

A

substance that completely ionizes in solution

11
Q

What are the Strong Acids?

A
Nitric Acid- HNO3
Sulfuric Acid- H2SO4
Chloric Acid- HClO3
Perchloric Acid- HClO4
Hydrochloric Acid- HCl
Bromic Acid- HBr
Hydroiodic Acid- HI
12
Q

Define Weak Acid

A

substance that doesn’t completely ionize in solution

13
Q

What are some weak acids?

A
Hydrofluoric acid- HF
Acetic acid- HC2H3O2
Formic acid- HCHO2
Sulfurous acid- H2SO3
Carbonic acid-H2CO3
Phosphoric acid- H3PO4
14
Q

What does the acid ionization constant (Ka) do?

A

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

15
Q

Ka constant

A

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

16
Q

What is the autoionization of water?

A

when water reacts with itself.

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

17
Q

What is the equilibrium constant of water?

A

Kw= [H+][OH-] also…

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

18
Q

How to tell the types of solutions?

A

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

Basic solution: [H30+] [Oh-]

19
Q

How to find pH?

A

pH= -log(H30+)

20
Q

How to find pH of a strong acid?

A

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

21
Q

How to find pH of a weak acid?

A

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

22
Q

What is the percent ionization of a weak acid?

A

[H3O]/[HA]intital times 100%

23
Q

What is another type of p scale?

A

pOH scale

24
Q

What’s it used for?

A

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

25
Q

How to read a pOH scale?

A

Basic: pOH > 7
Acid: pOH