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Chemistry SAT > Chapter 11 > Flashcards

Chapter 11 Flashcards

(70 cards)

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1
Q

water solutions (aq) of acids conduct what?

A

Electricity

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2
Q

The degree of condensation depends on the acid’s degree of _______

A

ionization

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3
Q

Acids will react with metals that are more active than __________ ions

A

hydrogen

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4
Q

If an acid is a strong oxidizer, then it will not release ___________

A

hydrogen ions

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5
Q

________ have the ability to change the color of indicators?

A

Acids

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6
Q

What is Litmus?

A

A paper that indicates if a solution is acidic or basic (Red if acidic, purple if neutral)

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7
Q

What is phenolphthalein?

A

Similar to Litmus (Pink in basic, colorless in neutral or acidic)

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8
Q

What is the formula for Nitric acid?

A

HNO3

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9
Q

What is the formula for hydrochloric acid?

A

HCl

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10
Q

What is the name of H2SO4

A

Sulfuric acid

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11
Q

What is the name of HI

A

Hydriodic acid

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12
Q

What is the name of HBr

A

Hydrobromic acid

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13
Q

What do HNO3, HCl, H2SO4, HI, and HBr have in common?

A

They are all completely or nearly completely ionized

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14
Q

WHat is the formula of Oxalic acid?

A

H2C2O4

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15
Q

WHat is the formula of phosphoric acid?

A

H3PO4

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16
Q

What is the name of H2SO3

A

Sulfurous acid

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17
Q

What do oxalic, phosphoric, and sulfurous acid all have in common?

A

They are all moderately ionized

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18
Q

What is the formula for Hydrofluoric acid

A

HF

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19
Q

What is the name of HC2H3O2

A

Acetic acid

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20
Q

What is the formula for carbonic acid?

A

H2CO3

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21
Q

What is the formula for hydrosulfuric acid?

A

H2S

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22
Q

WHat do Hydrofluoric, Acetic, Carbonic, Hydrosulfuric, and most other acids have in common?

A

They are all slightly ionized

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23
Q

Acids react with bases to form water and a ______

A

salt

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24
Q

The act of an acid reacting with a base is called

A

Neutralization

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25
WHat is the general equation for neutralization
Acid + Base = Salt + water
26
Acids react with _______ to release CO2
Carbonates
27
What is the Arrhenius Theory?
An acid is a substance that yields hydrogen ions in an aqueous solution
28
Are there really separate hydrogen ions in an aqueous solution?
No, they are usually bonded to the oxygen in the water molecule (Since the water is polar) and become H3O
29
While it is expressed a hydrogen ion when talking about an acidic solution, what are we really talking about?
Hydronium (H30)
30
What is this: HX (Double arrows) H+ + X-
The general reaction for the dissociation of an acid
31
Bases are conductors of what in an aqueous solution?
Electricity
32
Similar to acids, the degree of condensation in bases depends on the degree of _____
ionization
33
Bases change what in indicators?
color
34
Bases react with acids to ______ each other to form a ____ and _______
Neutralize, salt, water
35
Bases react with what to form a class of compounds called soaps
Fats
36
Aqueous solutions of bases feel _____ while stronger bases are very ______ to the skin
Slippery, Caustic
37
What theory defines a base as a substance that yields hydroxide ions (OH-) in an aqueous solution
The Arrhenius Theory
38
WHat is the formula of Potassium hydroxide
KOH
39
What is the name of NaOH
Sodium hydroxide
40
What is the name of Ba(OH)2
Barium hydroxide
41
What is the formula for Strontium hydroxide?
Sr(OH)2
42
What is the formula for calcium hydroxide
Ca(OH)2
43
What do KOH, NaOH, Ba(OH)2, Sr(OH)2, and Ca(OH)2 have in common?
They are all completely or nearly completely ionized
44
What is an example of a slightly ionized base?
Ammonium hydroxide
45
What is the formula for Ammonium hydroxide
NH4(OH)
46
What is the Bronsted-Lowry Theory
It states how acids are proton donors and bases are proton acceptors.
47
In an acid-base reaction, the original acid gives up its proton and becomes a ________
conjugate base
48
What a base accepts a proton from an acid, it becomes a _____________
conjugate acid
49
If an acid is strong then it will give up protons ______
easily
50
The stronger an acid it, the ______ its conjugate base will be
Weaker
51
The stronger the base, the ________ its conjugate acid
weaker
52
Proton transfer reactions favor the production of what?
Weaker bases and weaker acids
53
The reactants (Acids and bases) must much ______ compared to the products
stronger
54
What is Lewis Theory
An acid is an electron pair acceptor and a base is an electron pair donor
55
What can PH be defined as (hint: math)
-Log[H+]
56
What is [H+] in the formula -Log[H+]
The concentration of hydrogen ions in moles per liter
57
What is the [H+] concentration of water
10^-7, in other words: 7
58
pH + pOH = ?
14
59
What are buffer solutions
systems that resist change in acidity and maintain a constant ph level even if acids and bases are added.
60
In a lab setting, how does one create a buffer?
One could mix equal molar quantities of a weak acid and its salt
61
What is a salt
it is an ionic compound containing positive ions other than hydrogen ions, and negative ions other than hydroxide ions
62
How do you create a salt?
By neutralizing the appropriate acid and base to create a salt and water
63
An active metal replaces hydrogen in an acid by single replacement to do what?
create a salt
64
When you combine two elements to create a salt
combustion
65
Similar to single replacement in the fact that it replaces ions to create salt (1 soluble, 1 not soluble)
Double replacement
66
To create a salt one could react a _____ with a _________
metallic oxide and nonmetallic oxide
67
What are Amphoteric substances?
Substances that can either donate protons or receive them depending on the substance they come into contact with.
68
When do Amphoteric substance donate protons
In the presence of strong bases
69
When do Amphoteric substance accept protons
In the presence of strong acids
70
What forms when oxides of sulfur and nitrogen combine with atmospheric moisture to yield sulfuric and nitric acids
Acid rain

Chemistry SAT (5 decks)

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