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Honors Chemistry > Ch 15 Test > Flashcards

Ch 15 Test Flashcards

(68 cards)

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1
Q

Acids in your stomach help you _____ what you eat.

A

Digest

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2
Q

Which are common uses of bases?

A

soap

relieving an upset stomach

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3
Q

Foods that contain acidic solutions have a _____ taste.

A

Sour

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4
Q

Basic solutions tend to taste ______.

A

Bitter

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5
Q

Acids and bases can be identified by their reactions with ______ paper, ___________, and _________ carbonates.

A

Litmus, metals, metal

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6
Q

Which are common uses of acids?

A

digestion of food

defense mechanism of ants

flavoring for beverages

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7
Q

Which action involves a common use of a base?

A

washing hands

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8
Q

Acidic solutions tend to taste ______.

A

sour

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9
Q

Which types of solution are correctly classified based on the relative amounts of hydrogen ions and hydroxide ions?

A

A basic solution has more hydroxide ions than hydrogen ions.

A neutral solution has equal concentrations of hydrogen ions and hydroxide ions.

An acidic solution has more hydrogen ions than hydroxide ions.

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10
Q

Basic solutions, such as soapy water, have a ______ feel.

A

Slippery

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11
Q

Acids and bases can be identified by their reactions with which of the following?

A

metals

metal carbonates

litmus paper

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12
Q

What is an acidic solution?

A

a solution that contains more hydrogen ions than hydroxide ions

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13
Q

What is the Arrhenius model?

A

An acid ionizes to produce hydrogen ions; a base contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution.

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14
Q

When hydrogen chloride gas dissolves in water, what occurs that makes hydrogen chloride an Arrhenius acid?

A

Its molecules ionize to form hydrogen ions.

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15
Q

When sodium hydroxide dissolves in water, it dissociates to form _______ ions, which makes sodium hydroxide a(n) ________ base.

A

Hydroxide, Arrhenius

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16
Q

A solution that contains more hydroxide ions than hydrogen ions is a(n) _______ ________.

A

Basic solution

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17
Q

An acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor in the _______ ______ model.

A

Bronsted Lowry

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18
Q

An acid ionizes to produce hydrogen ions and a base contains a hydroxide group and dissociates to produce hydroxide ions in aqueous solution, according to the _______ model.

A

Arrhenius

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19
Q

When sodium hydroxide dissolves in water, what occurs that makes sodium hydroxide an Arrhenius base?

A

It dissociates to form hydroxide ions.

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20
Q

What is a conjugate acid?

A

the species produced when a base accepts a hydrogen ion

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21
Q

What is the Brønsted-Lowry model?

A

An acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.

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22
Q

What is a conjugate base?

A

the species that results when an acid donates a hydrogen ion

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23
Q

What is a conjugate acid-base pair?

A

two substances related to each other by the donating and accepting of a single hydrogen ion

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24
Q

Which are conjugate acid-base pairs from the equilibrium reaction

H2O(l) + HF(aq) ⇌ F–(aq) + H3O+(aq)?

A

H3O+ and H2O

HF and F–

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25
Which are conjugate acid-base pairs from the equilibrium reaction H2O(l) + NH3(aq) ⇌ NH+4(aq) + OH–(aq)?
H2O and OH– NH3 and NH+4
26
Which are described as amphoteric?
water and other substances that can act as both acids and bases
27
Two substances related to each other by the donating and accepting of a single hydrogen ion make up a _____ acid-base ______.
Conjugate, pair
28
What is a monoprotic acid?
a substance that can donate only one hydrogen ion
29
In an acid molecule, an ionizable hydrogen atom is connected to the molecule by a(n) _____ covalent bond while a hydrogen atom that is not ionizable is connected by a(n) _____ covalent bond.
Polar, nonpolar
30
An acid that can donate more than one hydrogen ion is called a ______ ______.
Polyprotic acid
31
What is the Lewis model?
An acid is an electron-pair acceptor and a base is an electron-pair donor.
32
Water and other substances that can act as both acids and bases are described as being ______.
Amphoteric
33
An acid that can donate only one hydrogen ion is called a _______ _______.
Monoprotic acid
34
Which describes the connection between ionizable hydrogen atoms and bond polarity in an acid?
Ionizable hydrogen atoms are connected to the other atom(s) in the molecule by polar bonds.
35
What is a polyprotic acid?
a substance that can donate more than one hydrogen ion
36
An acid is an electron-pair acceptor and a base is an electron-pair donor in the _______ model.
Lewis
37
Metal oxides are _____ anhydrides, and nonmetal oxides are ____anhydrides.
Base, acid
38
Which anhydrides are identified correctly?
A metal oxide is a base anhydride, and a nonmetal oxide is an acid anhydride. Carbon dioxide is an acid anhydride, and calcium oxide is a base anhydride.
39
Which statements about the strength of acids are true?
Strong acids ionize completely. Weak acids do not ionize completely.
40
An acid that ionizes only partially in dilute aqueous solution is a(n) _______ ________.
Weak acid
41
Which is a strong acid?
an acid that ionizes completely
42
A weak acid has a _____ conjugate base.
Strong
43
Which is the acid ionization constant?
the value of the equilibrium constant expression for the ionization of a weak acid
44
What happens to the strength of an acid as the acid ionization constant decreases?
The strength of the acid decreases.
45
Which is a weak acid?
an acid that ionizes only partially in dilute aqueous solution
46
A base that dissociates entirely into metal ions and hydroxide ions is a(n) ____ ______.
Strong base
47
How does the strength of a weak acid compare with the strength of its conjugate base?
A weak acid has a strong conjugate base.
48
A base that ionizes only partially in dilute aqueous solution is a(n) ______ ______.
Weak base
49
The strength of a base decreases as the base ionization constant ______.
Decreases
50
In the self-ionization of water, equal numbers of hydronium and ______ ions are formed.
Hydroxide
51
The value of the equilibrium constant expression for the self-ionization of water is called the _______ ______ _____.
Ion product constant
52
Which describe how changes in the concentrations of hydrogen ions and hydroxide ions in an aqueous solution are related?
An increase in the concentration of hydroxide ions causes a decrease in the concentration of hydrogen ions. An increase in the concentration of hydrogen ions causes a decrease in the concentration of hydroxide ions.
53
Which is pH?
the negative logarithm of the hydrogen ion concentration of a solution
54
What is the result of the self-ionization of water?
Equal numbers of hydronium and hydroxide ions form.
55
As the concentration of hydrogen ions in a solution increases, the concentration of hydroxide ions in the solution _______.
Decreases
56
The negative logarithm of the hydrogen ion concentration of a solution is ______.
pH
57
The negative logarithm of the hydroxide ion concentration of a solution is _______.
pOH
58
Which is the pH of an aqueous solution?
–log[H+]
59
Which is pOH?
the negative logarithm of the hydroxide ion concentration of a solution
60
To determine the pH of an aqueous solution, determine the negative logarithm of the _______ ______ concentration.
Hydrogen ion
61
The sum of the pH and the pOH of a solution is ______.
14
62
Which is the pOH of an aqueous solution?
–log[OH–]
63
True or false: The concentration of a strong, monoprotic acid can be used as the hydrogen ion concentration to calculate the pH of the solution.
True because every molecule of a strong acid produces one hydrogen ion because a strong acid ionizes completely.
64
The pH of a strong monoprotic acid solution can be calculated using which concentration?
the concentration of the acid
65
The concentration of the weak acid HF at equilibrium is equal to the initial concentration of the acid ______ the moles per liter of H+.
Minus
66
Which method uses the color changes of several indicators to measure the pH of a solution?
pH paper
67
Place the following steps in the order you would use to calculate the Ka
1. Measure the pH of the solution 2. Calculate [H+] 3. Infer [F-] and [HF] 4. Solve the Ka expression
68
The pH of a solution can be measured using an electronic device called a _____ _____.
pH meter

Honors Chemistry (13 decks)

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