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Honors Chemistry > Ch 15 Test > Flashcards

Ch 15 Test Flashcards

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
Q

Which are conjugate acid-base pairs from the equilibrium reaction H2O(l) + NH3(aq) ⇌ NH+4(aq) + OH–(aq)?

A

H2O and OH–

NH3 and NH+4

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26
Q

Which are described as amphoteric?

A

water and other substances that can act as both acids and bases

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27
Q

Two substances related to each other by the donating and accepting of a single hydrogen ion make up a _____ acid-base ______.

A

Conjugate, pair

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28
Q

What is a monoprotic acid?

A

a substance that can donate only one hydrogen ion

29
Q

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.

A

Polar, nonpolar

30
Q

An acid that can donate more than one hydrogen ion is called a ______ ______.

A

Polyprotic acid

31
Q

What is the Lewis model?

A

An acid is an electron-pair acceptor and a base is an electron-pair donor.

32
Q

Water and other substances that can act as both acids and bases are described as being ______.

A

Amphoteric

33
Q

An acid that can donate only one hydrogen ion is called a _______ _______.

A

Monoprotic acid

34
Q

Which describes the connection between ionizable hydrogen atoms and bond polarity in an acid?

A

Ionizable hydrogen atoms are connected to the other atom(s) in the molecule by polar bonds.

35
Q

What is a polyprotic acid?

A

a substance that can donate more than one hydrogen ion

36
Q

An acid is an electron-pair acceptor and a base is an electron-pair donor in the _______ model.

A

Lewis

37
Q

Metal oxides are _____ anhydrides, and nonmetal oxides are ____anhydrides.

A

Base, acid

38
Q

Which anhydrides are identified correctly?

A

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
Q

Which statements about the strength of acids are true?

A

Strong acids ionize completely.

Weak acids do not ionize completely.

40
Q

An acid that ionizes only partially in dilute aqueous solution is a(n) _______ ________.

A

Weak acid

41
Q

Which is a strong acid?

A

an acid that ionizes completely

42
Q

A weak acid has a _____ conjugate base.

A

Strong

43
Q

Which is the acid ionization constant?

A

the value of the equilibrium constant expression for the ionization of a weak acid

44
Q

What happens to the strength of an acid as the acid ionization constant decreases?

A

The strength of the acid decreases.

45
Q

Which is a weak acid?

A

an acid that ionizes only partially in dilute aqueous solution

46
Q

A base that dissociates entirely into metal ions and hydroxide ions is a(n) ____ ______.

A

Strong base

47
Q

How does the strength of a weak acid compare with the strength of its conjugate base?

A

A weak acid has a strong conjugate base.

48
Q

A base that ionizes only partially in dilute aqueous solution is a(n) ______ ______.

A

Weak base

49
Q

The strength of a base decreases as the base ionization constant ______.

A

Decreases

50
Q

In the self-ionization of water, equal numbers of hydronium and ______ ions are formed.

A

Hydroxide

51
Q

The value of the equilibrium constant expression for the self-ionization of water is called the _______ ______ _____.

A

Ion product constant

52
Q

Which describe how changes in the concentrations of hydrogen ions and hydroxide ions in an aqueous solution are related?

A

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
Q

Which is pH?

A

the negative logarithm of the hydrogen ion concentration of a solution

54
Q

What is the result of the self-ionization of water?

A

Equal numbers of hydronium and hydroxide ions form.

55
Q

As the concentration of hydrogen ions in a solution increases, the concentration of hydroxide ions in the solution _______.

A

Decreases

56
Q

The negative logarithm of the hydrogen ion concentration of a solution is ______.

A

pH

57
Q

The negative logarithm of the hydroxide ion concentration of a solution is _______.

A

pOH

58
Q

Which is the pH of an aqueous solution?

A

–log[H+]

59
Q

Which is pOH?

A

the negative logarithm of the hydroxide ion concentration of a solution

60
Q

To determine the pH of an aqueous solution, determine the negative logarithm of the _______ ______ concentration.

A

Hydrogen ion

61
Q

The sum of the pH and the pOH of a solution is ______.

A

14

62
Q

Which is the pOH of an aqueous solution?

A

–log[OH–]

63
Q

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.

A

True because every molecule of a strong acid produces one hydrogen ion because a strong acid ionizes completely.

64
Q

The pH of a strong monoprotic acid solution can be calculated using which concentration?

A

the concentration of the acid

65
Q

The concentration of the weak acid HF at equilibrium is equal to the initial concentration of the acid ______ the moles per liter of H+.

A

Minus

66
Q

Which method uses the color changes of several indicators to measure the pH of a solution?

A

pH paper

67
Q

Place the following steps in the order you would use to calculate the Ka

A
  1. Measure the pH of the solution
  2. Calculate [H+]
  3. Infer [F-] and [HF]
  4. Solve the Ka expression
68
Q

The pH of a solution can be measured using an electronic device called a _____ _____.

A

pH meter

Honors Chemistry (13 decks)

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