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CHE > Acids and Bases > Flashcards

Acids and Bases Flashcards

1
Q

Do not mix: ____ and ____
* Produces chlorine gas which can cause coughing, breathing problems, burning and watery eyes.

A

Bleach and Vinegar

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2
Q

Do not mix: ____ and ____
* Produce a toxic gas called chloramine that causes shortness of breath and chest pain.

A

Bleach and Ammonia

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3
Q

Do not mix: ____ and ____
* Makes chloroform which is highly toxic.

A

Bleach and Rubbing Alcohol

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4
Q

Do not mix: ____ and ____
* This combination makes peracetic or peroxyacetic acid which can be highly corrosive.

A

Hydrogen Peroxide and Vinegar

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5
Q
  • Prefix hydro- is used to represent hydrogen, followed by the name of the nonmetal with its ending replaced by the suffix –ic and the word acid added.
  • HCl: Hydrochloric Acid
  • HBr: Hydrobromic Acid
A

Naming Binary Acids

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6
Q
  • Replace hydrogen with a metal = oxysalt.
  • A salt is a compound consisting of a metal and a non-metal.
  • If the salt consists of a metal, a nonmetal, and oxygen it is called an oxysalt.
A

Naming Oxyacids and Oxysalts

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7
Q

Acid: H+ or H3O+ producer.
Base: OH- producer.

A

Arrhenius Definition

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8
Q

Acid: Proton (H+) donor.
Base: Proton (H+) acceptor.

A

Bronsted-Lowry Definition

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9
Q

Acid: Electron-pair acceptor.
Base: Electron-pair donor.

A

Lewis Definition

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10
Q
  • Earliest acid-base definition, which classifies these substances in terms of their behavior in water.
  • Acid is a substance with H in its formula that dissociates to yield H3O+
  • Base is a substance with OH in its formula that dissociates to yield OH-
A

Arrhenius Acid-Base Definition

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11
Q

When an acid reacts with a base.

A

Neutralization

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12
Q
  • Acid that dissociates completely into ions in water.
  • Its dilute solution contains no HA molecules.
A

Strong Acid

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13
Q
  • Acid that dissociates slightly to form ions in water.
  • Its dilute solution, most HA molecules are undissociated.
A

Weak Acids

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14
Q

Indication of acid strength.

A

Value of Ka

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15
Q
  • Stronger acid: higher H3O+ = ____ Ka.
  • Weaker acid: lower % dissociation of HA = ____ Ka.
A

Larger; Smaller

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16
Q
  • Acid is a proton donor, any species that donates an H+ ion. Acid must contain H in its formula.
  • Base is a proton acceptor, any species that accepts an H+ ion. Base must contain a lone pair of electrons to bond to H+
A

Bronsted-Lowry Acid-Base Definition

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17
Q

Acid-base reaction.

A

Proton-transfer Process

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18
Q

A Brønsted–Lowry acid must contain a ____ atom.

A

Hydrogen

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19
Q
  • Make neutral compounds bases.
  • (N)H3 - ammonia
  • H2(O) - water
A

Lone Pairs

20
Q
  • Base in each metal salt.
  • Na(OH) - sodium hydroxide
  • K(OH) - potassium hydroxide
  • Mg(OH)2 - magnesium hydroxide
  • Ca(OH)2 - calcium hydroxide
A

OH-

21
Q

Product formed by loss of a proton from an acid.

A

Conjugate Base

22
Q

Product formed by gain of a proton by a base.

A

Conjugate Acid

23
Q

Depends on the relative strength of the acids and bases involved.

A

Net Direction of an Acid-Base Reaction

24
Q

The stronger the acid is, the ____ its conjugate base.

A

Weaker

25
Q

When an acid reacts with a base that is farther down the list, the reaction proceeds to the ____ (Kc > 1).

A

Right

26
Q
  • A compound that contains both a hydrogen atom and a lone pair of e−.
  • It can be either an acid or a base.
A

Amphoteric Compound

27
Q

Process where water dissociates very slightly into ions in an equilibrium.

A

Autoionization or Self-Ionization

28
Q

Acid dissociation constant.

A

Ka

29
Q

Ion-product constant for water.

A

Kw

30
Q
  • A change in [H3O+] causes an ____ change in [OH-], and vice versa.
  • Higher [H3O+] = lower [OH-]
  • Higher [OH-] = lower [H3O+]
A

Inverse

31
Q
  • Acidic solution: ____ [H3O+]
  • Neutral solution: ____ [H3O+] and [OH-]
  • Basic solution: ____ [OH-]
A
  • Higher
  • Equal
  • Higher
32
Q
  • pH of a solution indicates its relative acidity.
  • ____: pH < 7.00
  • ____: pH = 7.00
  • ____: pH > 7.00
A
  • Acidic
  • Neutral
  • Basic
33
Q

Higher the pH, the ____ the [H3O+] and the ____ acidic the solution.

A

Lower; Less

34
Q

A low pKa corresponds to a ____ Ka.

A

High

35
Q

If pH increases, pOH ____.

A

Decreases

36
Q

A solution whose pH changes very little when acid or base is added.

A

Buffer

37
Q

Most buffers are solutions composed of roughly equal amounts of

A

Weak Acid and Salt of its Conjugate Base

38
Q

Added ____, OH− reacts with the weak acid.

A

Base

39
Q

Added ____, H3O+ reacts with the conjugate base.

A

Acid

40
Q

If an ____ is added to the following buffer equilibrium, then the excess acid reacts with the conjugate base, so the overall pH does not change much.

A

Acid

41
Q

If a ____ is added to the following buffer equilibrium, then the excess base reacts with the conjugate acid, so the overall pH does not change much.

A

Base

42
Q

Effective pH range of a buffer depends on its ____.

A

Ka

43
Q

Normal blood pH is between ____ and ____.

A

7.35 and 7.45

44
Q
  • Results when the body fails to eliminate enough CO2, due to lung disease or failure.
  • Lower RR = increases [CO2]
A

Respiratory Acidosis

45
Q
  • Caused by hyperventilating; very little CO2 is produced by the body.
  • Faster RR = decreases [CO2]
A

Respiratory Alkalosis

CHE (1 decks)

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