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9 Flashcards

1
Q

substance that produces H3O+ ions in aqueous solution

A

acid

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2
Q

substance that produces OH2 ions in aqueous solution

A

a base

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3
Q

H1 ion in water immediately combines with an H2O molecule to give a

A

hydronium ion

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3
Q

produces hydrogen ions, H+

A

acid

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4
Q

A base that ionizes completely in aqueous solution

A

Strong base

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4
Q

An acid that ionizes completely in aqueous solution

A

Strong acid

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4
Q

An acid that is only partially ionized in aqueous solution

A

Weak acid

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5
Q

Strong Acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO4

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5
Q

four common strong bases

A

LiOH, NaOH, KOH, Ba(OH)2

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5
Q

the acid in the gastric fluid in your stomach

A

HCl

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5
Q

also called lye

A

NaOH

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5
Q

one of the most widely produced single chemicals in the United States.

A

sulfuric acid

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5
Q

an important acid in chemistry laboratories

A

Hydrochloric acid

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5
Q

Pure acetic acid is called

A

glacial acetic acid

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5
Q

causes the skin to turn yellow because the acid reacts with skin proteins

A

Nitric acid

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5
Q

Pure acetic acid melting point

A

17°C

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5
Q

were once used as antiseptics, especially for eyes

A

Boric acid

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5
Q

An acid that can give up two protons

A

Diprotic acid

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5
Q

In the Brønsted Lowry theory, a substance formed when an acid donates a proton to another molecule or ion

A

Conjugate base

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6
Q

one of the strongest of the weak acids

A

Phosphoric acid

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6
Q

he most important weak base, is a
gas with many industrial uses

A

Ammonia

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7
Q

used in many industrial processes, including the manufacture of glass and soap

A

Sodium hydroxide

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7
Q

weaker solutions are used as “spirits of ammonia” to revive people who have fainted

A

Ammonia

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8
Q

An acid that can give up only one proton

A

Monoprotic acid

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8
Q

called milk of magnesia and is used as a laxative

A

Magnesium hydroxide

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8
Q

A pair of molecules or ions that are related to one another by the gain or loss of a proton

A

Conjugate acid–base pair

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9
Q

A base that is only partially ionized in aqueous solution

A

Weak base

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10
Q

Acids react with metal hydroxides to give

A

salt and water

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11
Q

In the Brønsted Lowry theory, a substance formed
when a base accepts a proton

A

Conjugate acid

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11
Q

the outermost part of the eye

A

cornea

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12
Q

pH of urine can vary from

A

5.5 to 7.5

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12
Q

An acid that can give up three protons

A

Triprotic acid

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12
Q

the equilibrium position always favors reaction of the

A

stronger acid and stronger base to form the weaker acid and weaker base

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12
Q

burns by bases can later develop

A

ulcerations in which the healing wound deposits scar tissue that is not transparent

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13
Q

the cornea is a tissue with no blood vessels and, therefore

A

can be transplanted without immunological rejection
problems

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13
Q

A substance that can act as either an acid or a base

A

Amphiprotic

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13
Q

type can also cause severe damage

A

bases

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14
Q

An equilibrium constant for the ionization of an acid in aqueous solution to H3O1 and its conjugate base; also called an acid dissociation constant

A

Acid ionization constant (Ka)

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14
Q

Strong acids react with certain metals (called active metals) to produce

A

hydrogen gas, H2, and a salt

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14
Q

most important reaction of acids and bases

A

neutralization

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15
Q

pH is less than 7.0

A

acidic

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15
Q

reaction of an acid with an active metal to give a salt and hydrogen gas is a

A

redox reaction

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16
Q

Strong acids react with metal oxides to give

A

water and a salt

16
Q

salt formed in the reaction of acid with metal hydroxide is

A

an ionic compound

17
Q

strong acid is added to a carbonate

A

bubbles of carbon dioxide gas are rapidly given off

17
Q

you probably have gotten “heartburn” caused by

A

excess stomach acidity

17
Q

strong acid is added to a carbonate overall reaction

A

summation of two reactions

17
Q

a substance that neutralizes acids

A

antacid

17
Q

two reactions involved in the reaction of strong acid and carbonate

A

-carbonate ion reacts with H3O to give carbonic acid
-carbonic acid decomposes to carbon dioxide and water

18
Q

reduce the secretion of acid into the stomach

A

acid reducers

18
Q

bases used in antacid

A

CaCO3, Mg(OH)2, Al(OH)3, and NaHCO3

18
Q

Any acid stronger than ____ is strong enough to react with NH3

A

NH4

19
Q

For a weak acid that imparts little or no flavor, bakers use

A

sodium dihydrogen phosphate, NaH2PO4, or potassium dihydrogen phosphate, KH2PO4

20
Q

pH is greater than 7.0

A

basic

21
Q

pH is equal to 7.0

A

neutral

22
Q

pH of blood

A

between 7.35 and 7.45

23
Q

Tomato juice

A

4.0–4.4

23
Q

a substance that changes color at a certain pH

A

pH indicator

23
Q

Vinegar

A

2.4–3.4

24
Q

Battery acid

A

0.5

24
Q

Gastric juice

A

1.0–3.0

24
Q

Lemon juice

A

2.2–2.4

25
Q

Black coffee

A

5.0–5.1

25
Q

Rain (unpolluted)

A

6.2

26
Q

Carbonated beverages

A

4.0–5.0

26
Q

Sea water

A

8.0–9.0

27
Q

The closer the pH of the buffer is to the of the weak
acid

A

the greater the buffer capacity

27
Q

Pancreatic fluid

A

7.8–8.0

27
Q

Milk

A

6.3–6.6

27
Q

Bile

A

6.8–7.0

28
Q

Saliva

A

6.5–7.5

29
Q

Soap

A

8.0–10.0

29
Q

Household ammonia

A

11.7

29
Q

Milk of magnesia

A

10.5

29
Q

analytical procedure whereby we react a known volume of a solution of known concentration with a known volume of a solution of unknown concentration

A

Titration

30
Q

Lye (1.0 M NaOH)

A

14.0

31
Q

point at which there is an equal amount of acid and base in a neutralization reaction

A

equivalence point

31
Q

point at which an indicator changes color is called

A

end point

32
Q

solution that resists change in pH when limited
amounts of an acid or a base are added to it; an aqueous solution containing a weak acid and its conjugate base

A

Buffer

32
Q

a method for determining the total acid or base concentration of a solution

A

titration

32
Q

consist of approximately equal amounts of a weak acid and its conjugate base

A

Buffer

33
Q

resists any change in pH upon the addition of small quantities of acid or base

A

buffer

34
Q

when the conjugate base of the weak acid removes H3O it is converted to the

A

undissociated weak acid

34
Q

The greater the concentration of the weak acid and its
conjugate base

A

the greater the buffer capacity

34
Q

the amount of hydronium or hydroxide ions that a buffer can absorb without a significant change in its pH

A

Buffer capacity

34
Q

an acid–base “shock absorber.”

A

buffer

35
Q

In human blood, a change larger than ___ pH unit
in either direction may cause illness

A

0.10

36
Q

most important of these systems for blood

A

carbonate buffer

36
Q

is a mathematical relationship between pH, the pKa of a weak acid, and the concentrations of the weak acid and its conjugate base

A

Henderson-Hasselbalch

37
Q

for acids, which lower the ratio and thus

A

improve buffer efficiency

37
Q

than for bases, which raise the ratio and

A

decrease buffer capacity

38
Q

second most important buffering system of the blood is a phosphate buffer made up of

A

hydrogen phosphate ion, HPO4, and dihydrogen phosphate ion, H2PO4

39
Q

the pH goes lower than 7.35 and 7.45.

A

the condition is called acidosis

39
Q

Cause of acidosis

A

respiratory acidosis

40
Q

hyperventilation in athlete

A

they force extra CO2 out of their lungs which causes more H2CO3 to dissociate into CO2 and H2O to replace the lost CO. The loss of the HA form of the bicarbonate blood buffer raises the pH of the blood.

40
Q

results from difficulty in breathing

A

hypoventilation

40
Q

pH of the blood decreases when holding breath in the water because

A

the CO2, unable to escape fast enough, remains in the blood, where it lowers the [HCO ]/[H2CO3] ratio

41
Q

Two causes of metabolic acidosis

A

starvation (or fasting) and heavy exercise

41
Q

starvation

A

body doesn’t get enough food, it burns its own fat, and the products of this reaction are acidic compounds that enter the blood

42
Q

Heavy exercise

A

causes the muscles to produce excessive amounts of lactic acid, which makes muscles feel tired and sore

42
Q

disease diabetes mellitus produces acidic compounds

A

ketone bodies

43
Q

the lack of oxygen

A

oxygen debt

43
Q

pathway has lactic acid as an end product

A

glycolysis

44
Q

pH may also be elevated

A

alkalosis

45
Q

alkalosis

A

excessive loss of CO2 raises both the ratio
of [HCO ]/[H2CO3] and the pH

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