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CHEM 101 > Lecture 4: Acids and Bases II > Flashcards

Lecture 4: Acids and Bases II Flashcards

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1
Q

One that reacts completely with water to form H3O+ ions

A

Strong acid

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2
Q

One that reacts completely with water to form OH– ions

A

Strong base

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3
Q

A substance that dissociates only partially in water to produce H3O+ ions

A

Weak acid

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4
Q

A substance that only partially reacts with water to produce OH– ions

A

Weak base

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5
Q

A proton donor

A

Acid

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6
Q

A proton acceptor

A

Base

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7
Q

A proton-transfer reactio

A

Acid–base reaction

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8
Q

Any pair of molecules or ions that can be interconverted by transfer of a proton

A

Conjugate acid–base pair

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9
Q

do not require water as a reactan

A

Brønsted–Lowry definitions

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10
Q

One of the most important amphiprotic substances

A

H2O

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11
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

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12
Q

One whose pH is less than 7.0

A

Acidic solution

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13
Q

One whose pH is greater than 7.0

A

Basic solution

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14
Q

One whose pH is equal to 7.0

A

Neutral solution

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15
Q

A solution that resists change in pH when limited amounts of acid or base are added to it

A

pH buffer

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16
Q

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

A

Buffer capacity

17
Q

The average pH of human blood is close to

A

7.4

18
Q

H2CO3 and its conjugate base, HCO3-

A

Carbonate buffe

19
Q

H2PO4– and its conjugate base, HPO42-

A

Phosphate buffer

20
Q

were made from simple acids and bases, such as acetic acid, phosphoric acid, and citric acid and their conjugate bases

A

Biochemical Buffers

21
Q

A mathematical relationship between:
* pH
* pKa of the weak acid, HA
* The concentrations of HA and its conjugate base A–.

A

Henderson–Hasselbalch equation

CHEM 101 (12 decks)

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