Acids and Bases

Question 1

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

Answer 1

Bleach and Vinegar

Question 2

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

Answer 2

Bleach and Ammonia

Question 3

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

Answer 3

Bleach and Rubbing Alcohol

Question 4

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

Answer 4

Hydrogen Peroxide and Vinegar

Question 5

• 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

Answer 5

Naming Binary Acids

Question 6

• 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.

Answer 6

Naming Oxyacids and Oxysalts

Question 7

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

Answer 7

Arrhenius Definition

Question 8

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

Answer 8

Bronsted-Lowry Definition

Question 9

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

Answer 9

Lewis Definition

Question 10

• 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-

Answer 10

Arrhenius Acid-Base Definition

Question 11

When an acid reacts with a base.

Answer 11

Neutralization

Question 12

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

Answer 12

Strong Acid

Question 13

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

Answer 13

Weak Acids

Question 14

Indication of acid strength.

Answer 14

Value of Ka

Question 15

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

Answer 15

Larger; Smaller

Question 16

• 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+

Answer 16

Bronsted-Lowry Acid-Base Definition

Question 17

Acid-base reaction.

Answer 17

Proton-transfer Process

Question 18

A Brønsted–Lowry acid must contain a ____ atom.

Answer 18

Hydrogen

Question 19

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

Answer 19

Lone Pairs

Question 20

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

Answer 20

OH-

Question 21

Product formed by loss of a proton from an acid.

Answer 21

Conjugate Base

Question 22

Product formed by gain of a proton by a base.

Answer 22

Conjugate Acid

Question 23

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

Answer 23

Net Direction of an Acid-Base Reaction

Question 24

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

Answer 24

Weaker

Question 25

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

Answer 25

Right

Question 26

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

Answer 26

Amphoteric Compound

Question 27

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

Answer 27

Autoionization or Self-Ionization

Question 28

**Acid** dissociation constant.

Answer 28

Ka

Question 29

**Ion-product** constant for water.

Answer 29

Kw

Question 30

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

Answer 30

Inverse

Question 31

* **Acidic** solution: ____ [H3O+] * **Neutral** solution: ____ [H3O+] and [OH-] * **Basic** solution: ____ [OH-]

Answer 31

* Higher * Equal * Higher

Question 32

* pH of a solution indicates its **relative acidity**. * ____: pH < 7.00 * ____: pH = 7.00 * ____: pH > 7.00

Answer 32

* Acidic * Neutral * Basic

Question 33

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

Answer 33

Lower; Less

Question 34

A **low pKa** corresponds to a ____ Ka.

Answer 34

High

Question 35

If **pH increases**, pOH ____.

Answer 35

Decreases

Question 36

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

Answer 36

Buffer

Question 37

**Most buffers** are solutions composed of roughly **equal amounts** of

Answer 37

Weak Acid and Salt of its Conjugate Base

Question 38

Added ____, OH− reacts with the **weak acid**.

Answer 38

Base

Question 39

Added ____, H3O+ reacts with the **conjugate base**.

Answer 39

Acid

Question 40

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.

Answer 40

Acid

Question 41

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.

Answer 41

Base

Question 42

**Effective** pH range of a buffer depends on its ____.

Answer 42

Ka

Question 43

**Normal** blood pH is between ____ and ____.

Answer 43

7.35 and 7.45

Question 44

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

Answer 44

Respiratory Acidosis

Question 45

* Caused by **hyperventilating**; **very little CO2** is produced by the body. * Faster RR = decreases [CO2]

Answer 45

Respiratory Alkalosis