Acids and Bases

Question 1

Bronsted Lowry Acid

Answer 1

Substance that can donate an H+ (a proton) in another substance
(loses a proton]

Question 2

Bronsted Lowry Base

Answer 2

a substance that can ACCEPT an H+ (a proton) from another substance
would gain a proton

Question 3

Hydronium

Answer 3

H3O+

Question 4

Arrhenius Acid

Answer 4

Substances that PRODUCE H+ ions when dissolved in water

Question 5

Arrhenius Bases

Answer 5

Substances that produce OH- ions when dissolved in water.

Question 6

calculate Ka from equilibrium expression

Answer 6

ka = [Product]^x [Product] ^x / [Reactant]^x [Reactant]^x

Question 7

How to make a conjugate base

Answer 7

Acid loses a proton

loses 1 H+

Question 8

Make Conjugate Acid

Answer 8

Base gains a proton

1 H+

Question 9

Conjugate Acid Base Pair (listing)

Answer 9

HA / A-
Acid / Conjugate Base
Conjugate Acid/ Base

Question 10

Kw

Answer 10

Kw= [H3O+][H-]
Kw = 1.0 x 10 ^-14 (@25 K)

Question 11

H3O+ and OH- : Neutral Solution

Answer 11

[H3O+] = [OH-]

Question 12

H3O+ and OH- : Acidic Solution

Answer 12

[H3O+] > [OH-]

Is greater than

Question 13

H3O+ and OH- : Basic Solution

Answer 13

[H3O+] < {OH-]

is less than

Question 14

pH of Acid

Answer 14

Less than 7

Question 15

pH of Base

Answer 15

more than 7

Question 16

pH pf Neutral

Answer 16

7

Question 17

Calculate pH

Answer 17

• log [ H3O+ ]

Question 18

Calculate pOH

Answer 18

• Log [ OH- ]

Question 19

calculate [ H3O+]

Answer 19

10 ^ - pH

Question 20

calculate [ OH- ]

Answer 20

10 ^ -pOH

Question 21

Calculate pKw

Answer 21

• Log ( Kw )

pH + pOH = 14 = pKw

Question 22

Characteristics of Strong Acids

Answer 22

• Ka&raquo_space; 1 ( ka much larger than 1 ) ((the higher ka the stronger the acid)
• 100% dissociation
• Large [H3O+] @ equilibrium
• Low pKa (the lower, the stronger the acid)

Question 23

Characteristics of Weak Acids

Answer 23

• ka «1 (ka less than 1, the smaller the weaker)
• Small % dissociation
• Small [H3O+] @ equilibrium
• High pKa (the higher, the weaker)