Module 11

Question 1

Lewis Acid

Answer 1

Electron acceptor

Question 2

Lewis Base

Answer 2

electron donor

Question 3

Bronsted-lowry Acid

Answer 3

proton donor

Question 4

Bronsted-Lowry Base

Answer 4

Proton acceptor

Question 5

Conjugate Pairs

Answer 5

A = CB
B = CA

Question 6

H20 is an Acid or Base?

Answer 6

Both; depending on the environment

Question 7

Can two strong or weak acids react together?

Answer 7

Yes, the labeling of acid and base is not absolute but rather its relative.

The stronger acid would be the acid

the weaker acid would act like the base

Question 8

Strong acids

Answer 8

HCI
HBr
HI
HNO3 (Nitric Acid)
HClO4 (Perchloric Acid)
H2SO4 (Sulfuric Acid)

Question 9

Weak Acids

Answer 9

HF
H2CO3 (Carbonic Acid)
H3PO4 (Phosphoric Acid)
organic acids (carboxylic acids, protonated drugs, etc)

Question 10

___ acid have ___ conjugate bases

Answer 10

Strong ; weak

Question 11

Strong bases

Answer 11

LiOH
NaOH
KOH
Sr(OH)2
Ca(OH)2
Ba(OH)2

Question 12

Weak Bases

Answer 12

Mg(OH)2
NH3 (ammonia)
transition metal hydroxides

Question 13

What is the difference between strong and weak bases/acids?

Answer 13

the complete or partially ionize when dissolved in water.

Strong Acid/Base = complete ionize
Weak acid/base = partially ionize

Question 14

water is amphoteric?

Answer 14

can act as either an acid or a base

Question 15

Water constant (Kw) is?

Answer 15

measure of the self ionization of water

Question 16

pH formula

Answer 16

(-) log [ H3O+ ]

or

(-) log [OH-]

**depends on the solution.

Question 17

Logarithmic scale?

Answer 17

change of 1 actually scales to a change by a factor of 10

Question 18

Limitation of pH scale?

Answer 18

highly concentrated and diluted samples of acid and bases

Question 19

Ka measures?

Answer 19

measure known as the acid-dissociation constant

Question 20

the larger the Ka =

Answer 20

the easier it is to remove the proton (more acidic)

Question 21

What can you use instead of Ka values?

Answer 21

pKa

(lower values = more acidic)

Question 22

What is the additional step needed when calculating the pH of a weak acid?

Answer 22

must calculate pH of equilibrium concentration!!! (more workkk)

Question 23

pH calculation of a strong acid?

easier calculation why?

Answer 23

using the ** negative** log of the given solution pH will result in the answer d/t the concept of strong acid fully dissociating in solution.

Question 24

steps for pH calculation of strong bases (single OH)

Answer 24

1. solve for pOH = (-log [OH-])
2. pH = 14 - pOH
3. actual pH of base solution

Question 25

steps for pH calculation of strong bases (double OH)

Answer 25

1. [OH-] = 2x[base w/ (OH) 2]
2. solve pOH = -Log [product from step #1]
3. solve for pH = 14 - pOH
4. actual pH of base solution

Question 26

Acid strength consist of?

Answer 26

relative and depends on the ability of the group to give up a proton.

Question 27

Range on pKa

Answer 27

(-20) to (>60)