Chapter 10- Acids And Bases

Question 1

Arrhenius acid vs base

Answer 1

Acid- dissociate to form excess of H+

Base- dissociate to form excess of OH-

Question 2

Brønsted-Lowry acid vs base

Answer 2

Acid- donates H+ ions

Base- accepts H+ ions

Question 3

Lewis acid vs base

Answer 3

Acid- electron pair acceptor

Base- electron pair donor

Question 4

One way a Lewis acid can be used in organic chemistry

Answer 4

As a catalyst

Question 5

Oxyanions to Oxyacids naming

Answer 5

• ite (less O) it will end with -ous acid.

- are (more O) if will end with -ic acid

Question 6

Amphoteric and amphiprotic

Answer 6

Amphoteric- both - and +

Amphiprotic- lose or gain a proton (H+)

Question 7

Water dissociation constant (Kw)

Answer 7

10^-14 (concentration of each ion- H3O+ and OH- - is 10^-7) ONLY TEMPERATURE DEPENDENT

Question 8

Smaller Ka or Kb means….

Answer 8

Weaker acid or weaker base

Question 9

Generally speaking Ka and Kb values…

Answer 9

Ka smaller than 1 = weak acid

Kb smaller than 1 = weak base (almost always amines)

Question 10

7 most common strong acids

Answer 10

1. HCl
2. HClO4
3. HClO3
4. HI
5. HBr
6. H2SO4
7. HNO3

Question 11

Find pH or pOH based on Ka or Kb

Answer 11

p value = m -0.n
Ex. Ka = 1.8 x 10^-5
So 5 - 0.18 = 4.82

Question 12

Acetic acid

Answer 12

CH3COOH

Question 13

Mathematical relationship between Ka, Kb, and Kw

Answer 13

Ka x Kb = Kw

Question 14

Buffers and 2 examples

Answer 14

Weak acid or base and its salt. Ex: acetic acid and sodium acetate. Ex2: ammonia and ammonium chloride

Question 15

Sodium acetate

Answer 15

CH3COO-Na+

Question 16

Ammonia

Answer 16

NH3

Question 17

Ammonium chloride

Answer 17

NH4+Cl-

Question 18

Bicarbonate buffer system

Answer 18

H2CO3 and HCO3- are in the blood plasma to keep its pH within the narrow range. Tied to respiratory system and breathing out CO2 which is not very soluble.

Question 19

Estimate pH or pOH of buffer solution

Answer 19

pH= pKa + log (base/acid) OR pH= pKb + log (acid/base)

Question 20

When does pH = pKa?

Answer 20

Half equivalence points in a titration. Buffering capacity is also optimal at this pH

Question 21

Where Ka and equivalence points are on a titration curve?

Answer 21

Assuming pH is y-axis and volume added is x-axis.

pKa is the middle of the horizontal line and equivalence point is middle of the vertical line.

Question 22

Gram equivalence weight

Answer 22

Molar mass / number of acidic or basic equivalence included

Question 23

Generally How to answer dissociation questions given molarity and Ka

Answer 23

Ka = x^2 / molarity