Acids and Bases

Question 1

Arrhenius Acid

Answer 1

Substances that produces H+ ions in aqueous solutions

Question 2

Arrhenius Base

Answer 2

Substances that produce OH- ions in aqueous solutions

Question 3

Bronsted-Lowry Acid

Answer 3

Proton (H+) Donor

Question 4

Arrhenius vs Bronsted Definitions

Answer 4

BL Definition: Focuses on H+ transfer in acid-base reactions

–> ALL Arrhenius acids/bases are BL acids/bases

–> Not all BL acids/bases are Arrhenius acids/bases

Question 5

Bronsted-Lowry Base

Answer 5

Proton (H+) Acceptor

Question 6

Amphoteric

Answer 6

Able to act as either an acid or base (dual nature)

–> Like water (produces both OH- and H+ when dissociating)

Question 7

Conjugate Acid-Base Pairs

Answer 7

2 substances related to each other by the transfer of ONE proton

Question 8

Acid and Conjugate Base

Answer 8

Acid = Proton donor

Conj. Base = The resulting form of acid with H+ removed (becomes capable of accepting H+)

–> Any acid from which a proton (H+) is removed

Question 9

Base and Conjugate Acid

Answer 9

Base = Proton acceptor

Conj. Acid = The resulting form of base with H+ added (becomes capable of donating H+)

–> Any base to which a proton (H+) is added

Question 10

Strong Acids

Answer 10

Ionizes completely in solution

–> H+ and A- attraction = weak (ionizes more easily)

Question 11

Weak Acids

Answer 11

Ionizes incompletely in solution

–> H+ and A- attraction = strong (more difficult to ionize/separate)

Question 12

The stronger the acid…

Answer 12

the weaker the conjugate base

(and the other way around)

Question 13

6 Main Strong Acids

Answer 13

1) HCl
2) Hbr
3) HI
4) HNO3
5) HClO4
6) H2SO4

Question 14

Acid Ionization Constant

Answer 14

Ka = The equilibrium constant for the ionization rxn. of weak acids

Question 15

The smaller the Ka…

Answer 15

The weaker the acid

Question 16

Autoionization

Answer 16

When water acts as an acid and base within itself

K = [OH-][H+]

Question 17

Ion Product Constant for Water

Answer 17

Kw = Equilibrium constant for auto-ionization of water

Kw = 1.0 x 10^-14 AT 25C
[OH-][H+] = 1.0 x 10^-4

–> In pure water, [OH-]=[H+] (Neutral)

Question 18

Neutral Solution

Answer 18

[OH-] = [H+]

Question 19

Acidic Solution

Answer 19

[H+] > [OH-]

Question 20

Basic Solution

Answer 20

[OH-] > [H+]

Question 21

pH

Answer 21

A logarithmic scale specifying the acidity of a solution

–> pH = -log[H+]

pH < 7 = Acidic
pH = 7 = Neutral
pH > 7 = Basic

Question 22

pOH

Answer 22

A log scale exactly like pH except in respect to OH- instead

–> pOH = -log[OH-]

pOH < 7 = Basic
pOH = 7 = Neutral
pOH > 7 = Acidic
(inverted scale)

Question 23

Determining [H3O+] from Strong Acids

Answer 23

[HA] = [H3O+]

–> Completely ionizes, therefore conc. of acid = conc. of H+ produced

Question 24

Determining [H3O+] from Weak Acids

Answer 24

[HA] DOES NOT = [H3O+]

–> Need to use ICE table to determine value

Question 25

Percent Ionization

Answer 25

Quantification of the ionization of a weak acid according to the % of molecules that actually ionize

% ion. = [H+]/[HA] * 100%

Question 26

Converting Between pH and pOH

Answer 26

pH + pOH = 14

Question 27

Percent ionization increases as…

Answer 27

Concentration of acid decreases (= smaller denominator)