chapter 12

Question 1

Arrhenius Definition

Answer 1

Acids: produce H+ ions in water
Bases: produce OH- ions in water

Question 2

Hydronium

Answer 2

H3O+

Question 3

Polyprotic

Answer 3

Can release more than one H+ into aqueous solution

Question 4

BrØnsted-Lowry definition

Answer 4

Acids: compounds that donate H+ ions
Bases: compounds that accept H+ ions

Question 5

Strong acids

Answer 5

completely ionize in water

Question 6

Weak acids

Answer 6

partially ionize in water

Question 7

equilibrium reactions

Answer 7

goes in both forward and backward directions

example: reactions of weak acids

Question 8

conjugate acid/base

Answer 8

the acid/ base on the R hand side of an equilibrium equation

Question 9

acid-base pair

Answer 9

the pair of an acid and a conjugate base or a base and a conjugate acid.
the conjugate to an acid/base is the same but without the H+

Question 10

acid-base neutralization reactions

Answer 10

acid+base—>water+”salt”

the formation of water drives neutralization reactions

Question 11

reactions of acids with metals

Answer 11

most metals react with acids to produce metal cations and hydrogen gas

Question 12

formation of acids from nonmetal oxides

Answer 12

often reacts with water to form acids

Question 13

self-ionization of water

Answer 13

2H2O(l) H3O+(aq)=OH-(aq)
H2O(l) H+(aq)+OH-(aq)
in pure water one out of every 560 million water molecules is ionized

Question 14

in pure water the concentration of H+ and OH-

Answer 14

[H+][OH-] = 1.0x10^-14

inversely? related, one goes up, the other goes down and vice versa. but their product always remains constant

Question 15

the pH scale

Answer 15

pH= -log[H+]
(-log(10^-7) = pH of 7)
strongly acidic: pH of 0
neutral: pH of 7
strongly basic: pH of 14