Chapter 16: Acid-Base Equilibria

Question 1

Bronsted Lowry ACID

Answer 1

donates a proton to another substance

Question 2

Bronsted Lowry BASE

Answer 2

accepts a proton from another substance

Question 3

Lowry NEUTRALIZATION

Answer 3

reaction between an acid and a base

Question 4

Lewis ACID

Answer 4

accepts a pair of electrons from a base

Question 5

Lewis BASE

Answer 5

donates a pair of electrons to an acid

Question 6

Lewis NEUTRALIZATION

Answer 6

an electron pair transfer from a base to an acid

Question 7

acids

Answer 7

increase the concentration of protons, H+

Question 8

bases

Answer 8

increase the concentration of hydroxide ions, OH-

Question 9

strong acids

Answer 9

HCl, HBr, HI, HNO3, HClO4, HClO3, H2SO4

Question 10

ionization of strong acids

Answer 10

comes to completion (single arrow); so you can assume that the concentration of H3O+ ions is equal to the initial concentration of the strong monoprotic acid

Question 11

About protons in aqueous solutions…

Answer 11

at minimun it forms a hydronium cation

Question 12

strong bases

Answer 12

all 1A metals and some 2A metals hydroxides

Question 13

the reaction favors the side with the weaker species

Answer 13

proton transfer equilibrium reactions proceed from the stronger species to the weaker species

Question 14

the weaker the acid or base, the more stable it is

Answer 14

the tendency to form as stable species as possible is the driving force behind many =m reactions (to go from a stronger to a weaker species)

Question 15

having a strong acid (HCl) on the reactant side will make it essentially complete

Answer 15

any reaction involving a strong acid or a strong base (or both) runs to a virtual completion

Question 16

acidic

Answer 16

0-6

Question 17

basic

Answer 17

8-14