chem 116 quiz 6

Question 1

Arrhenius definition

Answer 1

acid is a substance that produces H+ ions in aqueous solution

Question 2

Bronsted-Lowry definition

Answer 2

acid is a proton donor and becomes a conjugated base

Question 3

Lew definition

Answer 3

acid is an electron pair acceptor (it has an empty orbit that can accept an electron pair)

Question 4

strong acids

Answer 4

ionize 100%; also strong electrolytes

Question 5

to show the ionization goes to completion, a (single-headed/double-headed) arrow is used b/w the reactants and products

Answer 5

single-headed

Question 6

weak acid

Answer 6

ionizes less than 100%; classified as weak electrolytes

Question 7

double-headed arrow is used to show

Answer 7

a reaction is reversible/some kind of equilibrium is involved

Question 8

the stronger the acid, the (weaker/stronger) the conjugate base

Answer 8

weaker

Question 9

if the forward reaction has a high tendency to occur, then the

Answer 9

reverse reaction has a low tendency to occur

Question 10

? is unique to a particular acid/solvent combination

Answer 10

degree of ionization

Question 11

? is a way to quantify acidity and basicity; ? is defined as ?

Answer 11

pH; pH is defined as -log[H+]

Question 12

pH < 7
pH > 7
pH = 7

Answer 12

acidic
basic
neutral

Question 13

pOH is very similar to the pH scale but is defined as ?; the relationship is ?

Answer 13

pOH = -log[OH-]

pH + pOH = 14

Question 14

from pH, [H+] =

Answer 14

10^(-pH)

Question 15

pKa =

Answer 15

-log(Ka)

Question 16

the pKa of a weak acid is

Answer 16

high

Question 17

the smaller the pKa, the (weaker/stronger) the acid

Answer 17

stronger

Question 18

the smaller the Ka, the (weaker/stronger) the acid

Answer 18

weaker

Question 19

the equilibrium constant for the ionization reaction of a weak acid

Answer 19

Ka

Question 20

the point of exact neutralization can be visually determined through the use of

Answer 20

an indicator

Question 21

an indicator is

Answer 21

a chemical that is sensitive to pH and is one color in a basic solution and another color in an acidic solution

Question 22

the equivalence point allows you to calculate

Answer 22

the unknown concentration of the acid

Question 23

one half the volume at the equivalence point allows you to calculate

Answer 23

the Ka (acid ionization constant)

Question 24

Ka =

Answer 24

10^(-pKa)

Question 25

the equivalence point does not necessarily coincide with

Answer 25

a pH of 7

Question 26

precautions for working with NaOH and unknown acid

Answer 26

splash-proof goggles, long pants, close-toed shoes