exam three

Question 1

what is an acid?

Answer 1

proton/H+ donor

Question 2

what is a base?

Answer 2

proton/H+ accepter

Question 3

what defines a strong acid?

Answer 3

completely ionizes in water

Question 4

what defines a weak acid?

Answer 4

partially ionizes in water

Question 5

five weak acids:

Answer 5

CH3COOH
HCOOH
HF
HClO
HNO2

Question 6

how is a conjugate base created?

Answer 6

negative charge due to acid donating H+

Question 7

how is a conjugate acid created?

Answer 7

positive charge due to accepting the H+

Question 8

four strong acids:

Answer 8

HCl
HClO4
HNO3
H2SO4

Question 9

how can you tell something is a weak base?

Answer 9

metal hydroxide (OH group)

Question 10

how can you tell something is a strong base?

Answer 10

amine group

Question 11

what is the strongest acid that can exist in an aqueous solution?

Answer 11

H3O+

Question 12

how is Kw calculated?

Answer 12

Kw=[H3O+][OH-]=1x10^-14

Question 13

how is pH calculated?

Answer 13

pH=-log[H3O+]

Question 14

how is pOH calculated?

Answer 14

pOH=-log[OH-]

Question 15

what is the sum of pH and pOH?

Answer 15

14

Question 16

how can you calculate [H3O+] by only knowing pH?

Answer 16

10^-pH

Question 17

if pH value is greater than the pOH value, what is true about the solution?

Answer 17

basic

Question 18

if pH value is less than pOH, what is true about the solution?

Answer 18

acidic

Question 19

what does a low ionization constant mean?

Answer 19

negligible/won’t change or ionize a significant amount

Question 20

hydrolysis of salts reaction:

Answer 20

acid + base –> salt + water

Question 21

what does amphoteric mean?

Answer 21

can act as an acid or a base

Question 22

what is a buffer?

Answer 22

solution that will resist changes in pH

Question 23

what is common ion effect?

Answer 23

shift in equilibrium caused by addition of a compound having an ion in common with the dissolved substance

Question 24

Henderson hasselbach equation:

Answer 24

pH=pKa +log ([base]/[acid])

Question 25

what is the equivalence point in titrations?

Answer 25

point at which the reaction is complete

Question 26

what is an indicator?

Answer 26

substance that changes color at or near the equivalence point

Question 27

if you are titrating a strong acid and a strong base, what is the equivalence point?

Answer 27

~7

Question 28

what is Ksp?

Answer 28

solubility product constant

Question 29

what is solubility?

Answer 29

amount of solute that dissolves (g/L)

Question 30

what is molar solubility?

Answer 30

moles of solute dissolved in 1L of a saturated solution (moles/L)

Question 31

what does a high Ka value indicate?

Answer 31

strong acid

Question 32

if a Ka value is given to us, what can be assumed about the solution?

Answer 32

it is a weak acid

Question 33

what can be said about the conjugate base of a weak acid?

Answer 33

weak base

Question 34

what i