Chemistry- Acids and Bases

Question 1

properties of acids

Answer 1

• form electrolytic aqueous solutions
• taste sour
• corrosive to metals
• turn litmus red

Question 2

properties of bases

Answer 2

• form electrolytic aqueous solutions
• taste bitter
• slippery
• turn litmus blue

Question 3

acids

Answer 3

release H+ ions into solution

Question 4

bases

Answer 4

release OH- ions into solution

Question 5

anions ending in “-ide”

Answer 5

• replace the “ide” ending with “-ic”

- use the prefix “hyrdo-“

Question 6

anions ending in “-ate”

Answer 6

• replace the “-ate” ending with “-ic”
• no prefix
• i ATE something ICKY at the cafeteria

Question 7

anions ending in “-ite”

Answer 7

• replace the “-ite” ending with “-ous”
• no prefix
• you’ll be AIGHT with US

Question 8

Arrhenius acid

Answer 8

a substance that releases H+ ions in an aqueous solution

Question 9

Arrhenius base

Answer 9

a substance that releases OH= ions in an aqueous solution

Question 10

Bronsted-Lowry acid

Answer 10

• an species that can donate a proton (H+ ion)

- proton donor

Question 11

Bronsted-Lowry base

Answer 11

• an species that accepts a proton

- proton acceptor

Question 12

Lewis acid

Answer 12

electron pair acceptor

Question 13

Lewis base

Answer 13

electron pair donor

Question 14

amphoteric substances

Answer 14

• can behave as a Bronsted-Lowry acid or base
• must be able to donate and accept a proton
• example is water

Question 15

strong acid

Answer 15

• dissociates completely

- forward reaction only

Question 16

weak acid

Answer 16

• dissociates partially
• double arrows
• exists at equilibrium

Question 17

strong base

Answer 17

tend to be ionic compounds containing OH- and a metal cation

Question 18

weak base

Answer 18

tend to be Bronsted bases that produce OH by reacting with water

Question 19

the 7 strong acids

Answer 19

• HCl
• HBr
• H2SO4
• HNO3
• HI
• HClO3
• HClO4

Question 20

the 7 strong bases

Answer 20

• KOH
• NAOH
• Ca(OH)2
• RbOh
• CsOH
• Sr(OH)2
• Ba(OH)2

Question 21

self ionization of water

Answer 21

• two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
• H2O + H2O –> H3O+ + OH-

Question 22

at 25 C, [H3O+] = [OH-] =

Answer 22

1.0 x 10^-7

Question 23

in an acidic solution

Answer 23

• [H+] > [OH-]

- ph

Question 24

in a basic solution

Answer 24

• [H+] 7

Question 25

in a neutral solution

Answer 25

- [H+] = [OH-] | - ph = 7

Question 26

pH

Answer 26

- translates to hydrogen power - H+ concentration is generally large - negative of the common logarithm off the hydronium concentration

Question 27

pH formula

Answer 27

pH = -log[H3O+]

Question 28

pOH

Answer 28

negative of the common logarithm of the hydroxide ion concentration

Question 29

pOH formula

Answer 29

- pOH = -log[OH-] | - THEN subtract from 14

Question 30

for dilute solutions of acids and bases

Answer 30

- the ions from water must be taken into account - add H+ or OH- from water - when exponents are -7, -8, -9

Question 31

conjugate base

Answer 31

- species that remains after a Bronsted-Lowry acid has GIVEN UP A PROTON - the stronger the acid, the weaker the conjugate base

Question 32

conjugate acid

Answer 32

species that is FORMED when a Bronsted-Lowry base GAINS a proton

Question 33

neutralization equation

Answer 33

Acid + Base --> Salt + H2O

Question 34

neutralization

Answer 34

- reaction of hydronium ions and hydroxide ions to form water molecules - also produces salt - double replacement reaction

Question 35

salt

Answer 35

- ionic compound composed of a cation from a base and an anion from an acid - identity depends on acid and base used - generally soluble

Question 36

acid base indicators

Answer 36

- compounds whose colors are sensitive to pH - color changes as pH changes - determines when the equivalence point is reached

Question 37

transition interval

Answer 37

pH range over which an indicator changes color

Question 38

titration

Answer 38

determines concentration of unknown through neutralization

Question 39

burette

Answer 39

- used for titration | - deliver very precise volumes of solution

Question 40

equivalence point

Answer 40

when [H+] = [OH-] in a titration

Question 41

endpoint

Answer 41

point in a titration at which an indicator changes color

Question 42

strong acid and strong base

Answer 42

- produces neutral salt (= 7) | - indicators: bromthymol blue or litmus

Question 43

strong acid and weak base

Answer 43

- produces acidic salt (

Question 44

weak acid and strong base

Answer 44

- produces basic salt (> 7) | - indicators: phenolphthalein, thymol blue

Question 45

weak acid and weak base

Answer 45

- never titrated | - pH doesn't change dramatically as the equivalence point is approached