Week 4 (Acids, Bases, Salts)

Question 1

Acid

Answer 1

-Arrhenius
-a chemical that, when dissolved in water, will increases the concentration of H+ ions
-changes litmus paper to red
-reacts with carbonates to form CO2
-reacts with active metals to form H2
-pH < 7.00

Question 2

Active metals

Answer 2

very electropositive metals

Question 3

Base

Answer 3

-Arrhenius
-a chemical that, when dissolved in water, will increase the concentration of OH- ions
-causes litmus paper to turn blue
-reacts with many metal ions to form precipitates
-pH > 7.00

Question 4

Neutralization

Answer 4

-an acid reacts with a base to form a salt (ex. HCl + NaOH -> NaCl + H2O)
-cation comes from base, anion comes from acid
-not all salt solutions are neutral

Question 5

Bronsted-Lowry base/acid definition

Answer 5

-Acid: a substance that can donate a proton to another substance (ex. acid donates H+ to water to form H3O)
-Base: a substance that can accept a proton from another substance (ex. bases accept H+ cation from an acid (OH + H = H2O))

Question 6

Lewis base/acid definition

Answer 6

-Acid: electron pair acceptor
-Base: electron pair donor

Question 7

Identifying acids by chemical formulas

Answer 7

-HnA
–(A(-n) is a simple anion (HCl, H2S, HCN, HI) or a polyatomic anion (H2SO4, HNO3, HClO))
-COOH
–(Organic acid (CH3COOH))

Question 8

Identifying bases by chemical formulas

Answer 8

-M(OH)m
–(M(m+) is a metal cation (KOH, Ca(COH)2))
-R3N
–(Ammonia or an organic amine where R can be H or alkyl group (-CH3, -CH2CH3, etc.))

Question 9

How are bases formed?

Answer 9

metal oxides (base anhydrides) dissolve in water to form hydroxides
(ex. Na2O + H2O -> 2 NaOH)

Question 10

How are acids formed?

Answer 10

non-metal oxides (acid anhydrides) dissolve in water to form acids
(ex. SO3 + H2O -> H2SO4)

Question 11

acid anhydrides

Answer 11

non-metal oxides that form acids when they react with water

Question 12

Oxide

Answer 12

a chemical compound containing at least one oxygen atom and one other element in its chemical formula (N2O, CaO, SiO3, etc)

Question 13

base anhydride

Answer 13

metal oxide that forms base when it reacts with water

Question 14

Strong acid

Answer 14

-completely dissociate in water
-strong electrolyte
- HCl, HBr, HI, HClO3, H2SO4, HNO3

Question 15

Weak acid

Answer 15

-only partially dissociate in water
-weak electrolyte
- HClO2, HClO, H2SO3, HNO3
-most organic acids (R-COOH)

Question 16

Strong base

Answer 16

-completely dissociate in water
-group 1/group 2 metal hydroxides (ex. NaOH)

Question 16

Weak base

Answer 16

-only partially disassociate in water (ex. NH3)

Question 17

pH scale

Answer 17

-ionization of water is point of reference to tell us if something is an acid or base

Question 18

Neutral solution H+ to OH- ratio

Answer 18

[H+]=[OH-]

Question 19

Acidic solution H+ to OH- ratio

Answer 19

[H+]>[OH-]

Question 20

Basic solution H+ to OH- ratio

Answer 20

[H+]<[OH-]

Question 21

p-scale

Answer 21

-calculates number that describes acid/base
-pX = -log[X]
-For acids/bases: pH = -log[H+]
(ex. if [H+] = 0.012 M, then pH = -log(1.2x10-2) = 1.92)
(ex. if [H+] = 1.2x10-11 M, then pH = -log(1.2x10-11) = 10.92)

Question 22

Neutral solution pH

Answer 22

-Water at 25C, [H+][OH-]= 1x10-14
-[H+] = 1x10-7 M
-[OH-] = 1x10-7 M
-pH = 7.00

Question 23

Neutral salt solution

Answer 23

made from reaction of strong base and strong acid (ex. KNO3, KOH is strong base, HNO3 is strong acid)

Question 24

Basic salt solution

Answer 24

made from reaction of a strong base and a weak acid (ex. Na2S, NaOH is strong base, H2S is weak acid)

Question 25

Acidic salt solution

Answer 25

made from reaction of a weak base and a strong acid (ex. NH4Br, NH3 is weak base, HBr is strong acid)

Question 26

Litmus test

Answer 26

-test for acidity or alkalinity using litmus (dye)
-base turns paper blue
-acid turns paper red
-gives qualitative value (yes/no)

Question 27

Acid-base indicator

Answer 27

-substance that changes color to indicate whether a solution is acidic or basic
-color changes over specific pH ranges
-stable in solution of lower pH: HIn + H2O
-stable in solution of higher pH: H3O+ + In-

Question 28

monoprotic acid

Answer 28

acid that has one proton to donate (ex. HCl)
(HCl + H2O -> H3O+ + Cl-)

Question 29

polyprotic acid

Answer 29

acid that has multiple protons to donate (ex. H2SO4)
(H2SO4 + 2H2O -> 2H3O+ + SO4(2-))

Question 30

The 7 Strong Acids

Answer 30

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