Unit 7

Question 1

What are binary acids? How are they named?

Answer 1

Contain hydrogen and one of the more electronegative elements
Hydro-element-ic acid
Ex: Hydrofluoric acid HF

Question 2

What are oxyacids? How are they named?

Answer 2

Contain hydrogen, oxygen, and a third element (usually a nonmetal)
Based off polyatomic ions
Polyatomic ion-ic acid

Question 3

For the oxyacids, which prefixes and suffixes mean what?

Answer 3

Hypo____ous means 2 less oxygen
______ous means 1 less oxygen
______ic means most common form or first discovered
Per______ic means one more oxygen

Question 4

How does polyatomic ion ending relate to the acid naming?

Answer 4

Poly Acid
Ate ic
Ite ous

Question 5

According to Arrhenius, what do a base and an acid increase?

Answer 5

A base increases the [OH-]

An acid increases the [H+]

Question 6

What is a strong acid/base and a weak acid/base

Answer 6

Strong acids and bases ionize/dissociate completely and are strong electrolytes

Weak acids and bases only ionize/dissociate partially and are weak electrolytes

Question 7

What is the difference between an acid and a base?

Answer 7

Acids dissociate into hydronium (H3O+) and an element

Bases dissociate into hydroxide (OH-) and an element

Question 8

What are the strong acids?

Answer 8

HCl
HBr
HI
HClO4
HClO3
H2SO4
HNO3

Question 9

What are the strong bases?

Answer 9

LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2

Question 10

Does the solubility of a compound affect the strength of acids and particular bases?

Answer 10

Yes, if metal hydroxide is insoluble they won’t produce OH-

Question 11

What are neutral compounds?

Answer 11

Compounds that do not produce H+ or OH-

Question 12

What is a Brønsted-Lowry acid?

Answer 12

A molecule or ion that is a proton donor (H+ is a proton)

Base is a proton acceptor

Question 13

In the compound
HCl+NH3 –> NH4 + Cl
Which is the proton donor?
Which is the proton acceptor?

Answer 13

Proton donor- HCl

Proton acceptor- NH3

Question 14

What is a monoprotic, diprotic, and tripotic acid?

Answer 14

Monoprotic- can donate 1 proton/molecule- HCl
Diprotic- can donate 2- H2SO4
Triprotic- can donate 3- H3PO4

Question 15

How do monoprotic, diprotic, and triprotic acids affect concentration and how weak the acid is?

Answer 15

Monoprotic= lowest conc. and weakest acid
Diprotic= higher conc. and middle weak acid
Triprotic= greatest conc. and least weak acid

Question 16

According to Gilbert Lewis, what is a Lewis acid?

Answer 16

An atom, molecule, or ion that accepts an electron pair to form a covalent bond
There is an electron pair acceptor (acid) and an electron pair donor (base)

Question 17

What is a conjugate base and a conjugate acid?
Name the base, acid, conjugate base, and conjugate acid for this reaction
NH3 + H2O -> NH4 + OH

Answer 17

When an acids donates a proton(H+), it creates a conjugate base, this is what's left over after losing a proton
NH3- base
H2O- acid
NH4- conjugate acid
OH- conjugate base

Question 18

The stronger the acid or base, the _________ the conjugate acid or base will be

Answer 18

Weaker

Question 19

What does amphoteric mean?

Answer 19

This is what water is called when it can act as either an acid or a base

Question 20

What does amphiprotic mean?

Answer 20

Means that it can donate or accept H+

All Amphiprotic substances are amphoteric (not vice versa tho)

Question 21

What is neutralization? What is the general neutralization equation?

Answer 21

It involves the reaction of hydronium and hydroxide ions to form water and a salted

Acid + metal -> salt + hydrogen

Question 22

When writing a neutralization equation what must be done in the overall ionic equation?

Answer 22

Use hydronium (H3O+) instead of H and double water

Question 23

Can water ionize on its own? Wrote the equation

Answer 23

Yes it can

H2O + H2O -> H3O + OH

Question 24

What are the concentrations of [H3O+] and [OH-] at room temp?

Answer 24

Both are 1.0 x 10^-7

Question 25

As [H30+] concentration increases, the concentration of [OH-] ___________.

Answer 25

Decreases

Question 26

What is the ionization constant of water? What's the equation?

Answer 26

Kw=ionization constant | Kw= [H3O+][OH-] = 1.0x10^-14 M^2 (at 25C)

Question 27

What does pH stand for? Mathematically what does p mean?

Answer 27

Potential power of hydrogen | P means -log10

Question 28

What does pH equal?

Answer 28

-log [H3O+]

Question 29

What does pOH equal?

Answer 29

-log [OH-]

Question 30

What is pH below 7, at 7, and above 7 mean?

Answer 30

Below 7- acidic At 7- neutral Above 7- basic

Question 31

How do significant figures work with pH?

Answer 31

It goes by the number of digits after the decimal 0. 27 2 sig figs 0. 00045 5 sig figs

Question 32

How do you find the [H3O+] given the pOH of something?

Answer 32

Find the pH Use the equation [H3O+] = antilog (-pH)

Question 33

How do you find the [OH-] given the pH of something?

Answer 33

Find the pOH (pOH+pH=14) Use this equation [OH-]= antilog (-pOH)

Question 34

What is titration?

Answer 34

Titration is the process of mixing an acid with a base to find the equivalence point (when the concentration of [H3O+] = [OH-] If you know the concentration and volume of one reactant, you can determine the concentration of the other knowing the volume required to neutralize it

Question 35

What is the formula used for finding the number of mols given the concentration and volume?

Answer 35

n= CV | C=n/V

Question 36

What is the volume always to be put in for titration? (Stoich)

Answer 36

Litres

Question 37

What is the acid ionization constant? Equation?

Answer 37

``` Ka, it is the equilibrium constant for an acid as it ionizes in water Ka=products/reactants Ex: CH3COOH + H2O -> H3O + CH3COO Ka= [H3O+][CH3COO-] / [CH3COOH] Liquids solids do not count ```

Question 38

The larger the Ka, the ________ the acid.

Answer 38

Stronger

Question 39

What is pKa?

Answer 39

pKa=-log[Ka] | Lower the pKa, stronger the acid

Question 40

What is Kb?

Answer 40

Kb is the equilibrium constant for a base as it reacts with water. Same equation as Ka Kb= products/reactants not including liquid or solid

Question 41

The larger the Kb, the _________ the base.

Answer 41

Stronger

Question 42

What is pKb?

Answer 42

pKb= -log[Kb] | Lower the pKb, stronger the base

Question 43

What is Ka x Kb equal?

Answer 43

Kw

Question 44

What reactions are Ka and Kb each used for?

Answer 44

Ka is used for reactions with H3O+ Acid ionization Kb is used for reactions with OH- Base reacting with water

Question 45

What are Arrhenius, Brønsted-Lowry, and Lewis acids?

Answer 45

Arrhenius- H+ (H3O+) producer Brønsted-Lowry- H+ (proton) donor Lewis- e- pair acceptor

Question 46

What are Arrhenius, Brønsted-Lowry, and Lewis bases?

Answer 46

Arrhenius- OH- producer Brønsted-Lowry- H+ (proton) acceptor Lewis- e- pair donor