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Chemistry 30 > Unit 7 > Flashcards

Unit 7 Flashcards

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1
Q

What are binary acids? How are they named?

A

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

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2
Q

What are oxyacids? How are they named?

A

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

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3
Q

For the oxyacids, which prefixes and suffixes mean what?

A

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

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4
Q

How does polyatomic ion ending relate to the acid naming?

A

Poly Acid
Ate ic
Ite ous

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5
Q

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

A

A base increases the [OH-]

An acid increases the [H+]

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6
Q

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

A

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

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

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7
Q

What is the difference between an acid and a base?

A

Acids dissociate into hydronium (H3O+) and an element

Bases dissociate into hydroxide (OH-) and an element

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8
Q

What are the strong acids?

A 
HCl
HBr
HI
HClO4
HClO3
H2SO4
HNO3
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9
Q

What are the strong bases?

A 
LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
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10
Q

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

A

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

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11
Q

What are neutral compounds?

A

Compounds that do not produce H+ or OH-

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12
Q

What is a Brønsted-Lowry acid?

A

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

Base is a proton acceptor

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13
Q

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

A

Proton donor- HCl

Proton acceptor- NH3

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14
Q

What is a monoprotic, diprotic, and tripotic acid?

A

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

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15
Q

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

A 
Monoprotic= lowest conc. and weakest acid
Diprotic= higher conc. and middle weak acid
Triprotic= greatest conc. and least weak acid
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16
Q

According to Gilbert Lewis, what is a Lewis acid?

A

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)

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17
Q

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

A 
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
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18
Q

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

A

Weaker

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19
Q

What does amphoteric mean?

A

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

20
Q

What does amphiprotic mean?

A

Means that it can donate or accept H+

All Amphiprotic substances are amphoteric (not vice versa tho)

21
Q

What is neutralization? What is the general neutralization equation?

A

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

Acid + metal -> salt + hydrogen

22
Q

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

A

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

23
Q

Can water ionize on its own? Wrote the equation

A

Yes it can

H2O + H2O -> H3O + OH

24
Q

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

A

Both are 1.0 x 10^-7

25
Q

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

A

Decreases

26
Q

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

A

Kw=ionization constant

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

27
Q

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

A

Potential power of hydrogen

P means -log10

28
Q

What does pH equal?

A

-log [H3O+]

29
Q

What does pOH equal?

A

-log [OH-]

30
Q

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

A

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

31
Q

How do significant figures work with pH?

A

It goes by the number of digits after the decimal

  1. 27 2 sig figs
  2. 00045 5 sig figs
32
Q

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

A

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

33
Q

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

A

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

34
Q

What is titration?

A

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

35
Q

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

A

n= CV

C=n/V

36
Q

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

A

Litres

37
Q

What is the acid ionization constant? Equation?

A 
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
38
Q

The larger the Ka, the ________ the acid.

A

Stronger

39
Q

What is pKa?

A

pKa=-log[Ka]

Lower the pKa, stronger the acid

40
Q

What is Kb?

A

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

41
Q

The larger the Kb, the _________ the base.

A

Stronger

42
Q

What is pKb?

A

pKb= -log[Kb]

Lower the pKb, stronger the base

43
Q

What is Ka x Kb equal?

A

Kw

44
Q

What reactions are Ka and Kb each used for?

A

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

45
Q

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

A

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

46
Q

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

A

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

Chemistry 30 (8 decks)

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