Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

General Chemistry > Chem Lesson 4: 14.1 - 14.3 > Flashcards

Chem Lesson 4: 14.1 - 14.3 Flashcards

1
Q

Bronsted Lowry Acid

A

Give up a proton (H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Bronsted Lowry Base

A

Accepts/Receives a proton (H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Conjugate Base

A

The species that remains when an acid donates a H+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Conjugate Acid

A

When a base accepts a proton (H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Acid Ionization

A

Reaction between a Bronsted Lowry acid and water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Base Ionization

A

Reaction between a Bronsted Lowry base and water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Amphiprotic

A

Capable of accepting and donating protons (polyatomic)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Autoionization

A

When two of the same molecules react to yield ions.

Water breaking down into hydronium and hydroxide.

H2O(l) + H2O(l) —> <— H3O+(aq) + OH-(aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Kw (Definition)

A

Ion product constant for water (equlibrium)

Let’s us to see the concentrations of either the [OH-] and/or [H3O+] in water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Kw (temp and value)

A

25c and 1.0*10^-14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Amphoteric Elements (how can you tell by looking at molecule if it can be both and Acid or Base?)

A

H—-^- (Start with H and end with a neg charge)

H2O or NH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Neutral Solution

A

Contains equal concentrations of hydronium (or H+) and hydroxide ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Acidic Solutions

A

Contains higher concentrations of hydronium (or H+) than hydroxide.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Basic Solution

A

Contains higher concentration of hydroxide (OH-) in comparison with hydronium (or H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

PH

A

Measures the concentration of H+ ions in solution in comparison to hydroxide ions. (Tells us how acidic a solution is).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

POH

A

Measures the concentration of hydroxide ions in a solution in comparison to H+. (Tells us how basic a solution is)(OH-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

PH and POH vs [H+] [OH-]

A

-PH and POH tells us how basic/acids a solution is. (The concentrations of each compared to each other)

-[H+] [OH-] tells us how many moles of H+ OH- are in a solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

PH (equation)

A

PH = -log[H+]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

POH (equation)

A

PH = -log[OH-]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Find Molar of H given PH (equation)

A

H = 10^-PH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Find Molar OH given PH (equation)

A

OH = 10^-PH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Sig Fig log rule (PH and OH)

A

Keep as many decimal places are there sig figs in the question when working with log

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

PH < 7

A

More acidic. (More H+ than OH-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

PH > 7

A

More basic. (More OH- than H+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
PH Scale rule/equation (How much more basic is 9 to 7 on the PH scale?)
10^deltaPH 10^9-7 = 10 ^2 = 100 times
26
PH + POH = 14 (can only be used at what temp?)
At 25c
27
Strong Acids (def)
Ionize to a great extent in water to create hydronium. More readily to give up an proton.
28
Strong Acids Mnemonic
So I Brought No Clean Clothes
29
Strong Bases (Period Table) - what do they exclude as well?
Group 1 and group 2 cations, besides the first and last in each group.
30
The stronger the acid or base the x its conjugate partner. (x = weaker or stronger?)
Weaker Ka * Kb = Kw = 1.0*10^-14
31
The weaker the acid or base the x its conjugate partner. (x = weaker or stronger?)
Stronger Ka * Kb = Kw = 1.0*10^-14
32
Percent Ionization Equation
([Ions (H+,OH-,H3O+)] / Original Molecule) * 100
33
Acid Ionization Constant (Ka)
Equilibrium constant for an acid (product/reactant). -Used to determine the strength of a weak acid. (The higher the constant the stronger the acid)
34
Ka (Equation)
Concentration of ions (product)/Concentration of unionized acid
35
Base Ionization Constant (Kb)
Equilibrium constant for a base (product/reactant). -Used to determine the strenght of a base. (Higher the number the stronger the base)
36
Strong Acids and Base (definition)
Acids and bases that ionize completely in water to form electrically charged atoms and molecules.(Nothing left over from the reactant)
37
Neutralization Reaction
When an acid reacts with a base.
38
Relative Trends of Strong Acids/Bases and their Conjugate Bases/Acids
Strong Acid ---> Neutral Conjugate Base Strong Base ---> Neutral Conjugate Acid
39
Leveling Effect (Acid)
Acids stronger than H3O+ can't be used in water or it will interact. (Can't use acids stronger than the conjugate acid of the solvent).
40
Leveling Effect (Base)
Bases stronger than OH- can't be used in water or it will interact. (Can't use Bases stronger than the conjugate base of the solvent).
41
Aqueous solution (means combing with what?)
H2O (water)
42
Atomic Number
Number of protons in the nucleus which determines it's chemical properties
43
Mass Number
Some of number of Protons and Neutrons.
44
Solute
Substance that is dissolved in a solution.
45
Solvent
What the solute is dissolved in to form a solution.
46
Strong Acids/Bases
Breakups (ionizes) completely into it's conjugate base/acid in water. (More product than reactant)
47
Weak Acids/Bases
Only a small amount breakups (ionizes) into it's conjugate base/acid in water. <5% (More reactant than product) (They don't readily want to accept or give up protons).
48
Why do strong acids/bases produce neutral conjugates
The resulting cation and anion are so weak that they don't react in water (readily accept protons).
49
The stronger the base or acid the (x) it's conjugate is?
Weaker
50
Dissociation (Ionic Compound)
When an Ionic Compound breaks apart in a solution (water)
51
Covalent Compound
Compounds that are combined through the sharing of electrons.
52
Ionic Compound
Compounds made from ionic bonds (electron transfer).
53
Bases are x and Acid are x compounds? (Covalent or ionic)
Bases are Ionic and Acids are covalent.
54
Balancing Neutralization Reactions (Tip) Balance what first?
Balance the Base and Acid First.
55
Arrhenius Base
Base that gives off OH- ions (hydroxide).
56
Two Acid types
Oxoacid and Binary
57
Oxoacid
Acid that contains hydrogen, oxygen, and one other element.
58
Oxoacid strength Trends
1. More oxygen more acidic. (Most important). 2. More electronegative the stronger it is. (Bottom left to top right).
59
Oxobase (strength trend)
Opposite of oxoacid
60
Binary Acid
Acid composed of two elements. (Hydrogen and non-metal).
61
Electronegativity (bottom left to top right).
The tendency of an atom to attract electrons towards itself.
62
Binary Acid (Acidity trend)
1. Acid strength increases as you go down a group. (size/atomic radius). Most important factor. 2. Increase when going left to right across a period because of electronegativity. (Use if they're in the same period).
63
Binary Base Trend
1. Basicity Increase as we go up period. (Smaller the atomic radius) 2. Basicity Increase as we go to the left across the period table. (Less electronegativity).
64
Why the more electronegative and acid becomes the stronger it is?
Electronegativity is the tendency for an electron to become more negative and acids do that by giving up H+ ions.
65
Binary Acid Trend Acidity
Across a period and down increases acidity. (So see which non H is the most to the right and down). Because the atomic radius increases and the attraction of the H+ ion to it's nucleus isn't as much so it's more likely to lose it.
66
When PH the solution becomes more..?
Acidic
67
When POH increases the solution becomes more...?
Basic
68
Strong Base PH
> 10
69
Strong Acid PH
1 or less
70
Autoionization of water (endo or exo)
Endothermic
71
How does an increase or decrease in temp affect Autoionization
Increase in heat moves reaction to the right so the concentration of H+ and OH- increases which in turn increases the KW.
72
Affects of Temp on Autoionization of Water
When temp PH decreases but the solution remains neutral.
73
% Ionization Equation for OH or H+
Ionization % = [OH]/[initial solution] %100
74
When to use Ice Tables
When the amount of reactant or product must be determined from the amount of the other reactant or problem.
75
Is PH at equilibrium?
Yes
76
Mass Percent Equation
(Mass of concentration/Mass of solution) * 100

General Chemistry (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions