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

Chem Lesson 4: 14.1 - 14.3 Flashcards

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1
Q

Bronsted Lowry Acid

A

Give up a proton (H+)

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2
Q

Bronsted Lowry Base

A

Accepts/Receives a proton (H+)

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3
Q

Conjugate Base

A

The species that remains when an acid donates a H+

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4
Q

Conjugate Acid

A

When a base accepts a proton (H+)

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5
Q

Acid Ionization

A

Reaction between a Bronsted Lowry acid and water

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6
Q

Base Ionization

A

Reaction between a Bronsted Lowry base and water

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7
Q

Amphiprotic

A

Capable of accepting and donating protons (polyatomic)

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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)

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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.

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10
Q

Kw (temp and value)

A

25c and 1.0*10^-14

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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

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12
Q

Neutral Solution

A

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

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13
Q

Acidic Solutions

A

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

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14
Q

Basic Solution

A

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

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15
Q

PH

A

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

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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-)

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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.

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18
Q

PH (equation)

A

PH = -log[H+]

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19
Q

POH (equation)

A

PH = -log[OH-]

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20
Q

Find Molar of H given PH (equation)

A

H = 10^-PH

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21
Q

Find Molar OH given PH (equation)

A

OH = 10^-PH

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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

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23
Q

PH < 7

A

More acidic. (More H+ than OH-)

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24
Q

PH > 7

A

More basic. (More OH- than H+)

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25
Q

PH Scale rule/equation (How much more basic is 9 to 7 on the PH scale?)

A

10^deltaPH

10^9-7 = 10 ^2 = 100 times

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26
Q

PH + POH = 14 (can only be used at what temp?)

A

At 25c

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27
Q

Strong Acids (def)

A

Ionize to a great extent in water to create hydronium. More readily to give up an proton.

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28
Q

Strong Acids Mnemonic

A

So I Brought No Clean Clothes

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29
Q

Strong Bases (Period Table) - what do they exclude as well?

A

Group 1 and group 2 cations, besides the first and last in each group.

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30
Q

The stronger the acid or base the x its conjugate partner. (x = weaker or stronger?)

A

Weaker

Ka * Kb = Kw = 1.0*10^-14

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31
Q

The weaker the acid or base the x its conjugate partner. (x = weaker or stronger?)

A

Stronger

Ka * Kb = Kw = 1.0*10^-14

32
Q

Percent Ionization Equation

A

([Ions (H+,OH-,H3O+)] / Original Molecule) * 100

33
Q

Acid Ionization Constant (Ka)

A

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
Q

Ka (Equation)

A

Concentration of ions (product)/Concentration of unionized acid

35
Q

Base Ionization Constant (Kb)

A

Equilibrium constant for a base (product/reactant).

-Used to determine the strenght of a base. (Higher the number the stronger the base)

36
Q

Strong Acids and Base (definition)

A

Acids and bases that ionize completely in water to form electrically charged atoms and molecules.(Nothing left over from the reactant)

37
Q

Neutralization Reaction

A

When an acid reacts with a base.

38
Q

Relative Trends of Strong Acids/Bases and their Conjugate Bases/Acids

A

Strong Acid —> Neutral
Conjugate Base

Strong Base —> Neutral Conjugate Acid

39
Q

Leveling Effect (Acid)

A

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
Q

Leveling Effect (Base)

A

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
Q

Aqueous solution (means combing with what?)

A

H2O (water)

42
Q

Atomic Number

A

Number of protons in the nucleus which determines it’s chemical properties

43
Q

Mass Number

A

Some of number of Protons and Neutrons.

44
Q

Solute

A

Substance that is dissolved in a solution.

45
Q

Solvent

A

What the solute is dissolved in to form a solution.

46
Q

Strong Acids/Bases

A

Breakups (ionizes) completely into it’s conjugate base/acid in water.

(More product than reactant)

47
Q

Weak Acids/Bases

A

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
Q

Why do strong acids/bases produce neutral conjugates

A

The resulting cation and anion are so weak that they don’t react in water (readily accept protons).

49
Q

The stronger the base or acid the (x) it’s conjugate is?

A

Weaker

50
Q

Dissociation (Ionic Compound)

A

When an Ionic Compound breaks apart in a solution (water)

51
Q

Covalent Compound

A

Compounds that are combined through the sharing of electrons.

52
Q

Ionic Compound

A

Compounds made from ionic bonds (electron transfer).

53
Q

Bases are x and Acid are x compounds?

(Covalent or ionic)

A

Bases are Ionic and Acids are covalent.

54
Q

Balancing Neutralization Reactions (Tip) Balance what first?

A

Balance the Base and Acid First.

55
Q

Arrhenius Base

A

Base that gives off OH- ions (hydroxide).

56
Q

Two Acid types

A

Oxoacid and Binary

57
Q

Oxoacid

A

Acid that contains hydrogen, oxygen, and one other element.

58
Q

Oxoacid strength Trends

A
  1. More oxygen more acidic. (Most important).
  2. More electronegative the stronger it is. (Bottom left to top right).
59
Q

Oxobase (strength trend)

A

Opposite of oxoacid

60
Q

Binary Acid

A

Acid composed of two elements.

(Hydrogen and non-metal).

61
Q

Electronegativity (bottom left to top right).

A

The tendency of an atom to attract electrons towards itself.

62
Q

Binary Acid (Acidity trend)

A
  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
Q

Binary Base Trend

A
  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
Q

Why the more electronegative and acid becomes the stronger it is?

A

Electronegativity is the tendency for an electron to become more negative and acids do that by giving up H+ ions.

65
Q

Binary Acid Trend Acidity

A

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
Q

When PH the solution becomes more..?

A

Acidic

67
Q

When POH increases the solution becomes more…?

A

Basic

68
Q

Strong Base PH

A

> 10

69
Q

Strong Acid PH

A

1 or less

70
Q

Autoionization of water (endo or exo)

A

Endothermic

71
Q

How does an increase or decrease in temp affect Autoionization

A

Increase in heat moves reaction to the right so the concentration of H+ and OH- increases which in turn increases the KW.

72
Q

Affects of Temp on Autoionization of Water

A

When temp PH decreases but the solution remains neutral.

73
Q

% Ionization Equation for OH or H+

A

Ionization % = [OH]/[initial solution] %100

74
Q

When to use Ice Tables

A

When the amount of reactant or product must be determined from the amount of the other reactant or problem.

75
Q

Is PH at equilibrium?

A

Yes

76
Q

Mass Percent Equation

A

(Mass of concentration/Mass of solution) * 100

General Chemistry (15 decks)

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