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Chemistry 12 > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

What is the name of the theory that says acids release H= ions and bases release OH- ions, and the cation from the base and anion from the acid make a salt?

A

Arrhenius theory

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2
Q

What does the Bronsted-Lowry theory say about acids?

A

An acid donates an H+ ion

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3
Q

What does the Bronsted-Lowry theory say about bases?

A

A base accepts an H+ ion.

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4
Q

In a Bronsted-Lowry equilibrium, acids and bases can be found on which sides of the formula?

A

Both

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5
Q

What do you call the H3O+ ion?

A

Hydronium

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6
Q

What is a conjugate acid/base pair?

A

Two substances on opposite sides of the formula that differ by an H+ ion.

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7
Q

What do you call a chemical species that can act as both an acid and a base?

A

Amphiprotic

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8
Q

Are uncharged substances usually amphiprotic?

A

No.

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9
Q

What charge are amphiprotic species usually?

A

negative

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10
Q

Does the strength of an acid or base depend on concentration?

A

No.

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11
Q

What is the strength of an acid/base?

A

The ability to produce ions in solution (dissociate)

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12
Q

What do you call an acid that completely ionizes in solution?

A

Strong acid.

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13
Q

What do you call an acid that only partially ionizes in solution?

A

Weak acid.

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14
Q

Is an equilibrium an indicator of a strong or weak acid/base?

A

WEAK

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15
Q

What do you call a base that completely dissociates in solution?

A

Strong base

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16
Q

What do you call a base that partially dissociates in solution?

A

Weak base.

17
Q

What does the acid/base ionization constant not include?

A

Water

18
Q

What is the acid ionization constant equation? (Ka)

A

Ka = [product] [H3O] / [reactant]

19
Q

What is the base ionization constant equation? (Kb)

A

Kb = [product] [OH-] / [reactant]

20
Q

If Keq > 1 then the reaction favours the

A

reactants

21
Q

If Keq < 1 then the reaction favours the

A

products

22
Q

What levels the strength of strong acid/bases?

A

Water

23
Q

What do you call it when two water molecules automatically exchange an H+ ion between them?

A

The autoionization of water

24
Q

What is the ionization constant for water? (Kw)

A

Kw = [H3O+] [OH-] = 1.00x10^-14 = 25 degrees

25
Q

What happens when you add strong acids and bases to each other?

A

They neutralize each other

26
Q

What do you get when you multiply Kb and Ka?

A

Kw

27
Q

How to find the Kb value?

A

divide Kw (10^-14) by the Ka of the conjugate acid

28
Q

What is the equation to determine pH?

A

pH= -log [H3O+]

29
Q

What is the pH of acidic solutions?

A

less than 7

30
Q

What is the pH of basic solutions?

A

more than 7

31
Q

Every unit decrease in pH represents a decrease in how much [H3O+]?

A

a factor of 10

32
Q

What is the equation to calculate [H3O+] from pH?

A

[H3O+] = 10^-pH

33
Q

what does the lowercase “p” represent?

A

-log10 (10 is subscript)

34
Q

What do you get when you add pH and pOH?

A

pH + pOH = pKw

35
Q

For metal oxides we do not include what in our ionization equation?

A

Equilibrium arrows

36
Q

What are the steps for calculating whether a solution is acidic or basic when a strong acid is mixed with a strong base?

A

1: net reaction equation (neutralization)
2: calculate # of mol present before and after reaction
3: From excess reactant, calculate pH

37
Q

How do you determine the pH of weak acids?

A

Use the Ka expression, as well as an ice table.

38
Q

How do you determine the pH of weak bases?

A

Use an ice table and Kb expression

39
Q

How do you calculate the [weak base] necessary to produce a certain pH?

A

1: equilibrium equation + ice table
2: calculate [OH-]
3: compute Kb
4: solve

Chemistry 12 (8 decks)

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