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AP Chemistry > Textbook Ch.4: Reactions in Aqueous Solution > Flashcards

Textbook Ch.4: Reactions in Aqueous Solution Flashcards

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1
Q

Molarity

A

the concentration of a solute in solution

molarity (M) = moles of solute / liters of solution

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2
Q

What does the symbol [ ] represent?

A

the molarity of a species in solution

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3
Q

What can the molarity of a solution be used to calculate?

A
  • The number of moles of solute in a given volume of solution
  • The volume of solution containing a given number of moles of solute
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4
Q

Precipitate

A

formed when two different ionic compounds are mixed, an insoluble solid separates out of a solution

  • The precipitate that forms is itself ionic
  • The cation comes from one solution, the anion comes from the other
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5
Q

Net ionic equation

A

the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction.

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6
Q

What does a net ionic equation have to show?

A
  • Atom balance (same number of atoms of each element on both sides)
  • Charge balance (must be the same total charge on both sides)
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7
Q

Acid

A

a species that produces H⁺ ions in water solution

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8
Q

Base

A

a species that produces OH⁻ ions in a water solution

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9
Q

Strong acids

A

acids that ionize completely, forming H⁺ ions and anions

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10
Q

Weak acids

A

acids that only partially ionize to H⁺ ions in water

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11
Q

What does a double arrow ⇌ symbol mean?

A

the reaction does not go into completion, instead a mixture is formed containing significant amounts of both products and
reactants

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12
Q

Strong bases

A

bases that completely ionize into OH⁻ ions and cations

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13
Q

Weak bases

A

produce OH⁻ ions by reacting with water molecules, acquiring H⁺ ions and leaving OH⁻ ions behind

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14
Q

Strong acid-strong base reactions

A

acids and bases both completely and the H⁺ and OH⁻ ions react with each other to form H₂O molecules, this reaction is referred to as neutralization

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15
Q

What is the net ionic equation for a strong acid-strong base reaction?

A

H⁺(aq) + OH⁻(aq) —> H₂O

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16
Q

Weak acid-strong base reactions

A

a two-step reaction occurs

  1. Ionization of the weak acid into H+ and an anion
  2. Neutralization of the H+ ions produced from (1) react with the OH- of the base to produce water
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17
Q

What is the net ionic equation for a weak acid-strong base reaction?

A

HB(aq) + OH⁻(aq) —> H₂O + B⁻(aq)

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18
Q

Strong acid-weak base reactions

A

two-step reaction occurs

  1. Acid reacts with water to form cations and OH⁻
  2. Neutralization occurs when ions produced from (1) react with the OH⁻ of the base to produce water
19
Q

What is the net ionic reaction for a strong-acid weak base reaction?

A

H⁺(aq) + B(aq) —> BH⁺(aq)

20
Q

Titration

A

when acid-base reactions in water solution are commonly used to determine the concentration of a dissolved species or its
percentage in a solid measure, so the volume of a standard solution (a solution of known concentration) required to react with a measured amount of sample is measured

21
Q

Redox reaction

A

a reaction in an aqueous solution that involves a transfer of electrons between two species

22
Q

Which species in a redox reaction is considered to be oxidized?

A

the species that loses (i.e. donates) electrons

23
Q

Which species in a redox reaction is considered to be reduced?

A

the species that gains (i.e. received) electrons

24
Q

How are redox reactions split?

A

it can be split into two half-equations, one of oxidation and the other of reduction

25
Q

What is unique to redox reactions?

A
  • Oxidation and reduction occur together in the same reaction; you can’t have one without the other
  • there is no net charge in the number of electrons in a redox reaction. Those given off in the oxidation half-reaction are taken
    on by another species in the reduction half-reaction
26
Q

Oxidizing agent

A

the ion or molecule that accepts electrons

27
Q

Reducing agent

A

the ion or molecule that donates electrons

28
Q

Oxidation number

A

a concept that is used to simplify the electron bookkeeping in redox reactions

29
Q

The oxidation number of an element in an elementary substance is:
(I.e. Cl₂, P₄)

A

0

30
Q

The oxidation number of an element in a monatomic ion is:

A

equal to the charge of the ion

Ex: in NaCl, sodium has an oxidation number of +1 (because it has a charge of +1) and chlorine has an oxidation number of -1
(because it has a charge of -1)

31
Q

Group 1 elements always have an oxidation number of ____ in their compounds

A

they always have an oxidation number of +1 because they always exist as +1 ions in their compounds

32
Q

Group 2 elements always have an oxidation number of ____ in their compounds

A

they always have an oxidation number of +2 because they always exist as +2 ions in their compounds

33
Q

Oxygen is ordinarily assigned an oxidation number of ____ in its compounds

A

-2 (except for peroxide, where the oxidation number of oxygen is -1)

34
Q

The sum of the oxidation numbers in a neutral species is:

A

0

35
Q

The sum of oxidation numbers in a polyatomic ion is:

A

equal to the charge of that ion

36
Q

Define oxidation in terms of increasing/decreasing oxidation number

A

oxidation is defined as an increase in oxidation number

37
Q

Define reduction in terms of increasing/decreasing oxidation number

A

reduction is defined as a decrease in oxidation number

38
Q

Half-equation

A

two equations that come from a redox reaction: one for oxidation (electron loss) and one for reduction (electron gain

39
Q

When balancing half-reactions, what aspects need to be balanced and in what order should you balance them?

A
  1. Number of atoms of the element being oxidized or reduced
  2. Oxidation number
  3. Charge
  4. Hydrogen
  5. Oxygen
40
Q

When you are balancing the oxidation number in reduction half-equations, which side do you add electrons onto?

A

left

41
Q

When you are balancing the oxidation number in oxidation half-equations, which side do you add electrons onto?

A

right

42
Q

When balancing the charge of a half-equation in an acidic solution, what do you add?

A

H⁺ ions

43
Q

When balancing the charge of a half-equation in a basic solution, what do you add?

A

OH⁻ ions

44
Q

In order to put the two half-equations together to balance the entire redox reaction, what should you make sure cancels?

A

the electrons

AP Chemistry (11 decks)

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