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Chemistry > Chapter 4: Types of Chemical Reactions and Solution Stoichiometry > Flashcards

Chapter 4: Types of Chemical Reactions and Solution Stoichiometry Flashcards

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1
Q

Polar molecule

A

Contains an unequal
distribution of charge

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2
Q

define

Hydration

A
  • Process by which the positive side of H2O molecules is attracted to negative ions. And the negative side of water molecules is attracted to positive ions
  • Causes salt to split when dissolved in water (When ionic salts dissolve in water, they break into individual cations and anions)
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3
Q

What does the solubility of ionic substances in water varies depending on

A
  • The attraction between ions of opposite charges
  • The attraction of ions for water molecules
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4
Q

Which substances are expected to be more soluble in water

Polar and ionic substances OR nonpolar

A

Polar and ionic substances

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5
Q

Solute vs. solvant

A
  • Solute : Substance being dissolved
  • Solvent : The dissolving medium
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6
Q

define

Electrolyte

A

Substance that dissolves in water to produce a solution that can conduct electricity

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7
Q

Strong electrolytes are…

A

Highly efficient conductors of current in aqueous solutions
fully ionize in water

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8
Q

Weak electrolytes…

A

Conduct small current in aqueous solutions

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9
Q

Nonelectrolytes

A

Do not conduct current in aqueous solutions

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10
Q

What does the extent to which solutions can conduct electricity depend on

A

It depends on the number of ions present

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11
Q

Types of strong electrolytes

A
  • soluble salts
  • strong acids
  • strong bases
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12
Q

when disolved in water, how do acids act

and what do they produce

A

They act as strong electrolytes
(produce H+ ions)

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13
Q

What am I?

Every molecule is completely ionized when dissolved in water

A

A strong acid

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14
Q

Ionization of an acid

x + x –> x + x

A

HA(aq) + H20(l) –> H3O+(aq) + A-(aq)

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15
Q

How does a strong base act

- what it produces and what it contains

A
  • Contains the OH- ion
  • when dissolved in water, cations of OH- ions seperate and move independently
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16
Q

Dissolving KOH in water

x –> x + x

A

KOH(s) –> K+(aq) + OH-(aq)

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17
Q

Weak electrolytes…

A
  • Exhibit a small degree of ionization in water
  • Include weak acids and weak bases

*dissociate only to a slight extent

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18
Q

What will be the resulting solution of a weak base

A

a weak electrolyte

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19
Q

What is a nonelectrolyte

A

Substances that dissolve in water but do not produce any ions (leads to absence of electrical conductivity)

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20
Q

What is molarity

A

Moles of solute per volume of solution in liters

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21
Q

What is dilution

A

Process of adding water to a concentrated (stock) solution to achieve the molarity desired for a particular solution

22
Q

Why is this correct:

Moles of solute after dilution = moles of solute before dilution

A

Since only water is added to accomplish dilution

23
Q

Formula for dilution

A

M1V1=M2V2

- M1 + V1 = for original solution
-M2 + V2 = for diluted solution

24
Q

Steps for the preperation of a standard aqueous solution

A

Process of preparation:
1. Place a weighed amount of the solute into a volumetric flask, and add a small amount of water
2. Dissolve the solid by swirling the flask
3. Add more water until the level of the solution reaches the mark etched on the flask
4. Mix the solution by inverting the flask several times

25
Q

Precipitation Reaction

A

When two solutions are mixed, a precipitate separates from the solution

26
Q

What is precipitate

A

Insoluble solid that is formed in a precipitation reaction

27
Q
A
28
Q

What kind of reaction is this:

When a yellow aqueous solution of potassium chromate is added to a colourless aqueous solution of barium nitrate, yellow barium chromate precipitates

A

A precipitation reaction

29
Q

Rules of solubility of salts in water

(6)

A
  1. Most nitrate (NO3-) salts are soluble.
  2. Most salts containing the alkali metal ions (Lit, Na+, K+, Cs+, Rb+) and the ammonium ion
    (NH+) are soluble.
  3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag+, Pb2+, and Hg2 2+,
  4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4, and CaSO4.
  5. Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH and
    KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH), are marginally soluble.
  6. Most sulfide (S2-), carbonate (CO3 2-), chromate (CrO4 2-), and phosphate (PO4 3-) salts are only slightly soluble, except for those containing the cations in Rule 2.
30
Q

What am I?

  • shows the complete chemical formula of reactantsand products
  • Does not provide correct information regarding the actual forms of the
    reactants and products
A

Formula equation

31
Q

What am I?

All reactants and products that are strong electrolytes are presented as ions

A

Complete ionic equation

32
Q

What am I?

Includes the solution components that undergo change (does not include spectator ions)

A

Net ionic equation

33
Q

What are spectator ions

A

Ions that do not participate in a chemical reaction

34
Q

According to the Brønsted Lowry definitions for acids and bases:

What is an acid and what is a base

A
  • Acid: it’s a proton donor
  • Base: It’s a proton acceptor
35
Q

What is a neutralization reaction

A

The name given to acid base reactions
-An acid is neutralized when enough base reacts exactly with it in a solution

36
Q

What is volumetric analysis

A

Technique used to ascertain the concentration of a given solution by using a solution of known concentration

37
Q

What is titration, a titrant and an analyte

A

-Titration: Delivery of a titrant into an analyte
- Titrant: Solution of known concentration
- Analyte: It’s the solution being analyzed

38
Q

In an acid-base titration

What is the equivalence (stoichiometric) point

A

Marks the point in titration where enough titrant has been added to react exactly with the analyte

39
Q

Definition of indicator

A

Substance added to show the end point of titration
(Changes color at the equivalence point)

40
Q

What is the endpoint

A

Point where the indicator actually changes color

41
Q

Requirements for a successful titration

(3)

A
  • Exact reaction between titrant and analyte must be known and must be rapid
  • Equivalence point must be accurately marked
  • Volume of titrant that is needed to reach the equivalence point must be accurately known
42
Q

what is Phenolphthalein

A

An indicator used in acid-base titrations
- Colourless in an acidic solution
- Pink in a basic solution

43
Q

What is an oxidation-reduction (redox) reaction

A

Involve the transfer of one or more electrons

44
Q

What is an oxidation state

For atoms in covalent compounds

A

imaginary charges that atoms would have if:
- Shared electrons were equally divided between identical atoms bonded to each other
- The shared electrons are assigned to the atom with the greater electron affinity

45
Q

What is an oxidation state

For monoatomic ions

A

the oxidation state is the charge of the ion

46
Q

What must the sum of oxidation states equal for electrically neutral compounds?

A

zero

47
Q

Oxidation

What is it? what is it characterized by?

A
  • Increase in oxidation state
  • Characterized by a loss of electron
48
Q

Reduction

What is it? what is it characterized by?

A
  • Decrease in oxidation state
  • Characterized by a gain of electron
49
Q

Reducing agent

A

Electron donor

50
Q

Oxidizing agent

A

Electron acceptor

Chemistry (7 decks)

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