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Chem 115 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

What are two reasons why the actual yield from a chemical reaction is usually less than the theoretical yield?

A

1) The observed, or actual, yield for a reaction is usually less than the theoretical yield because reactions do not always go to completion
2) the reaction may be slow or may have, for a portion of the reaction, created different products than expected

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2
Q

What kind of anhydride is dichlorine trioxide? What type of solution will be formed? What color litmus paper should be used to test the relative pH of the solution formed?

A

Cl2O3 is a nonmetal oxide and an acid anhydride.
Acidic Cl2O3+H2O —> [H2Cl2O4] —> 2HClO2 which is a weak acid
Blue paper should be used to test for acidity

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3
Q

What kind of anhydride is potassium oxide?

A

K2O metal oxide and a base anhydride
Basic: K2O + H2O —> 2KOH which is a strong base
Use red litmus paper to test for basicity

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4
Q

What are the differences between strong electrolytes, weak electrolytes, and non-electrolytes in terms of i) electrical conductivity in water and ii) how they dissolve in water

A
  • Strong electrolytes conduct a strong electrical current and dissociate 100% into ions in H2O
  • Weak electrolytes conduct a weak electrical current and dissociate less than 100% into ions in H2O (mostly neutral molecules)
  • Non-electrolytes conduct no electrical current and dissolve as neutral molecules in H2O
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5
Q

Identify as a strong, weak, or non electrolyte when dissolved in water. Indicate how it dissolves in water.

CaCl2*

A

Strong electrolyte
Ions
Ca+2 + 2Cl-

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6
Q

NH3*

A

Weak electrolyte
Weak base
Mainly NH3

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7
Q

HCLO4*

A

Strong electrolyte
Strong acid
H+ + CLO4-

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8
Q

Fe(NO3)3*

A

Strong electrolyte
Ions
Fe+3 + 3NO3-

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9
Q

Ba(OH)2*

A

Strong electrolyte
Strong base
Ba+2 + 2OH-

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10
Q

H2SO3

A

Weak electrolyte
Weak acid
H2SO3

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11
Q

O2*

A

Non-electrolyte
Molecular compound
O2

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12
Q

(CH3)2NH*

A

Weak electrolyte
Weak base
(CH3)2NH

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13
Q

AgNO3*

A

Strong electrolyte
Ionic
Ag+ + NO3-

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14
Q

AgCL*

A

Non-electrolyte
Insoluble I.C
AgCL

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15
Q

NiSO4*

A

Strong electrolyte
Ionic
Ni2+ + SO4-2

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16
Q

BaSO4*

A

Non-electrolyte
Insoluble I.C
BaSO4

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17
Q

C12H22O11*

A

Non-electrolyte
Molecular compound
Neutral

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18
Q

HNO2*

A

Weak electrolyte
Weak acid
HNO2

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19
Q

HCLO2*

A

Weak electrolyte
Weak acid
Mainly HCLO2

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20
Q

C2H5OH

A

Non-electrolyte
Molecular compound
C2H5OH

21
Q

HNO3*

A

Strong electrolyte
Strong acid
H+ + NO3-

22
Q

H2S*

A

Weak electrolyte
Weak acid
Mainly H2S

23
Q

What are the Bronsted-Lowry definitions for acids and bases?

A

Acid: proton donor
Base: proton acceptor

24
Q

What are the Arrhenius definitions for acids and bases?

A

Acid: produces H+ when dissolved in H2O
Base: produces OH- when dissolved in H2O

25
Q

What are the differences between strong and weak acids?

A

Strong acids dissociates/ionizes 100% to produce H+/H3O+

Weak acid is less than 100% dissociation

26
Q

What are the differences between strong and weak bases?

A

Strong bases dissociate 100% and weak bases less than 100% to produce OH-

27
Q

List the strong acids

A

HI, HCL, HBr, HNO3, HCLO3, HCLO4, H2SO4

28
Q

List the strong bases

A

LiOH, NaOH, KOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

29
Q

Short of weak acids

A

H3PO4, H2S, HC2H3O2, HNO2, H2SO3, HCLO3-

30
Q

Short list of weak bases

A

NH3, NH2OH, CH3NH2, (CH3)2NH

31
Q

Discuss the electrolyte activity of strong and weak acids and bases.

A

Strong acids/bases are strong electrolytes and weak acids/bases are weak electrolytes

32
Q

CH3CH2CH2OH

A

Is not a strong base
Is not a hydroxide
Is an alcohol

It differs from NaOH when it dissolves in water because propanol is a molecular compound, so even though it dissolves, it does not dissociate into ions like NaOH does

33
Q

Any substance that has the (aq) designation splits into ions when dissolved in solution…..true or false

A

False because the (aq) designation only indicates that a substance dissolves in water but NOT how it dissolves. It should read “Any substance that is a strong electrolyte splits into ions when dissolved in aqueous solution”

34
Q

Define equivalence point

A

Point where stoichietric amounts of both reagents are present

35
Q

Define indicator

A

Substance with one color in more acidic solutions and different color in more basic

36
Q

Define end point

A

Point in titration where indicator changes color

37
Q

Define the term solute

A

Any component in a solution other than the solvent

Substance dissolved in solvent

38
Q

Define the term solvent

A

A component of a solution that is present in the greatest amount

Substance dissolving the solute

39
Q

Define the term solution

A

Resulting mix of solute and solvent, solute in uniformly distributed

40
Q

Define solubility

A

Measure of maximum amount of solute that will dissolve in a given amount of solvent (measured in g/100mL)

41
Q

Define unsaturated solution

A

a chemical solution in which the solute concentration is lower than its equilibrium solubility

42
Q

Define saturated solution

A

a chemical solution containing the maximum concentration of a solute dissolved in the solvent

43
Q

Define supersaturated solution

A

a state of a solution that contains more of the dissolved material than could be dissolved by the solvent under normal circumstances

44
Q

Solubility Rule 1

A

Ionic compounds that contain Group 1(IA) metal cations (Na+, K+, Li+, etc.) or ammonium (NH +) are soluble.
4

45
Q

Solubility Rule 2

A

Ionic compounds that contain NO -, ClO -, ClO -, C H O -, or HCO - are soluble.

46
Q

Solubility Rule 3

A

Ionic compounds that contain Cl-, Br-, or I- (halogens) are soluble EXCEPT when combined with Cu+, Ag+, Hg 2+, or Pb2+. Most F- compounds are soluble EXCEPT when combined with Pb2+ and Group 2(Ca+2, Ba+2, etc).

47
Q

Solubility Rule 4

A

Ionic compounds that contain SO 2- are soluble EXCEPT when combined with Ag+, Hg 2+,
2+ 2+ 2+ 2+ 4 2 Pb , Ca , Sr , or Ba . Note: Ag2SO4 is sparingly soluble.

48
Q

Solubility Rule 5

A

Most ionic compounds that contain OH-, O2-, CO 2-, PO 3-, CrO 2-, or S2- are insoluble 344+
EXCEPT when combined with Group 1(IA) metal cations or NH4 .
– Extra exception(s): CrS, SrS, and BaS are considered soluble. Ca(OH)2, Ba(OH)2, and Sr(OH)2 are considered soluble. Group 1 and heavier Group 2 oxides react with water to form corresponding hydroxide which is soluble.

49
Q

Solubility Rule 6

A

Combining anions and cations not listed above results in formation of an insoluble compound

Chem 115 (3 decks)

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