Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 1210 > Ch 4. Reactions in an Aqueous Solution > Flashcards

Ch 4. Reactions in an Aqueous Solution Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Solution

A

a homogenous mixture of two or more substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Solvent

A

the substance present in the greatest quantity in a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Solutes

A

the other substance in a solution that are not the solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Electrolyte

A

a substance whose aqueous solutions contain ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

nonelectrolytes

A

a substance that does not form ions in a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Solvation

A

helps stabalize the ions in a solution and prevents cations and anions from recombining.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Dissociation

A

when an ionic substance dissolves in H2O, the solvent pulls the individual ions from the crystal and solvates them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Are most molecular compounds nonelectrolytes?

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What molecular compounds are electrolytes

A

Acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Strong Electrolytes

A

are solutes that exist in a solution completly or nearly completly as ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Weak Electrolytes

A

solutes that exist in solutions mostly in the form of neutral molecules with only small fractions in the form of ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Chemical Equilibrium

A

a state in which the relative numbers of each type of ion or molecule in the reaction are constant overtime.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Precipitation Reactions

A

reactions that result in the formation of an insoluble product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Precipitate

A

an insoluble solid formed by a reaction in a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Soluble Ionic Compounds

A 
NO3-
CH3COO-
Cl-
Br-
I-
SO4-
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Exceptions to NO3- solubility

A

None

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Exceptions to CH3COO-

A

None

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Exceptions to Cl- Solubility

A

Pb 2+, Hg 2+, Ag +

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Exceptions to Br- solubility

A

Pb 2+, Hg 2+, Ag +

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Exceptions to I- solubiltiy

A

Pb 2+, Hg 2+, Ag +

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Exceptions to SO4- solubiltiy

A

Sr 2+, Ba 2+, Hg 2+, Pb 2+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Insoluble compounds

A

S 2-
CO3 2-
PO4 2-
OH -

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Exception to insoubility of S 2-

A

NH4 +, alkali Metals, Ca 2+, Sr 2+, Ba 2+

24
Q

Exceptions to insolubility of CO3 2-

A

NH4 +, Alkali Metals

25
Q

Exceptions to insolubility of PO4 2-

A

NH4 +, Alkali Metals,

26
Q

Exceptions to insolubility of OH-

A

NH4 +, Alkali Metals, Ca 2+, Sr 2+, Ba 2+

27
Q

Metathesis Reaction

A

AX + BY —> AY + BX

28
Q

Molecular Equations

A

Shows the chemical formulas without indicating ionic characters

29
Q

Complete Ionic Equations

A

A chemical equation in which dissolved strong electrolytes are written as seperate ions

30
Q

Spectator Ions

A

ions that appear in identical form on both sides of a complete ionic equation and play no role in the reaction

31
Q

Net ionic equation

A

includes only the ions and molecules directly involved in the reaction

32
Q

Strong Acids

A 
HCl
HBr
HI
HClO3
HClO4
HNO3
H2SO4
33
Q

Strong Bases

A 
LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
34
Q

Acids

A

substances that ionize in aqueous solutions to form H+

-proton donors

35
Q

Monoprotic acids

A

yield 1 H+

36
Q

diprotic acids

A

yield 2 H+

37
Q

Bases

A

substances that accept H+ ions and produce OH- ions in water

  • a proton exceptor
  • they do not have to contain OH-
38
Q

Strong Electolytes are

A

Ionic

strong acids and bases

39
Q

Weak Electrolytes are

A

Weak acids and Bases

40
Q

Nonelectolytes

A

All molecular compounds that are not acids or bases

41
Q

Neutrilization reaction

A

when a soultion of an acid and base are mixed

42
Q

salt

A

any ionic compound whose cation comes from a base and whose anion comes from a acid

43
Q

Oxidation-reduction reaction/ redox reaction

A

reactions in which electrons are transferred from one reactant to another

44
Q

Oxidation

A

Loss of electrons by a substance

45
Q

Reduction

A

the gain of electrons by a substance

46
Q

oxidation numbers/states

A

a positive or negative whole number assigned to an element in a molecule or ion on the basis of a set of formula rules

47
Q

Displacement reactions

A

the ion in the solution is displaced/replaced through oxidation of an element

48
Q

Activity Series

A

a list of metals arranged in order of decreasing ease of oxidation
-any metal on the list can be oxidized by the ions of elements below it

49
Q

Active metals

A

react most readily to form compounds

-alkali metals and alkaline earth metals

50
Q

Noble metals

A

are very stable and form less readily

-near the bottom of the table

51
Q

Concentration

A

designates the amount of solute dissolved in a given quantity of solvent or quantity of solution

52
Q

Molarity (M)

A

expresses the concentration of a solution as the number of moles in a liter of solution
- a conversion factor between volume of a solution and moles of solute

53
Q

Molarity Formula

A

M= Moles of solute/Volume of solution in Liters

54
Q

Dilution

A

adding water to concentrated solutions

-moles of solute before dilution = moles solute after dilution

55
Q

Dilution Formula

A

M1 x V1 = M2 x V2

56
Q

Titration

A

involves combining a solution where the solute concentration is not known with a reagent solution of known concentration called a standard solution

57
Q

Equivalence Point

A

the point at which stoichiometrically equivalent quantities are brought together

Chem 1210 (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions