Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem 141 Dr. Mark Cybulski > Chapter 4 > Flashcards

Chapter 4 Flashcards

1
Q

Solvent

A

Component of a solution that is present in the greatest amount

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

Solute

A

any component in the solution other than the solvent

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

ppm of a solution component

A

Mass of component/total mass of solution•10^6

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

ppb of component

A

mass of component in solution/total mass of solution•10^9

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

Stock solution

A

A concentrated solution of a substance used to prepare solutions of lower concentrated

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

Dilution

A

The profess of lowering the concentration of a solution by adding more solvent. Number of moles of solution does not change, only volume

Vi•Mi=Vd•Md=n
n=number of moles of solute present in the solution

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

Mixing solution of 2 different substances

A

Mfa=MiaVa/(Va+Vb)

Mfb=MibVb/(Va+Vb)

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

Mixing 2 solutions of the same substance

A

Mf=(M1V1+M2V2)/(V1+V2)

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

Beer’s law definition, equation and variable meanings

A

Intensity of color can be used to measure concentrations of solution
A=ebc
A=Absorbance
e=molar absorptivity(actually looks like backwards 3)
b=path length
c=concentration

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

Electrolytes+types

A

Substances that break into ions when they are dissolved in water

Strong electrolytes: Completely(nearly) ionize: consist of strong acids, strong based and soluble salts. Conduct currents efficiently

Weak electrolytes: Partially ionized: weak acids and bases. Slightly conductive

Nonelectrolytes: substances that do not break into ions when they are dissolved in water. Sugar, enthanol, ethylene

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

Acids and bases definitions

A

Acids
Arrhenius: acids yield H+ ions when dissolved in wayer
Bronsted and Lowry: Acids are proton donors

Bases
Arrhenius: Yield OH- ions when dissolved in water
Bronsted and Lowry: Bases are proton acceptors

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

Amphiprotic

A

Substance or ions that acts as an acid or a base

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

Neutralization reaction

A

a reaction that takes place when and acid and base react to produce a salt and water

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

Salt

A

Product of a neutralization(acid/base) reaction, made up of a cation base plus an anion acid. Salts are ionic

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

Molecular equations

A

Reactants/Products are written as undissociated molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Overall ionic equations

A

Distinguish between molecular/ionic substances, ionic species are represented as dissolved ions

17
Q

Net ionic equations

A

Remove spectator ions(ions present in reactants and products)

18
Q

Nonmetal oxides

A

Form acids in a hydrolysis reaction

19
Q

Titration

A

An analytical method to determine concentration of a solute in a sample by reacting it with a standard solution

20
Q

Standard solution

A

a solution of known solution, also called a titrant

21
Q

Equivalence point

A

point when moles of added titrant are stoichiometrically equivalent to moles of substance being analyzex

22
Q

End point

A

Point reached when indicator changes color

23
Q

Indicator

A

Weak acid/weak base that changes color when titrating

24
Q

Precipitate

A

Solid product formed from a reaction in solution, precipitate formula can be predicted based on solubility rules

25
Q

Soluble cations

A

Group 1 ions and NH4+

26
Q

Soluble anions

A

Nitrate, acetate, perchlorate

Cl-, Br- and I- unless bonded to Ag+, Cu+, Pb2+ or (Hg2)2+

Sulfates except sulfates of Pb2+, (Hg2)2+, Ca2+, Ba2+, Sr2+

27
Q

Insoluble compounds

A

All hydroxides except group 1, Ca, Sr and Ba hydroxides

All sulfides except group 1 and NH4+, CaS, SrS and BaS

All carbonates except group 1 and NH4+

All phosphates except group 1 and NH4+

28
Q

Solubility of fluorides/chlorides

A

Soluble: Silver fluoride, H2F2

Poor solubility: MgF2, CaF2

29
Q

A combination of which two compounds results in a precipitate?

A

Insoluble anion+insoluble cation

30
Q

Metathesis reaction

A

Double displacement precipitation reaction

31
Q

Redox reactions/Oxidation/reduction definitions

A

Oxidation: Increase oxygen, lose electrons, increase oxidation number

Reduction: Loss of oxygen, gain electrons, decrease oxidation number

Redox reactions: gain/lose electrons

32
Q

Oxidation numbers for:

  1. Pure elements
  2. Monoatomic ion
  3. Fluorine
  4. Br and Cl
  5. H and O
A
  1. 0
  2. Charge of ion
  3. -1
  4. -1 unless combined with O or F
  5. H=+1, Oxygen=-2(except peroxides, O=-1)
33
Q

Oxidizing/reducing agents

A

Reducing agent: Oxidized

Oxidizing agent: reduced

34
Q

Which elements are active metals? noble metals?

A

Active: Alkali, alkaline earth metals

noble metals: group 11, Cu, Ag, Au and neighboring metals in periods 5 and 6

Chem 141 Dr. Mark Cybulski (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions