Chapter 4

Question 1

Solvent

Answer 1

Component of a solution that is present in the greatest amount

Question 2

Solute

Answer 2

any component in the solution other than the solvent

Question 3

ppm of a solution component

Answer 3

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

Question 4

ppb of component

Answer 4

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

Question 5

Stock solution

Answer 5

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

Question 6

Dilution

Answer 6

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

Question 7

Mixing solution of 2 different substances

Answer 7

Mfa=MiaVa/(Va+Vb)

Mfb=MibVb/(Va+Vb)

Question 8

Mixing 2 solutions of the same substance

Answer 8

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

Question 9

Beer’s law definition, equation and variable meanings

Answer 9

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

Question 10

Electrolytes+types

Answer 10

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

Question 11

Acids and bases definitions

Answer 11

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

Question 12

Amphiprotic

Answer 12

Substance or ions that acts as an acid or a base

Question 13

Neutralization reaction

Answer 13

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

Question 14

Salt

Answer 14

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

Question 15

Molecular equations

Answer 15

Reactants/Products are written as undissociated molecules

Question 16

Overall ionic equations

Answer 16

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

Question 17

Net ionic equations

Answer 17

Remove spectator ions(ions present in reactants and products)

Question 18

Nonmetal oxides

Answer 18

Form acids in a hydrolysis reaction

Question 19

Titration

Answer 19

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

Question 20

Standard solution

Answer 20

a solution of known solution, also called a titrant

Question 21

Equivalence point

Answer 21

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

Question 22

End point

Answer 22

Point reached when indicator changes color

Question 23

Indicator

Answer 23

Weak acid/weak base that changes color when titrating

Question 24

Precipitate

Answer 24

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

Question 25

Soluble cations

Answer 25

Group 1 ions and NH4+

Question 26

Soluble anions

Answer 26

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+

Question 27

Insoluble compounds

Answer 27

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+

Question 28

Solubility of fluorides/chlorides

Answer 28

Soluble: Silver fluoride, H2F2 Poor solubility: MgF2, CaF2

Question 29

A combination of which two compounds results in a precipitate?

Answer 29

Insoluble anion+insoluble cation

Question 30

Metathesis reaction

Answer 30

Double displacement precipitation reaction

Question 31

Redox reactions/Oxidation/reduction definitions

Answer 31

Oxidation: Increase oxygen, lose electrons, increase oxidation number Reduction: Loss of oxygen, gain electrons, decrease oxidation number Redox reactions: gain/lose electrons

Question 32

Oxidation numbers for: 1. Pure elements 2. Monoatomic ion 3. Fluorine 4. Br and Cl 5. H and O

Answer 32

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)

Question 33

Oxidizing/reducing agents

Answer 33

Reducing agent: Oxidized Oxidizing agent: reduced

Question 34

Which elements are active metals? noble metals?

Answer 34

Active: Alkali, alkaline earth metals noble metals: group 11, Cu, Ag, Au and neighboring metals in periods 5 and 6