Ap Chem Chapter 4 Test

Front 1

What is the solute

Back 1

the substance dissolved in the solvent

Front 2

what are strong electrolytes

Back 2

substances that are completely ionized when they are dissolved in water; conduct electricity very well

Front 3

What are the three kinds of strong electrolytes

Back 3

Soluble Salts
Strong Acids (ionize to produce H+ and Anion-)
Strong Bases(Ionize to produce cation and OH-)

Front 4

Name the strong Acids

Back 4

HCl
HNO3
H2SO4 (First H+ only)

Front 5

Name the strong Bases

Back 5

NaOH
KOH

Front 6

What are weak electrolytes

Back 6

Exhibit a small degree of ionization in water; conduct only a small electrical current

Front 7

what is a nonelectrolyte

Back 7

dissolve in water but do not produce ions; solution does not conduct electricity

Front 8

What is the formula for Molarity

Back 8

Molarity=(moles of solute/Liters of solution)

Front 9

What is a standard solution

Back 9

a solution whose concentration is accurately known

Front 10

What is the formula for Dilution

Back 10

m1v1=m2v2

Front 11

What is a precipitate

Back 11

solid that forms (and separates from solution) when 2 solutions are mixed

Front 12

What is a net-ionic equation

Back 12

Includes only those solution components (ions) directly involved in the reaction

Front 13

What is the first solubility rule

Back 13

1. Most Nitrate(NO3^1-) salts are soluble and acetate salts

Front 14

What is the second solubility rule?

Back 14

2. Most salts containing the alkali metals ions (group 1A) and the ammonium ion (NH4+) are soluble.

Front 15

What is the third solubility rule

Back 15

3. Most Chloride, Bromide, and iodide salts are soluble. Notable exceptions are salts containing Ag+, Pb2+, and Hg2^2+.

Front 16

What is the fourth solubility rule

Back 16

4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4, and CaSO4.

Front 17

What is the fifth solubility rule

Back 17

5. Most hydroxide salts are only slightly soluble. The important soluble hydroxides are NaOH and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble.

Front 18

What is the sixth solubility rule

Back 18

6. Most sulfide (S^2-, carbonate (CO3^2-), chromate (Cr04^2-), and phosphate (PO4^3-) salts are only slightly soluble

Front 19

What is Volumetric analysis?

Back 19

technique for determining the amount of a certain substance by titration

Front 20

What is titration

Back 20

delivery (from a buret) of a measured volume of a solution of known concentration (the titrant) into a solution containing the substance being analyzed (the analyte)

Front 21

What is the equivalence point (stoichiometric point)

Back 21

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

Front 22

What is the indicator

Back 22

substance added at or near the beginning of the titration that changes color at (or very near) the equivalence point

Front 23

What is the endpoint?

Back 23

the point of titration where the indicator actually changes color

Front 24

What are the three requirements necessary for a titration to be successful

Back 24

1. The exact reaction between the titrant and the analyte must be known
2. The stoichiometric (equivalence) point must be marked accurately
3. The volume of the titrant required to reach the stoichiometric point must be known accurately

Front 25

What are redox reactions

Back 25

Reactions in which one or more electrons are transferred

Front 26

What is Florine's oxidation number in its compounds

Back 26

-1

Front 27

What is Oxygen's oxidation number it its compounds

Back 27

usually -2, but -1 in peroxides

Front 28

What are the units of pressure and what are the conversions

Back 28

mm Hg= torr
atmosphere
pascals
1atm=760 mmHg=760 torr= 101.325kPa

Front 29

Volume and Pressure are _________ proportional

Back 29

inversely

Front 30

What is Boyle's Law

Back 30

p1v1=p2v2

Front 31

What is an ideal gas?

Back 31

a gas that strictly obey's Boyle's law

Front 32

What is Charles's Law

Back 32

The volume of a gas increases linearly. (v1/t1)=(v2/t2)

Front 33

What is Avogadro's Law

Back 33

For a gas at a constant temperature and pressure, the volume is directly proportional to the number of moles. (v1/n1)=(v2/n2)

Front 34

What is the ideal gas law

Back 34

PV=nRT

Front 35

What does the ideal gas law express

Back 35

Expresses behavior that real gases approach at low pressures and high temperatures

Front 36

Explain the STP relation

Back 36

1 mole of an ideal gas at standard temperature and pressure (0ºC and 1atm) has a volume of 22.42 L

Front 37

Explain the relation between Molar mass and the gas properties

Back 37

Molar mass = (density(d)*R*T)/P

Front 38

What is Dalton's Law? What are the equations that go with it?

Back 38

For a mixture of gases in a container, the total pressure exerted in the sum of the pressures that each gas would exert if it were alone in the container.
Ptot=Pa+Pb+Pc...
Ptot=(Ntot*R*T)/V
Pa=(Na*R*T)/V
...etc

Front 39

What is the mole fraction (X)?

Back 39

The ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture
Xa=(Na/Ntotal)=(Pa/Ptotal)

Front 40

What is the Kinetic Molecular Theory?

Back 40

1. The Particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be negligible (zero).
2. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by gas.
3. The particles are assumed to exert no force on each other; they are assumed neither to attract nor to repel each other.
4. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.

Front 41

What is the formula for average Kinetic Energy

Back 41

(3/2)RT

Front 42

What is the formula for Root Mean Square Velocity

Back 42

√(3RT/M) R = 8.3145 J/K mol

Front 43

What is effusion?

Back 43

The passage of a gas through a tiny orifice into an evacuated chamber

Front 44

what does the rate of effusion measured?

Back 44

The rate of effusion measures the speed at which the gas is transferred into the chamber

Front 45

Explain the formula for Effusion

Back 45

the rate of effusion of a gas is inversely proportional to the square root of the mass of its particles. (rate of effusion for gas 1/rate of effusion for gas 2) = √M2/√M1