Solutions

Question 1

Less than the maximum amount of a solute is dissolved in a solvent

Answer 1

unsaturated

Question 2

the maximum amount of a solute is dissolved in a solvent

Answer 2

saturated

Question 3

Soluble salts are group ____ metal cations, ___, ___, ___ and ___

Answer 3

1, NO3, ClO4-, C2H3O2, NH4+

Question 4

Insoluble salts are __, __, __, __, __, __, ___

Answer 4

Ag+, Pb2+, Hg2+, OH-, S2-, CO32-, PO43-

Question 5

The molecule as a whole is ___ if there is at least one soluble compound in it

Answer 5

soluble

Question 6

Electrolytes are substances that have a natural __ or __ charge when dissolved in water. They help the body regulate __ ___ and maintain balance between __ in and outside cells

Answer 6

positive, negative, chemical reactions, fluids

Question 7

electrolyte that fully dissociates in water

Answer 7

strong electrolyte

Question 8

electrolyte that incompletely dissociate in water

Answer 8

weak electrolytes

Question 9

electrolytes that do not dissociate in water

Answer 9

non-electrolytes

Question 10

Strong electrolytes are soluble ___ ___, strong __ and ____

Answer 10

ionic compounds, acids, bases

Question 11

Strong acids are ___, __, __, ___, __, __, and ___

Answer 11

HCl, HBr, HI, HClO4, HClO3, H2SO4, HNO3

Question 12

Strong bases are group 1 __ __, ___, __ and ___

Answer 12

metal hydroxides, Ba(OH)2, Sr(OH)2, Ca(OH)2

Question 13

Weak electrolytes are weak ___ and ____

Answer 13

acids bases

Question 14

non electrolytes are molecular compounds that aren’t __ or __ such as ___ and __

Answer 14

acidic, basic, C6H12O6, CH3OH

Question 15

solids are more soluble at ___ temperatures. Gases are more soluble at ___ temperatures, and _____ pressures

Answer 15

higher, lower, higher

Question 16

When light is passed through a solution and a spectrophotometer is used to measure how much is sent in and comes out

Answer 16

spectrophotometry

Question 17

Beer’s law says that light absorption is __ to path length and the __ of the solution, and is given by the formula ____. It demonstrates that a more ____ solution absorbs more light than a ____ solution

Answer 17

proportional, concentration, A=elc, concentrated, dilute

Question 18

Equations in which all compounds are written as though all substances exist as molecules

Answer 18

molecular equations

Question 19

Equations in which ionic compounds are written as separated ions

Answer 19

ionic equation

Question 20

Ions that do not take part in the reaction and are found in solution before and after the reaction

Answer 20

spectator ions

Question 21

Equations that only shows the elements, compounds and ions directly involved in the reaction

Answer 21

net ionic equations

Question 22

If molecules of a solute experience the same __ __ as the solvent, the solute will likely ___ in that solvent

Answer 22

intermolecular forces, dissolve

Question 23

Samples of matter with both definite and constant composition and distinct chemical properties; elements and compounds

Answer 23

pure substances

Question 24

made with two or more combined substances that are not combined chemically

Answer 24

mixtures

Question 25

the number of moles of solute per 1 kg of solvent

Answer 25

molality

Question 26

The new concentration of volume of a solution after a dilution is given by the formula __-

Answer 26

M1V1=M2V2

Question 27

Normality expresses the concentration in terms of the ___ of one chemical species that react stoichiometrically with another chemical species and is given by ___

Answer 27

equivalents, N = nxM

Question 28

the part of a chemical species that participates in the chemical reaction

Answer 28

equivalents

Question 29

the ratio of the number of moles of one component of a mixture to the total number of moles; should equal one in total

Answer 29

mole fraction

Question 30

Properties that depend on the concentration of solute molecules or ions but not on the identity of the solute

Answer 30

colligative properties

Question 31

properties that depend on the identity of the dissolved species and the solvent

Answer 31

non colligative properties

Question 32

Some non colligative properties are ___ __, ___, ____, __ and ___

Answer 32

surface tension, viscosity, solubility, colour, density

Question 33

colligative properties include ____ __, ____ ___, ____ __, and ___ ___

Answer 33

vapor-pressure depression, boiling-point elevation, freezing-point elevation, osmotic pressure

Question 34

the boiling point is when the vapor pressure is equal to the __ __

Answer 34

atmospheric pressure

Question 35

As elevation increases, the atmospheric pressure ___, this means that the vapor pressure needed to reach the boiling point ____ and boiling point ____

Answer 35

decreases, decreases, decresases

Question 36

As elevation decreases, the atmospheric pressure ___, and the vapor pressure needed to reach the boiling point ___, and thus the boiling point ___

Answer 36

increases, increases, increases

Question 37

in general an increase in __ ___ equal a decrease in boiling point. When a solute is added, the vapor pressure is ____ and thus the boiling point is ___. Thus, the vapor pressure of a ___ __ is greater than that of a solution with a ___ ___

Answer 37

vapor pressure, lowered, raised, pure solvent, non-volatile solute

Question 38

Raoult’s law

Answer 38

Pa = XaP°a

Question 39

Boiling point elevation equation

Answer 39

Tb change = kb i m

Question 40

the number of particles the solute breaks into when it dissolves

Answer 40

van’t hoff factor (i)

Question 41

freezing point depression equation

Answer 41

Tf change = -kf im

Question 42

the pressure it would take to stop osmosis from happening

Answer 42

osmotic pressure

Question 43

Equation for osmotic pressure

Answer 43

osmotic pressure = i MRT