Chapter 12: Solutions (sections 1 & 2) Flashcards Preview

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Flashcards in Chapter 12: Solutions (sections 1 & 2) Deck (34)
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1
Q

the composition of a solution is expressed as

A

concentration

2
Q

conentration is always expressed as the quantity of .. present in a fixed quantity of the … or …

A

solute; solution; solvent

3
Q

for most solutes, there is a limit to the quntity that can dissolve in a

A

fixed volume of a given solvent

4
Q

the solubility of a solute is reached when the …. and the …. are equal

A

rate of dissolution; rate of crystallization

5
Q

solubility is the concentration of solute that exists in equilibrium with an ….; that is, it is the maximum concentration that can … at a particular temperature

A

excess of that substance; dissolve

6
Q

a saturated solution is one that is in equilibrium with

A

an excess of the solute

7
Q

the concentration of a saturated solution is equal to the

A

solubility

8
Q

an unsaturated solution is one in which the concentration of the solute is

A

less than the solubility

9
Q

supersatured solutions have a concentration of solute that is

A

temporarily greater tahn its solubility

10
Q

supersaturation is an … condition

A

unstable

11
Q

two of the most important factors that determine whether a given substance will dissolve in a solvent include:

A

the enthalpy change that accompanies solute-solvent interactions
change in disorder

12
Q

three types of intermolecular forces are involved in the formation of condensed phase solutions:

A

solute-solute, solvent-solvent, solute-solvent

13
Q

(steps in solution formation) step 1 ΔH1: expanding the solute: separating the solute into

A

individual components; endothermic

14
Q

(steps in solution formation) step 2 ΔH2: expanding the solvent: overcoming …. of the solvent molecules

A

intermolecular forces ;endothermic

15
Q

(steps in solution formation) step 3 ΔH3: interaction of … and … to form the solution

A

solute; solvent; exothermic

16
Q

enthalpy of solution=

A

ΔH1 + ΔH2 + ΔH3

17
Q

heat of solution is the amount of heat energy absorbed or released when a

A

specific amount of solute dissolves in a solvent

18
Q

many substances with positive enthalpies of solution still dissolve … due to an increase in .. (…) which is favorable

A

spontaneously; entropy; disorder

19
Q

water surrounds ions in a

A

sphere of hydration

20
Q

disorder increases significantly when ionic solids

A

dissolve in solution

21
Q

the interaction of the ions with water molecules is called

A

hydration

22
Q

pressure has very little effect on the solubilities of .. and ..

A

solids; liquids

23
Q

the solubility of a gas is directly proportional to its …. at a …./ [a] is calculated via …

A

partial pressure; given temperature; henry’s law

24
Q

henry’s law:

A

C=kP

25
Q

an increase in pressure favors the

A

denser phase

26
Q

for gaseous solutes, an increase in pressure is relieved by additional

A

gas dissolving in the liquid

27
Q

le chatelier’s principle can be used to predict what is favored:
endothermic:
exothermic:

A

A + solvent + heat ↔ solution

B + solvent ↔ solution + heat

28
Q

as temperature increases, the solubility … for any substance with an endothermic enthalpy of solution and … for one with an exothermic enthalpy of solution

A

increases; decreases

29
Q

since the enthalpy of solution for most gases in water is exothermic their solubilities … with an increase in temperature

A

decrease

30
Q

the solubilities of most solids … as the temperature of the solution increases

A

increases

31
Q

some substances that appear to violate these generalizations undergo a more

A

complex dissolution process

32
Q

the rte at whcih solids dissolve …. with increasing surface area of the solid

A

increases

33
Q

solids tend to dissolve best when:

A

heated, stirred, ground into small particles

34
Q

gases tend to dissolve best when: the solution is …, … is high

A

cold; pressure