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AP Chemistry > chapter 4: Chemical Reactions in Solution > Flashcards

chapter 4: Chemical Reactions in Solution Flashcards

1
Q

for a reaction to occur, species must

A

collide

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2
Q

solvent: component that has the same … as the …

A

physical state; solution

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3
Q

solute: substance being … to form a solution; typically in … than the solvent; often a … but can also be a … or …

A

dissolved; lesser amounts; solid; gas; liquid

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4
Q

solution: a … mixture; often composed of substances …

A

homogeneous; dissolved in water

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5
Q

most common solvent:

A

water

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6
Q

solutions with water as solvent:

A

aqueous solutions

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7
Q

most ionic compounds:

A

electrolytes

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8
Q

strong electrolytes separate

A

Completely into ions

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9
Q

;solutions of strong electrolytes are good

A

conductors of electricity

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10
Q

compounds that dissolve but do not conduct electricity are …. they do not dissociate into ions when …

A

nonelectrolytes; dissolved

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11
Q

molecular compounds that only partially .. in solution are called …

A

ionize; weak electrolytes

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12
Q

acetic acid is a

A

weak electrolyte

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13
Q

double arrow indicates that the reaction proceeds in

A

both directions

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14
Q

acids that ionize completely are known as

A

strong acids

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15
Q

strong and weak acids are also

A

strong and weak electrolytes

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16
Q

weak electrolytes produce only a … when dissolved in water

A

few ions

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17
Q

solubility: the concentration of solute that exists in … with an … of that substance

A

equilibrium; excess

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18
Q

(soluble ionic compounds) no exceptions:

A

group 1 cations and ammonium; nitrates; perchlorates; acetates

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19
Q

(soluble ionic compounds) exceptions:

A

chlorides, bromides, iodides (except Ag, dimercury, lead (II))
sulfates (except, dimercury, lead (II), Sr2+, barium)

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20
Q

(insoluble ionic compounds) with exceptions of only group 1 cations and ammonium

A

carbonates; phosphates

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21
Q

(insoluble ionic compounds) with exceptions group 1 cations, ammonium, and others

A

hydroxides (except group 1, ammonium, Sr2+, barium)

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22
Q

solubility must be determined

A

experimentally

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23
Q

a precipitation reaction involves the formation of an …. from the reaction of …

A

insoluble product(s); soluble reactants

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24
Q

the products, if any, of many reactions of ionic compounds can be predicted from

A

solubility rules

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25
overall equation: shows all of the reactants and products in
undissociated form
26
complete ionic equation: more ... description; an equation in which strong electrolytes are shown as ... in the solution
accurate; ions
27
complete ionic equation represents the species as tey
exist in solution
28
spectator ions: do not participate in any
chemical achange
29
net ionic equation: shows only those species in the solution that actually
undergo a chemical change
30
net ionic equations are useful in writing ...
acid-base reactions
31
water is not present as ..., can be written as a product in a ...
ions; net ionic equation
32
concentration of a solution: the amount of ... in a given quantity of that ...
solute; solution
33
molarity: number of ... of solute per ... of solution
moles; liter
34
molarity is a measure of
concentration
35
molarity is based on the ... olume fo solution, not on the volume of ...
volume; added solvent
36
To prepare a solution, a given mass of solute is measured, added to a ... Or..., some... is added to ... the solute, and additional ... is added until the final desired volume is ...
volumetric flask; graduated sylinder; solvent; dissolve; solvent; achieved
37
solutions of known molarity can be prepared from a weighted sample dissolved in a solvent, then ... to a known volume of solution
diluted
38
the molarity of a solution provides the ... that converts between .... and ...
relation; volume of solution; moles of solute
39
it is common to use square brackets around a species to imply
concentration of this species in units of molarity
40
less .. solutions are often prepared from more ... stock solutions
concentrated; highly concentrated
41
the difference between preparing a dilute solution and preparing a regular solution is that the concentration of the new diluted solution is based on a known ... of the concentrated solution rather that on the ...
volume; mass of the solute
42
pipet: a calibrated device designed to deliver an .... of liquid with ...
accurately known volume; high precision
43
m1v1=
m2v2
44
dilution of a given amount of a concentrated solution does not change the number of
moles of solute
45
the moles of solute in the concentrated solution are the same as in th
dilute solution
46
the only difference between the two solutions is tha tmore solvent is present in th
dilute solution
47
m1v1=m2v2 cannot be used for problems involving
chemical reactions
48
solution stoichiomtry equations are similar to ch 3 problems, but the amounts are calculated from the ... of solutions of known ... rather than from ...
volumes; concentrations; masses
49
titration: a procedure to determine the ... of one substance by adding a measured amount of a ....
quantity; second substance
50
equivalence point: the point at which stoichiometrically ... of the two reactants are present
equivalent amounts
51
an acid-base titration is a titration n which the amount of an unknown acid or base is determined by adding a .... of a known ... of ... or ... to ... the unknown
given amount; concentration; base; acid; neutralize
52
indicators are used to detect the ... in acid-base titrations
equivalence point
53
an indicator is a compound that changes ...as an ... solution becomes ... or vice versa
color; acidic; basic
54
the point at which the indicator ... color is called the ....
changes; end point
55
a standard solution is a solution with an accurately known
concentration
56
volumetric analysis: a chemical analysis that involves measurement of the ... of a ... or ...
volume; solution; substance
57
a ... is chosen to standardize an acid
high-purity base
58
a precipitation reaction can be used to isolate a ... from a solution
desired ion
59
gravimetric analysis is a procedure in which one component of a solution is selectively
precipitated, separated from solution, dried, and weighed
60
one of the most widely used gravimetric procedures is the determination of halides by the addition of ... to precipitate the ...
silver nitrate; silver halides

AP Chemistry (24 decks)

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