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ap chemistry > chapter 4: Chemical Reactions in Solution > Flashcards

chapter 4: Chemical Reactions in Solution Flashcards

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AP® Chemistry flashcards Periodic Table 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
Q

overall equation: shows all of the reactants and products in

A

undissociated form

26
Q

complete ionic equation: more … description; an equation in which strong electrolytes are shown as … in the solution

A

accurate; ions

27
Q

complete ionic equation represents the species as tey

A

exist in solution

28
Q

spectator ions: do not participate in any

A

chemical achange

29
Q

net ionic equation: shows only those species in the solution that actually

A

undergo a chemical change

30
Q

net ionic equations are useful in writing …

A

acid-base reactions

31
Q

water is not present as …, can be written as a product in a …

A

ions; net ionic equation

32
Q

concentration of a solution: the amount of … in a given quantity of that …

A

solute; solution

33
Q

molarity: number of … of solute per … of solution

A

moles; liter

34
Q

molarity is a measure of

A

concentration

35
Q

molarity is based on the … olume fo solution, not on the volume of …

A

volume; added solvent

36
Q

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 …

A

volumetric flask; graduated sylinder; solvent; dissolve; solvent; achieved

37
Q

solutions of known molarity can be prepared from a weighted sample dissolved in a solvent, then … to a known volume of solution

A

diluted

38
Q

the molarity of a solution provides the … that converts between …. and …

A

relation; volume of solution; moles of solute

39
Q

it is common to use square brackets around a species to imply

A

concentration of this species in units of molarity

40
Q

less .. solutions are often prepared from more … stock solutions

A

concentrated; highly concentrated

41
Q

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 …

A

volume; mass of the solute

42
Q

pipet: a calibrated device designed to deliver an …. of liquid with …

A

accurately known volume; high precision

43
Q

m1v1=

A

m2v2

44
Q

dilution of a given amount of a concentrated solution does not change the number of

A

moles of solute

45
Q

the moles of solute in the concentrated solution are the same as in th

A

dilute solution

46
Q

the only difference between the two solutions is tha tmore solvent is present in th

A

dilute solution

47
Q

m1v1=m2v2 cannot be used for problems involving

A

chemical reactions

48
Q

solution stoichiomtry equations are similar to ch 3 problems, but the amounts are calculated from the … of solutions of known … rather than from …

A

volumes; concentrations; masses

49
Q

titration: a procedure to determine the … of one substance by adding a measured amount of a ….

A

quantity; second substance

50
Q

equivalence point: the point at which stoichiometrically … of the two reactants are present

A

equivalent amounts

51
Q

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

A

given amount; concentration; base; acid; neutralize

52
Q

indicators are used to detect the … in acid-base titrations

A

equivalence point

53
Q

an indicator is a compound that changes …as an … solution becomes … or vice versa

A

color; acidic; basic

54
Q

the point at which the indicator … color is called the ….

A

changes; end point

55
Q

a standard solution is a solution with an accurately known

A

concentration

56
Q

volumetric analysis: a chemical analysis that involves measurement of the … of a … or …

A

volume; solution; substance

57
Q

a … is chosen to standardize an acid

A

high-purity base

58
Q

a precipitation reaction can be used to isolate a … from a solution

A

desired ion

59
Q

gravimetric analysis is a procedure in which one component of a solution is selectively

A

precipitated, separated from solution, dried, and weighed

60
Q

one of the most widely used gravimetric procedures is the determination of halides by the addition of … to precipitate the …

A

silver nitrate; silver halides

ap chemistry (24 decks)

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