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Chem I Final Flashcards > Chapter 9 General Properties of Aqueous solutions > Flashcards

Chapter 9 General Properties of Aqueous solutions Flashcards

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1
Q

solution

A

a homogenous mixture

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2
Q

solute

A

the analyze of interest

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3
Q

solvent

A

the medium in which the solute is dissolved or dispersed

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4
Q

Aqueous solutions

A

a solution in which the water is the solvent

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5
Q

solubility

A

the maximum amount of substance that will dissolve into a solvent at a given temperature

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6
Q

saturated solution

A

a solution that contains the maximum amount of dissolve solid

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7
Q

electrolytes vs. non-electrolytes

A

once dissolved, different substances may behave differently and results in different types of solutions

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8
Q

electrolyte

A

substance that dissolve in water to form solutions that conduct electricity

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9
Q

non-electrolytes

A

substances that dissolve in water to form solutions that do not conduct electricity

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10
Q

electrolytes form ions there are two ways ion can be formed:

A

Dissociate: to separate, upon dissolving to form separate ions

ionize:the process in which a. molecular compound formed an ion

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11
Q

strong electrolytes

A

substances that dissociate or ionize completely

soluble salts, strong acids, strong bases

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12
Q

weak electrolytes

A

substances that partially dissociate or ionize

slightly soluble slats, weak acids, weak bases

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13
Q

conductivity

A

non-electrolytes: no ions-does not conduct electricity

molecular compounds(not acid/base)

strong electrolyte: lots of ions-conducts electricity very well

soluble salts

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14
Q

Soluble

A
  1. compounds containing an alkali metal cation(Li+,Na+,K+,Rb+,Cs+) or the ammonium ion(NH4+)
  2. compounds containing the nitrate ion(NO3-), acetate ion(C2H3O2-) or chlorate ion(ClO3-)
  3. compounds containing the chloride ion (Cl-), bromide ion(Br-), or iodide ion(I-)
    exceptions: compound that contains Ag+,Hg2^2+,Pb2+
  4. compounds containing the sulfate ion(SO4^2-)
    exceptions: compound that contains Ag+,Hg2^2+,Pb2+,Ca2+,Sr2+ or Ba2+
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15
Q

insoluble

A
  1. compounds containing the carbonate ion(CO3^2-) phosphate ion(PO4^3-) chromate ion(CrO4^2-) or sulfide ion(S2-)
    exception: Li+, Na+,K+,Rb+,Cs+ or NH4+
  2. compound containing the hydroxide ion (OH-)
    exception: Li+,Na+,K+,Rb+,Cs+,Ba+
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16
Q

molecular equation

A

the chemical equation that treats all species as molecules

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17
Q

total ionic equation

A

the chemical equation that explicitly shows the ions

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18
Q

spectator ion

A

ions that do not participate in the ration they appertains on both sides of the total ionic equation

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19
Q

acids

A

ability to dissolve metals. sour taste. turns litmus red

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20
Q

bases

A

slippery feel, bitter taste, turns litmus blue

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21
Q

acids

A

substances that contain H in the chemical formula and produces H+ ions when dissolved in water

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22
Q

bases

A

substances that contains OH in the chemical formula and produces OH- ion when dissolved in water

23
Q

Limitations

A
  1. restricts all acid-base reactions to water

2. excludes NHg and amines as bases

24
Q

acids

A

a proton donor

25
Q

bases

A

a proton acceptor

26
Q

Hydronium

A

H+ does not exist in the aqueous solution, in water, the H+ attaches to eater. H+ can be used for convenience, but it is H3O+

27
Q

Acid nomenclature

A

acidic compounds are named as acids if it is in solution. acids are named based on whether it contains oxygen or not.

no oxygen
hydro-anion-ic acid

with oxygen
anion acid
-ite anion-ous acid
-ate anion-ic acid

28
Q

polyphonic acid

A

acid with more than one ionizable proton

29
Q

monoprotic

A

acids with one ionizable proton

30
Q

diprotic

A

acids with two ionizable protons

31
Q

bronzed-lowry definition

A

proton accepts hydroxide compounds, metal oxides, ammonia ana amines

32
Q

strong acids

A

acids, that ionized completely

33
Q

strong bases

A

bases that ionize completely

34
Q

acid-base reactions

A

since acids are H+ donors and bases are H+ acceptors they are made to react together.

35
Q

Redox reactions

A

a chemical reaction in which electrons are transferred from one substance to another

36
Q

corrosion

A

the unwanted oxidation

4Fe + 3O2—>2Fe2O3

37
Q

combustion reactions

A

2C8H8+25O2—->16CO2+18H20

38
Q

metabolic process

A

C6H12O6+6O2—>6CO2+6H2O+ATP

39
Q

voltaic cells

A

batteries

Zn+MnO2+H2O—>ZnO+Mn(OH)2

40
Q

matallurgy

A

extraction of metals from ore

Fe2O3+3CO—>2Fe+3CO2

41
Q

oxidation states

A

the hypothetical charge an atom would have if all bonds were ionic

42
Q

rules for oxidation states

A
  1. the sum of the oxidation states must equal the net charge
  2. for lone elements the os=charge
  3. for ionic compounds, the charge of the ions are the os.
  4. in compounds a. F is alway -1 b. H is usually +1 c.O is usually -2
    except: hydride, peroxide’s, superoxides
43
Q

os

A

the hypothetical charge an atom would have if all bonds were ionic

44
Q

reduce agent

A

a substance that causes another compound to be reduced, therefore itself is oxidized

45
Q

oxidizing agent

A

a substance that cause another compound to be oxidized, therefore itself is reduced

46
Q

Concentration of solutions

A

the amount of solute in solution can vary. one way of expressing this amount is through the unit of molarity

Molarity, M: amount of solute, mol/ volume of solution L

47
Q

Dilutions

A

C1V1=C2V2. M1V1=M2V2
C1:mol/L
V1: L=mol initially

the amount of solute does not change when a solvent is added to dilute the solutions. but since the volume of solutions increases the concentration must decrease

48
Q

pH scale

A

in many applications the concentration of H+ ions is important often the concentration is small.

pH=-log[H+]

49
Q

auto ionization of water

A

process is driven by hydrogen bonding

50
Q

Gravimetric analysis

A

analytical technique based on masses requires reactions to be completed

51
Q

tritration

A

an analytical technique for precisely determine the concentration or amount of solute in a sample by reacting it with a standard of known concentration

52
Q

equivalence point

A

the point in the titration in which the number of moles of titrant and moles of analyze are in stoichiometric equivalence

53
Q

end point

A

the point in the titration in which the indicator changes color indicating the stoppage of the titration

Chem I Final Flashcards (11 decks)

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