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chem 10 > quiz 8 > Flashcards

quiz 8 Flashcards

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1
Q

molarity equation

A

moles (of solute)/liters (of solution)

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2
Q

dilution equation

A

M1V1=M2V2

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3
Q

arrhenius definition of acids

A

chemicals that increase the concentration of H+ (protons)

ex: HCl

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4
Q

arrhenius definition of bases

A

chemicals that increase the concentration of OH-

ex: NaOH

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5
Q

a solution is acidic if

A

it has more moles of acid than base, which means its pH is less than 7

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6
Q

a solution is basic if

A

it has more moles of base than acid, which means its pH is greater than 7

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7
Q

a solution is neutral if

A

it has an equal number of moles of acid and moles of base, meaning that its pH is exactly 7

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8
Q

bronsted-lowry definition of acids

A

chemicals that donate protons, AKA proton donors

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9
Q

bronsted-lowry definition of bases

A

chemicals that accept protons, AKA proton acceptors

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10
Q

H+ vs H3O+

A

they mean the same thing

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11
Q

strong acids

A
  • fully disassociate (separate) into their component ions, aka complete ionization
  • are strong electrolytes
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12
Q

weak acids

A
  • do not fully disassociate (separate) into their component ions
  • are weak electrolytes
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13
Q

strong bases

A

full disassociate (separate) into their component ions, AKA complete ionization

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14
Q

weak bases

A

-do not fully disassociate (separate) into their component ions

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15
Q

true or false, water reacts with itself in an acid-base reaction

A

true, this is self-ionization

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16
Q

value of [H3O+] and [OH-] in pure water

A

both 10^-7 M

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17
Q

diprotic acids

A
  • are acids that contain two acidic protons (ex H2SO4 has 2 H+, AKA acidic protons)
  • every 1 mole of diprotic acid can react with 2 moles of OH- instead of just one
  • similarly, acids with three acidic protons (ex H3PO4) can react as 1 mole of acid to 3 moles of OH-
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18
Q

buffer solution

A
  • resists change in pH and keeps pH level constant

- is created by making a solution where moles of weak acid and moles of conjugate base are present in 1 to 1 ratio

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19
Q

conjugate base

A
  • on the reactants side

- is the acid after donating a proton, thus becoming a base itself

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20
Q

conjugate acid

A
  • on the reactants side

- is the base after accepting a proton, thus becoming an acid

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21
Q

how to use a burette

A

amount dispensed = final volume - initial volume

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22
Q

titrant

A
  • what goes into the buret for titration

- concentration is always known

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23
Q

analyte

A

what is in the beaker during titration

-concentration is always unknown, to be determined from the titration experiment

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24
Q

phenolphthalein

A
  • an acid-base indicator
  • turns pink in basic solution
  • goes into the analyte solution
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25
Q

once a reversible reaction reaches equilibrium, what happens to the rate of the forward reaction and rate of reverse reaction?

A

they become equal

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26
Q

once a reversible reaction reaches equilibrium, what happens to the concentration of reactants and products?

A
  • both concentrations become stable

- but [reactants] does not always equal [products]

27
Q

in a reversible reaction, when is the rate for the forward reaction the fastest and slowest?

A
  • fastest at the very beginning

- slowest at equilibrium

28
Q

when is the rate for the reverse reaction the fastest?

A

-at equilibrium

29
Q

equilibrium can only be achieved when

A
  1. the reaction is reversible
  2. the reaction takes place in a closed system
  3. none of the chemical compounds precipitate as a solid
30
Q

equilibrium constant

A
  • Keq=[products]/[reactants]=([C]^c[D]^d)/([A]^a[B]^b) when aA + bB cC + dD (lowercase are coefficients, uppercase are reactants/products)
  • only take the concentrations of aq solutions and gases, and exclude solids and liquids
31
Q

at what Keq does the reaction become irreversible?

A
  • at Keq>10^10

- this means that it’s 0% reactant, 100% product

32
Q

at what Keq does the reaction become NO reaction?

A

at Keq<10^-10

-this means that it’s 100% reactant, 0% product

33
Q

le chatelier’s principle

A

when a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance

34
Q

ways to disturb an equilibrium

A
  1. change the concentration of one of the chemicals involved
  2. change the temperature
  3. change the volume of the system
35
Q

what change in concentration would make a system shift to the left?

A
  • adding product

- removing reactant

36
Q

what change in concentration would make a system shift to the right?

A
  • adding reactant

- removing product

37
Q

what change in temperature would shift a system to the left?

A
  • adding energy to an exothermic reaction

- removing energy from an endothermic reaction

38
Q

what change in temperature would shift a system to the right?

A
  • adding energy to an endothermic reaction

- removing energy from an exothermic reaction

39
Q

when volume is decreased in an equilibrium system,

A

reaction wants to shrink, and therefor shifts to the side with less volume

40
Q

when volume is increased in an equilibrium system,

A

reaction wants to expand, and therefor shifts to the side with more volume

41
Q

why do combustion reactions not immediately occur (without the assistance of energy)?

A

because all reactions have a required activation energy/barrier

42
Q

how to overcome the activation energy/barrier

A

either

  • raise the temperature
  • use a catalyst
43
Q

a catalyst

A

lowers the height of the activation barrier/energy

44
Q

enzymes

A

are biological catalysts

45
Q

pH

A
  • a way to express the concentration of H30+
  • pH less than 7 is acidic
  • pH of 7 is pure water
  • pH greater than 7 is basic
46
Q

when calculating pH

A
  • the SF in [H3O+] is the # of decimal places for your pH level
  • in reverse, the # of DP in your pH level gives you the # of SF in your concentration
47
Q

list of strong acids

A
  • HCl
  • HBr
  • HI
  • HClO4
  • HNO3
  • H2SO4
48
Q

list of weak acids

A

-HF
-HC2H3O2
-H2CO2
-H2CO3
-H2SO3
H3PO4

49
Q

list of strong bases

A

anything that contains OH and is soluble

50
Q

list of weak bases

A
  • NH3
  • C5H5N
  • CH3NH2
  • CH3CH2NH2
  • HCO3-
51
Q

oxidation state of elemental compound

A

always zero

52
Q

oxidation state of ion

A

equal to its charge

53
Q

relationship between sum of oxidation states and net charge of a molecule

A

they are equal

ex: h20 net charge is 0, and sum of its oxidation states is 0

54
Q

oxidation state of alkali metals

A

+1

55
Q

oxidation state of group alkaline earth metals

A

+2

56
Q

oxidation state of fluorine

A

-1

57
Q

oxidation state of hydrogen

A

+1, with exceptions like LiH, NaH, CaH2 (oxidation state of group 1 & 2 metals take precedent)

58
Q

oxidation state of oxygen

A

-2

59
Q

oxidation state of halides

A

-1

60
Q

oxidation state of sulfur and its group members

A

-2

61
Q

oxidation state of nitrogen and its group members

A

-3

62
Q

order of precedence for H, O, F oxidation states

A

FHO

63
Q

mnemonic for oxidation and reduction

A

LEO the lion goes GER
LEO: Loss of Electrons is Oxidation
GER: Gain of Electrons is Reduction

64
Q

half reaction method

A

write out net ionic equation, then separate into reduction half reaction and oxidation half reaction and add electrons to each accordingly. then (if necessary) multiply each by an integer to make the # of electrons on each side of the “complete” reaction equal

chem 10 (11 decks)

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