reactivity 3.1 Flashcards

1
Q

equation for calculating pH

A

– log₁₀[H⁺]

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2
Q

equation for calculating [H⁺]

A

10⁻ᴾᴴ

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3
Q

what defines an arrhenius acid?

A

a substance that disassociates in water to form hydrogen ions (H+) and anions

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4
Q

what defines an arrhenius base?

A

a substance that disassociates in water to form hydroxide ions (OH-) and cations

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5
Q

what does the bronsted-lowry theory focus on?

A

the transfer of H+ ions during an acid-base reaction (acids donate H+ while bases accept H+)

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6
Q

what is a bronsted-lowry acid?

A

a proton donor

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7
Q

what is a bronsted-lowry base?

A

a proton acceptor

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8
Q

define alkali

A

soluble bases which dissolve in water to release OH-

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9
Q

define amphiprotic

A

substances that can act as both bronsted-lowry acids and bases

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10
Q

requirement for a substance to be amphiprotic

A

must posses both a lone pair of electrons and hydrogen that can be released as H+

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11
Q

moving left to right across a period, oxides transition from ______ ______ oxides through ______ oxides then to ______ oxides

A

basic metal
amphiprotic
acidic

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12
Q

basic metal oxides react with an acid to form what?

A

a salt and water

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13
Q

non-metal oxides form ______ ______ in a solution

A

weak acids

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14
Q

amphiprotic oxides react with either an acid or a base to form what?

A

a salt and water

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15
Q

the burning of fossil fuels releases what 3 substances

A

GHG, nitrous oxides ans sulfuric oxides

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16
Q

what causes acid rain

A

increased emissions of nitrous oxides ans sulfuric oxides in the atmosphere, which turn rain water from its slightly acidic state (pH = 6) to become a stronger acid

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17
Q

where is acid rain’s negative effects seen? x3

A

structural materials, lakes/rivers & plant life/forests

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18
Q

what pH is acid rain?

A

pH = <5.6

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19
Q

what is the [H+] range (in numerical values) for the 0-14 pH scale?

A

1.0mol dm^-3 →10^-14 mol dm^-3

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20
Q

increasing pH by 1 = _______ [H+] by __ times

A

decrease, 10x

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21
Q

decreasing pH by 1 = _______ [H+] by __ times

A

increase, 10x

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22
Q

if the pH of a solution is changed from 3 to 5, how does the [H+] change?

A

pH = 3 => 10^-pH = 1 x 10^-3 mol dm^-3
pH = 5 => 10^-pH = 1 x 10^-5 mol dm^-3

[H+ ions] decreases by (1 x 10^-3 mol dm^-3)/(1 x 10^-5 mol dm^-3) = 100x times

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23
Q

what is the relationship between [H+] and [OH-]?

A

higher [H+] = lower [OH-]
lower [H+] = higher [OH-]

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24
Q

in terms of pH, what does a surplus of [H+] signify? what does a surplus of [OH-] signify?

A

surplus of [H+] = low pH = acidic
surplus of [OH-] = high pH = basic

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25
Q

pH’s neutral value = 7 at what temperature?

A

298K

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26
Q

how to find [H+] with value of [OH-]?

A

Kᵥᵥ / [OH-]

27
Q

how to find [OH-] with value of [H+]?

A

Kᵥᵥ / [H+]

28
Q

pH of pure water goes ____ as temperature goes ____

A

down, up

29
Q

despite changes in pH, why is water is still neutral?

A

[H+] = [OH-]

30
Q

characteristics of a strong acid x2

A

dissociates fully
good proton donors

31
Q

why do strong acids have weak conjugate bases?

A

because their reactions fo virtually to completion so they are not readily able to accept a proton

32
Q

characteristics of a weak acid x2

A

dissociates only partially
poor proton donors

33
Q

why do weaker acids have strong conjugate bases?

A

their dissociation reactions are equilibria that lies in favour of reactants, their CB are readily available to accept a proton

34
Q

acid dissociation reactions favour the production of a _______ conjugate. why?

A

weaker. better for strong acid to dissociate

35
Q

characteristics of a strong base x2

A

ionizes fully
good proton acceptors

36
Q

characteristics of a weak base x2

A

ionizes partially
poor proton acceptors

37
Q

base ionization reactions favours the production of the _____ conjugate

A

weaker

38
Q

strength of an acid or base is a measure of what?

A

how readily it dissociates/ionizes in aqueous solution (similar to solubility) to release H+/OH-

39
Q

strong acids x5

A

HCl
HBr
HI
HNO3
H2SO4

40
Q

strong bases x3

A

LiOH
NaOH
KOH

41
Q

weak acids x3

A

CH3COOH
H2CO3
H4PO4

42
Q

weak bases x2

A

NH3
C2H5NH2 (& other amines)

43
Q

as the halogen atom ______ in size going down group 17, the length of the H-halogen bond ________

A

increases, increases

44
Q

are longer bonds weaker or stronger? do they require more or less energy to break?

A

weaker, less

45
Q

acid strength of hydrogen halides _______ down the group

A

decreases
HF < HCl < HBr < HI

46
Q

electrical conductivity depends on the concentration of what?

A

mobile ions

47
Q

greater ionization in solution for strong acids & bases ⟹ _______ concentration of ions ⟹ ________ conductivity than weak acids and bases
(only if solutions of the same concentration are compared)

A

higher, higher

48
Q

neutralization reactions x2 products, exo or endo?

A

salt and water, exo

49
Q

when acids react with reactive metals, they also form salts as the hydrogen in the acid is replaced by the metal. why is there no transfer of a proton?

A

the hydrogen is released as H2 gas

50
Q

when acids react with reactive metals,
electrons as a product = what type of reaction?
electrons as a reactant = what type of reaction?

A

electrons as a product = oxidation
electrons as a reactant = reduction

51
Q

when acids react with reactive metals, why is the metal being ionized?

A

because H+ are becoming electrically neutral by accepting e- while the metal is being ionized by e- loss

52
Q

acid + carbonate → ___ + ___ + ___
2 examples of carbonates

A

salt, water, CO2 gas
metal carbonates (CO3^2-) and hydrogencarbonates (HCO3-)

53
Q

how to determine ionic/net ion equations

A

break up compounds, cancel out things shown on both sides of the reaction

54
Q

define effercescence

A

reactions involving a gas being given off so they visibly produce bubbles

55
Q

in neutralisation reactions, how is pure salt separated?

A

filtration followed by evaportation

56
Q

what is the net ion reaction for reactions between an acid and a base?

A

H+ (aq) + OH- (aq) → H2O (l)

57
Q

define spectator ions

A

other ions which do not change during the reaction and can be cancelled out

58
Q

why are neutralisation reactions exothermic?

A

because for every mole of H2O that forms, 2 moles of O-H bonds are made
bond making is exothermic, so overall it is an exothermic reaction

59
Q

what is the enthalpy of neutralisation reaction between all strong acids and strong bases? how is it expressed?

A

ΔH = -57 kJ mol^-1
expressed per mole of H2O formed

60
Q

define monoprotic acid

A

only has 1 H+ to give

61
Q

what point is reached when the acid and a base neutralise each other in a titration? x2 names

A

equivalence point OR stoichiometric point

62
Q

at the equivalence point of a strong acid and strong base titration, what does the solution contain?

A

water and salt

63
Q

how is the reaction ratio of acid to base to reach this point is determined by what?

A

the stoichiometry of the neutralisation reactions (mole ratios of acid to base reactants)

64
Q

review last page of r3.1 lesson 04 with volume of added base calculations

A

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