acids and bases Flashcards

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1
Q

bronsted acid

A

proton donor

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2
Q

strong acid

A

acid which ionises almost completely in an aqueous soln
eqm very far right
large Ka
HNO3, HCL,H2SO4

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3
Q

bronsted base

A

proton acceptor

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4
Q

weak acid

A

acid that only ionises partially in an aqueous soln
eqm lies far left
small ka

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5
Q

ionisation

A

reaction of a molecular substance with water to produce ions

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6
Q

dissociation

A

splitting of an ionic compound into its ions

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7
Q

polyprotic acids

A

able to donate more than one proton

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8
Q

dilute acid

A

small no. of moles in acid

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9
Q

strong base

A

base that dissociates almost completely in an aqueous soln
high Kb value
group 1 hydroxides

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10
Q

weak base

A

base that ionises partially in an aqueous soln
low Kb value

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11
Q

test for strong or weak base

A

conductivity

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12
Q

test for strong or weak base

A

conductivity

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13
Q

strength of an acid/base

A

independent of concentration of soln

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14
Q

concentrated acid/base

A

contains very large amount of acid/base than water in soln
has relatively more dissolved solute than a dilute soln

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15
Q

conjugate base pairs

A

1 product and 1 reactant, 1 H+ difference
stronger an acid/base- weaker its conjugate

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16
Q

conjugate base

A

substance formed when acid loses 1 proton

17
Q

conjugate acid

A

substance formed when base gains one 1 proton

18
Q

amphoterrpic/amphiprotic substance

A

substance that can act as either an acid or a base
H2O (water) , HCO3- (hydrocarbonate), HSO3- (hydrogen sulphate)

19
Q

autoprolysis

A

auto-ionisation of water
self ionises to extremely limited extent
concentration of ions extremely low- eqm far left

20
Q

Kw

A

1x10^-14 @25 degrees celcius

21
Q

pH scale

A

measure of hydronium concentration in soln @25 degrees celcius

= -log[H3O+]
high number-low pH
small number-high pH

22
Q

hydrolysis

A

reaction of an anion( from a salt) with water
occurs when salt of weak acid/base/both is dissolved in water causing water itself to decompose in rxn w ions of the salt
salt breaks down into pos + neg ions
water undergoes autoprolysis
conjugate ions of strong acids/bases and group 1 metals do NOT undergo hydrolysis

23
Q

neutralisation

A

a chemical reaction in which an acid + a base react so that neither is in excess
forms salt and water
equivalence point should be the same as end point if done correctly.

24
Q

standard solution

A

solution of known concentration

25
Q

standard solution

A

solution of known concentration

26
Q

acid-base titrations

A

acidic soln of known concentration added from a burette to a conical flask containing basic soln of unknwon concentration or vice versa, until end point is reached (indicator changes colour)
unknown concentration is calculated from readings from burrette
CHECK - titration point and equivalence point must be same

27
Q

salt

A

substance in which the hydrogen of an acid has been replaced by a cation

28
Q

salt

A

substance in which the hydrogen of an acid has been replaced by a cation

29
Q

smaller Kb

A

weaker base

30
Q

larger kb

A

stronger base

31
Q

conjugate base

A

substance formed when acid loses 1 proton

32
Q

conjugate base

A

substance formed when acid loses 1 proton

33
Q

conjugate acid

A

substance formed when base gains 1 proton

34
Q

neutral salt

A

made of strong acid + strong base
complete dissociation + ionisation
no hydrolysis will occur
no disruption to equal concentration of H3O+ and OH- ions in soln
salt has pH of 7

35
Q

acidic salt

A

strong acid + weak base
acid ions will not undergo hydrolysis (conjugate of strong acid)
base undergoes hydrolysis forms product of weak base which will not dissociate complete
the formation of the weak base removes OH- ions from water
disruption to concentration of OH- and H3O+ ions in soln
water equilibrium shifts right to replace (OH-)
therefore the concentration of H3O+ ions increases
hence the salt is acidic , and the pH is less than 7

36
Q

basic salt

A

weak acid + strong base
base does not undergo hydrolysis (dissociates completely)
therefore weak acid undergoes hydrolysis
product formed is a weak acid (won’t ionise completely)
formation of weak acid removes H+ ions , thus leading to a disruption in the concentration of H3O+ and OH- in soln.
The water equilibrium shifts right to replace H3O+ ions resulting in an increase in the concentration of [OH- ions]
therefore salt is basic , pH is larger than 7

37
Q

acid-base titrations

A

titration - volumetric analysis
acidic solution of non-concentration ( standard solution) is added from a burette to a conical flask (containing basic solution of undone concentration measured in pipette in fixed volume) vice versa until endpoint is reached (indicator changes colour)
unknown [ ] is calculated from readings from burette
CHECK: titration end point should = equivalence point

38
Q

equivalence point vs end point

A

equivalence- point in a titration where neither reactant is in excess
end point / point where indicator changes colour

39
Q

acid + metal

A

salt + H2(g)
redox rxn