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chem yr 13 NI > acids > Flashcards

acids Flashcards

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1
Q

acid + metal

A

= salt + hydrogen

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2
Q

acid + metal oxide

A

=salt + water

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3
Q

acid + metal hydroxide

A

=salt + water

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4
Q

acid + metal carbonate

A

= salt + co2 + water

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5
Q

ammonia + hydrochloric acid =

A

NH4CL(aq)

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6
Q

type of acid used and salt formed

A

hydrochloric - chloride (cl-)
sulfuric - sulfate (SO42-)
nitric - nitrate (NO3-)
phosphoric - phosphate (PO43-)
ethanoic - ethanoate (CH3COO-)

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7
Q

definition of an acid

A

proton donor

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8
Q

monoprotic / diprotic

A

monoprotic acids release 1 H+
diprotic acids release 2 H+

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9
Q

definition of a base

A

a base is a proton acceptor
will accept and bind to H+

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10
Q

water

A

water can act as a base or an acid so amphoteric

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11
Q

strong acids

A

fully dissociates
equilibrium lies entirely to the right hand side
so if original conc of strong acid is x when it fully dissociates the conc of H+ will now be x

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11
Q

equation of PH

A

PH = -Log10[H+]

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11
Q

weak acids

A

partially dissociate
position of equilibrium is way over to the left hand side - cant work out concentration H+

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12
Q

examples of strong acids

A

HCl
H2SO4
HNO3
H3PO4

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13
Q

Ka

A

used to figure out amount of H+ ions that have partially dissociated
higher Ka - more dissociated

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14
Q

ka expression example
eg HCOOH(aq) <-> HCOO-(aq) +H+(aq)

A

Ka = [H+] [HCOO-] / [HCOOH]
[H+] = [HCOO-]
Ka = [H+] ^2 / [HCOOH]
rearrange to find [H+]

15
Q

PKa=

A

pKa = -Log10Ka

16
Q

Kw

A

Kw ionic product of water
alters with temp
Kw = [H+] [OH-] —– Kw = [H+]^2
grouped together as Kc and [H20] are constants

17
Q

pure water is neutral

A

[H+] = [OH-]

18
Q

Kw value at 298K

A

1x10-14

19
Q

water dissociation
Temp rise

A

forward reaction is endothermic
at temperatures of 298K the equilibrium shifts to the right to oppose the temperature rise
this means that [H+] increase

20
Q

strong bases

A

fully dissociate to release OH- ions
position of equilibrium lies entirely to the right hand side
USE KW
Kw=[H+][OH-]
[OH-] = conc of base as fully dissociates

21
Q

method for PH titrations

A

1-measure the PH of the acid solution and record
2-add 1cm3 of the base solution
3-stir the mixture
4-measure the ph and record
5-repeat the process until the base is in excess
6-add base in smaller increments near the end point

22
Q

why should you calibrate the ph meter

A

important to calibrate as after storage it may not give an accurate reading
to calibrate it you place the ph meter in a solution of known ph and then adjust the meter accordingly

23
Q

equivalence point

A

is when exactly enough acid has been added to neutralise the base
mid point on the vertical section of the graph

chem yr 13 NI (17 decks)

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