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chemistry > C5 - salts and bases > Flashcards

C5 - salts and bases Flashcards

1
Q

why are group 1 metals different to most metals

A

as they react vigorously with water, giving off hydrogen and leave an alkali solution

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2
Q

why does magnesium lie between between lithium and copper in the reactivity series

A

as if you leave magnesium in a beaker of water it would take several days for it to collect enough gas to react

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3
Q

how does sodium potassium lithium and calcium react with water

A

fizzes, hydrogen is produced leaving an alkali solution with metal hydroxide

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4
Q

how does magnesium aluminium zinc and iron react with water

A

very slow reaction

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5
Q

how does tin and lead react with water

A

slight reaction with steam

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6
Q

how does copper silver and gold react with water

A

no reaction

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7
Q

what elements produces no reaction in water

A

copper silver and gold

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8
Q

what elements produces a slight reaction with steam in water

A

tin and lead

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9
Q

what elements produces a very slow reaction in water

A

magnesium aluminium zinc and iron

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10
Q

what elements produces fizzes and hydrogen gas leaving an alkaline solution of metal hydroxide in water

A

potassium sodium lithium and calcium

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11
Q

what elements produces an explosion in dilute acid

A

potassium sodium and lithium

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12
Q

what elements produces fizzing, hydrogen gas and a salt in dilute acid

A

magnesium aluminium calcium zinc and iron

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13
Q

what elements react slowly with warm acid in dilute acid

A

tin and lead

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14
Q

what elements produces no reaction in dilute acid

A

copper silver and gold

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15
Q

how does potassium sodium and lithium react in dilute acid

A

explode

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16
Q

how does magnesium calcium aluminium zinc and iron react in dilute acid

A

fizz, produces hydrogen gas and forms a salt

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17
Q

how does tin and lead react in dilute acid

A

react slowly with warm acid

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18
Q

how does copper silver and gold react in dilute acid

A

no reaction

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19
Q

what is the rule for displacement

A

a more reactive metal will displace a less reactive metal from an aqueous solution of one of its salts

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20
Q

what is carbon used for

A

it is used in the extraction of metal oxides by heating but can only do this for metals below aluminium in the reactivity series

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21
Q

what are metal ores found as

A

metal oxides or as compounds that can be changed into metal oxides

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22
Q

what products are formed when a iron oxide reacts with carbon

A

it forms iron + carbon dioxide

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23
Q

where are unreactive metals found

A

in the earths surface

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24
Q

how are unreactive metals found

A

they are found in the earth as metals so they exist in their native state

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25
what is a metal ore
naturally occurring rocks that contain metals or metal compounds in sufficient amounts to make it worth to extracting
26
what factors does extracting a metal ore depend on
- how easy it is to extract - how much metal it contains - the changing demands for the particular metal
27
how can the factors of extracting a metal ore change
- you might find a new way to extract a metal efficiently - you might find a cheaper way to extract metals
28
how is carbon used in industries
- carbon is used to extract some metal from their ores in industries
29
why is hydrogen used to extract tungsten from its oxide instead of carbon
as carbon forms the compound tungsten carbide with the metal by reduction
30
how are metal ore extracted
by electrolysis
31
what happens when a reaction between a metal and acid take place
it produces salt and hydrogen
32
what is a salt
a salt is the name for a compound formed when the hydrogen in an acid is replaced or partially replaced by metal ions
33
how are pure dry crystals of a salt solution obtained
- when some of the water is evaporated from the solution by heating until the point of crystallisation is reached - at this point the solution is saturated and crystals will appear at the edge of the salt solution in the evaporating dish
34
how to test for crystals
dip the glass rod into the hot salt solution the removing it and seeing if crystals form on the glass rod when it cools down
35
how can you obtain the best samples of crystals
- leave the salt solution at room temperature for the remaining water to evaporate slowly - you can remove any solution left on the crystals by patting it dry with a paper towl of filter paper
36
what salt is formed when you react metals with hydrochloric acid
chloride salts
37
what salt is formed when you react metals with nitric acid
nitrate salts
38
what salt is formed when you react metals with sulfuric acid
sulfates
39
what is a spectator ion
an ion that does not change during the reaction
40
in a reaction between metals and acids which one donated the electrons to the other
metals
41
what are bases
bases are compounds that can neutralise acids
42
what products are are formed acids and base
salt and water
43
what are salts made from
positive ions from a metal base or carbonate and negative ions from acids
44
what products are form from carbonate and acid
salt and water and CO2
45
charge of an aluminium ion
3+
46
charge of ammonium ion
1+
47
charge of nitrate ion
1-
48
charge of sulfate ion
2-
49
why isn't copper used for making copper sulfate
as copper is not reactive enough to form copper sulfate
50
method of copper sulfate REQUIRED PRACTICAL
1) start with a fixed volume of dilute sulfuric acid, this is our limiting reactant as we have to make sure all the acid is reacted as any remaining acid can contaminate our results 2) gently heat the acid until it almost boils as if we boil it would bubble over which is dangerous 3) using a spatula we add small amounts of copper oxide to the acid then stir it using a glass rod 4) the copper oxide will react and seem to disappear and the solution will will turn blue which is the colour of copper sulfate 5) continue to add copper oxide when the solution is blue until the powder remains after stirring at this point the reaction has stopped and all the acid has reacted meaning that we have mad copper sulfate and that the solution is neutral
51
method for copper sulfate crystals REQUIRED PRACTICAL
1) filter the unreacted copper oxide using filter paper and a filter funnel 2) put the copper solution into the evaporation basin and heat it gently over a beaker of boiling water and keep heating it until half the solution remains 3) leave the solution for 24hr in a cool place for crystals to form and finally we place the copper crystals onto a paper towel and pat and dry them
52
what products do acids and alkalis make
salt and water
53
how can we tell when an acid has fully reacted with an alkaline
titration
54
how to get pure dry crystals from acids and alkaline
- carry out titration with the indicator added to see how much acid reacts completely with the alkali - run the volume of acid into the solution without the indicator - crystallise and dry the crystals from the reaction mixture
55
what are alkalis
soluble hydroxides
56
properties of all acids
- they taste sour
57
what pH is water
7 (its neutral)
58
what do acids release when added to water
Hydrogen ions
59
what do alkalis release when added to water
aqueous hydroxide ions
60
what makes solutions alkaline
when there is excess OH ions in the solution
61
what can we use to test the pH
- universal indicator - pH meter - electric pH sensors which give a digital display of pH to test pH
62
what does the concentration of an acid tells us
the amount of acid molecules in a given solution
63
what does a dilute acid contain
few acid molecules in a given volume than a concentrated acid even if the strength of the acid is the same
64
examples of strong acids
- hydrochloric acid - nitric acid - sulfuric acid
65
examples of weak acids
- ethanoic acid - citric acid - carbonic acid
66
what is the rate of carbon dioxide released when a metal carbonate reacts with carboxylic acid and what does this mean
carbon dioxide is given off more slowly when it reacts metal carbonate with carboxylic acid (ethanoic acid) compared to when hydrochloric acid reactants with metal carbonate this mean that carboxylic acids are weak acids
67
why must acids dissolve in water before they show their acidic properties
as in water all ionise (split up) to form hydrogen ions and negative ions
68
why are strong acids strong and weak acids weak
as strong acids ionise completely whilst in weak acids most of the molecules stay as they are and dont release hydrogen ions into the the solution
69
how are the reactions with weak acids reversible
as the molecules of weak acids split up to form hydrogen ions and negative ions and the ions can recombine to form the orignal molecule
70
why do strong acids have a lower pH value than weak acids
as they fully ionise producing a greater concentration of hydrogen ions than weaker acids
71
rule for pH value
as the pH scale decreases by 1 unit the concentration of hydrogen ions increase by 10 times
72
do strong acids have a high or low pH value
low
73
when do acids produce hydrogen ions
when in aqueous solutions
74
what happens to molecules in aqueous solution
the ionise (split) and release hydrogen ions
75
The particular salt produced in any reaction between an acid and a base or alkali depends on what
the acid used the positive ions in the base, alkali or carbonate
76
how are soluble salts made
Soluble salts can be made from acids by reacting them with solid insoluble substances, such as metals, The solid is added to the acid until no more reacts and the excess solid is filtered off to produce a solution of the salt.
77
half equation for neutralisation reaction to produce water
H (+) + 0H(-) ----------------------> H20

chemistry (13 decks)

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