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Chemistry: Paper 1 > Chemical Changes > Flashcards

Chemical Changes Flashcards

(56 cards)

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1
Q

What do acids produce in aqueous solution

A

H+ ions

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2
Q

What do alkaline produce in aqueous solution

A

OH- ions

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3
Q

What is the pH of a neutral solution

A

7

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4
Q

What is the pH of an alkaline solution

A

more than 7 (stops before 14)

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5
Q

What is the pH of a acidic solution

A

less than six (stops at 0)

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6
Q

What does acids and alkaline do to phenolphthalein indicator

A

Acids = colourless
Alkaline = Pink

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7
Q

What does acids and alkaline do to methyl orange indicator

A

Acidic = red
Alkaline = yellow

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8
Q

What does acids and alkaline do to litmus solution

A

Acidic = red
Alkaline = blue

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9
Q

What colour does blue litmus paper go in acids and alkaline

A

Acid = turns red
Alkaline = stays blue

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10
Q

What colour does red litmus paper go in acids and alkaline

A

Acid = stays red
Alkaline = turns blue

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11
Q

What do acids with a lower pH have

A

A higher concentration of H+ ions

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12
Q

What do alkaline with a higher pH have

A

A higher concentration of OH- ions

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13
Q

What does a pH of 1 represent

A

Hydrogen ion concentration of 0.1mol/dm^3

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14
Q

What happens as you increase the pH by 1

A

you decrease the H+ ion concentration by 10

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15
Q

Derive a test to measure the change in pH

A
  1. Add dilute HCL into beaker and measure the pH
  2. Add a weighed mass of Calcium hydroxide and stir
  3. Record new pH
  4. Repeat and measure the change of acidity
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16
Q

Define a strong acid

A

fully dissociates in aqueous solution

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17
Q

Define a weak acid

A

partially dissociates in aqueous solution

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18
Q

State the neutralisation equation

A

acid + base -> salt + water
HCL + NaOH -> NaCl + H20

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19
Q

what is the general equation for a metal

A

acid + metal → salt + hydrogen gas (H2)

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20
Q

what is the general equation for a metal oxide

A

acid + metal oxide → salt + water

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21
Q

what is the general equation for a metal hydroxide

A

acid + metal hydroxide → salt + water

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22
Q

what is the general equation for a metal carbonate

A

acid + metal carbonate → salt + water + carbon dioxide (CO2)

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23
Q

What is the test for hydrogen

Study These Flashcards
A

Place burning splint held at the open end of a test tube of the gas - should create a ‘squeaky pop’ sound

24
Q

What is the test for carbon dioxide

Study These Flashcards
A

Bubble the gas through limewater
Will turn milky/ cloudy

25
What is the ionic equation for neutralisation
H+ (aq) + OH- (aq) = H2O (l)
26
How is a soluble salt made
Mixing of a acid and insoluble base
27
Why is the insoluble reactant added in excess when preparing a soluble salt
To ensure all the acid has reacted
28
How is excess reactant removed from a soluble salt
filtration - leaves behind salt and water
29
Why is titration used when make soluble salts with an acid and soluble reactant (3 points)
1-solutions are soluble excess cannot easily be removed 2- Titrations provide exact proportions 3- Everything will neutralsises except salt and water
30
Core practical: derive a method to prepare copper sulphate crystals (3 steps)
1- add an excess of copper oxide to sulphuric acid 2- filter off any copper oxide that hasn't reacted 3- evaporate off the water by placing final solution in a water bath
31
Describe how to carry out an acid-alkali titration resulting in crystals to form (6 steps)
1. Wash burette using the acid and then water 2. Fill burette to 100cm3 with acid 3. Use a pipette to add 25cm3 of alkali into a conical flask 4. Add a few drops of a suitable indicator to the conical flask 5. Add acid from burette to alkali until end-point is reached 6- warm the salt solution to evaporate the water
32
What are concordant titres
Titres within 0.10 cm^3 of each other
33
What solutions are ALWAYS soluble (6 groups)
N- Nitrates A- Acetates G- Group 1 S- Sulfates A- Ammonium G- Group 17
34
Which group 17 elements are not soluble (name 3)
1. Lead 2. Mercury 3. Silver
35
Which sulphates are not soluble (name 3)
1- Calcium 2- Strontium 3- Barium
36
What are the ONLY soluble carbonates/hydroxides (name 3)
1- sodium 2- potassium 3- ammonium
37
What do insoluble salts form as
Precipitate
38
Describe how you produce a pure, dry sample of a soluble salt
1. mix the two solutions needed to form the salt 2. filter the mixture using filter paper, which the insoluble salt will be left on 3. place on a water bath, and heat until about half the water from the solution has been removed by evaporation. 4. leave for small cystals to start forming around the edge of the evaporating basin.
39
What are electrolytes
Ionic compounds that are dissolved or in molten state so that ions are free to move
40
What is electrolysis
The use of electricity to break down electrolytes to form elements
41
Describe the movement of ions in electrolysis
Cations move towards the Cathode Anions move towards the Anode
42
What is the name of the positive electrode where oxidation occurs
Anode
43
What is the name of the negative electrode where reduction occurs
Cathode
44
What ions are in aqueous solutions when separated
Ions that make up the ionic compound Ions that found in water ( H+ and OH- )
45
What is the rule for the discharge of ions at the cathode in aqueous solutions
The ion of the least reactive element will be discharged
46
What is the rule for the discharge of ions at the anode in aqueous solutions
OH- ions are always discharged unless a halide is present
47
What happens at the electrolysis of Copper chloride
- Cu+ go to the cathode 🡲 Cu (s) produced - Cl- ions go to the anode 🡲 Cl2 (g) produced
48
What happens at the electrolysis of sodium chloride
H+ ions go to cathode 🡲 H2 (g) produced Cl- ions go to anode 🡲 Cl2 (g) produced
49
What happens at the electrolysis of sodium sulphate
H+ ions go to cathode 🡲 H2 (g) produced OH- ions go to anode 🡲O2 (g) produced
50
What happens at the electrolysis of water acidified with sulfuric acid
H+ to cathode 🡲 H2 (g) is produced OH- to anode 🡲 O2 (g) is produced
51
What happens at the electrolysis of molten lead bromide
Pb2+ to cathode 🡲 Pb (s) produced Br- to anode 🡲 Br2 (l) produced
52
What is oxidation and reduction in terms of electrons
Oxidation Is Loss Reduction Is Gain
53
How is electrolysis used to purify copper
Anode is impure copper Cathode is pure copper Solution is copper sulfate Cu2+ ions from anode more to cathode 🡲 gain electrons 🡲 discharged as pure copper Impurities form as sludge below the anode
54
Investigate the electrolysis of copper sulphate with inert electrodes
Cu (s) produced at cathode O2 (g) produced at anode H+ and SO4^2- ions left in solution react to form sulfuric acid
55
What is the ionic half equation for reactions at the negative electrode (reduction)
Gains an elecron so: (X+) + e- 🡲 X
56
What is the ionic half equation for reactions at the positive electrode (oxidation)
(X-) 🡲 (e-) + X

Chemistry: Paper 1 (5 decks)

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