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Chemistry Yr 10 > Chemical Changes > Flashcards

Chemical Changes Flashcards

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1
Q

What is an acid in terms of pH and ions released?

A

An acid has a pH less than 7. Acids release H⁺ ions in aqueous solution.

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2
Q

What is a base?

A

A base is a substance that reacts with an acid to form only a salt and water.

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3
Q

What is an alkali?

A

An alkali is a base that dissolves in water. Alkalis release OH⁻ ions in aqueous solution.

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4
Q

What is neutralisation?

A

Neutralisation is a reaction between an acid and a base, forming a salt and water.

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5
Q

What is a precipitate?

A

An insoluble solid formed when two solutions react together.

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6
Q

How can you make an insoluble salt using precipitation?

A

Mix two solutions containing ions that will form an insoluble salt. Filter the mixture to collect the precipitate. Wash and dry the precipitate.

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7
Q

Name three soluble salts and the ions they contain.

A

Sodium, potassium, and ammonium salts are soluble in water. Nitrates are soluble. Most chlorides are soluble (except silver and lead(II)). Most sulfates are soluble (except lead(II), barium, and calcium).

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8
Q

Name some common insoluble salts.

A

Most carbonates and hydroxides (except those of sodium, potassium, and ammonium). Lead(II) chloride, barium sulfate.

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9
Q

How can you make a soluble salt from an acid and a base?

A

Add excess insoluble base (e.g., copper oxide) to warm acid. Filter to remove excess base. Heat the filtrate to crystallise the salt. Leave to dry.

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10
Q

What is the importance of using excess base in this reaction?

A

To ensure all acid reacts and is neutralised, avoiding a contaminated product.

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11
Q

What is a strong acid?

A

A strong acid fully dissociates (ionises) in solution, releasing all H⁺ ions.

Examples: Hydrochloric acid, sulfuric acid, nitric acid.

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12
Q

What is a weak acid?

A

A weak acid only partially dissociates in solution.

Examples: Ethanoic acid, citric acid, carbonic acid.

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13
Q

How does pH relate to hydrogen ion concentration?

A

Every decrease of 1 on the pH scale represents a 10× increase in H⁺ ion concentration.

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14
Q

What is the general equation for acid + metal?

A

Acid + Metal → Salt + Hydrogen

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15
Q

What is the general equation for acid + metal oxide or hydroxide?

A

Acid + Metal oxide/hydroxide → Salt + Water

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16
Q

What is the general equation for acid + carbonate?

A

Acid + Metal carbonate → Salt + Water + Carbon dioxide

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17
Q

What are the products of neutralisation?

A

Salt and water

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18
Q

What is the ionic equation for neutralisation?

A

H⁺(aq) + OH⁻(aq) → H₂O(l)

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19
Q

Why are neutralisation reactions important in daily life?

A

Treating indigestion (antacids). Adjusting soil pH. Waste water treatment.

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20
Q

What is electrolysis?

A

Electrolysis is the breakdown of an ionic compound using electricity.

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21
Q

When can electrolysis occur?

A

When the ionic compound is molten or dissolved in water (so ions can move).

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22
Q

What is an electrolyte?

A

A liquid that conducts electricity and is broken down during electrolysis.

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23
Q

What happens at the electrodes?

Study These Flashcards
A

Positive ions move to the cathode (gain electrons – reduction). Negative ions move to the anode (lose electrons – oxidation).

24
Q

How is the product at the cathode determined in electrolysis of aqueous solutions?

Study These Flashcards
A

If metal is more reactive than hydrogen, hydrogen gas forms. If metal is less reactive, the metal is deposited.

25
What happens at the anode in aqueous solutions?
If halide ions are present: halogen is formed. If no halide ions: oxygen is formed from OH⁻ ions.
26
What happens during the electrolysis of copper sulfate with carbon electrodes?
Copper metal forms at the cathode. Oxygen gas forms at the anode.
27
What happens during the electrolysis of copper sulfate with copper electrodes?
Anode loses mass as copper atoms become Cu²⁺ ions. Cathode gains mass as Cu²⁺ ions are reduced to copper.
28
(Six Marker) Describe how to investigate the products of electrolysis of aqueous solutions using inert electrodes.
Set up electrolysis apparatus with inert electrodes (carbon or platinum). Use a power supply connected to the electrodes. Choose aqueous solutions (e.g. sodium chloride, copper sulfate). Observe and test gases formed (e.g. pop test for hydrogen, damp blue litmus for chlorine). Record observations at both electrodes. Write half-equations for the reactions. Repeat for different solutions and compare results.
29
What is an acid in terms of pH and ions released?
An acid has a pH less than 7. Acids release H⁺ ions in aqueous solution.
30
What is a base?
A base is a substance that reacts with an acid to form only a salt and water.
31
What is an alkali?
An alkali is a base that dissolves in water. Alkalis release OH⁻ ions in aqueous solution.
32
What is neutralisation?
Neutralisation is a reaction between an acid and a base, forming a salt and water.
33
What is a precipitate?
An insoluble solid formed when two solutions react together.
34
How can you make an insoluble salt using precipitation?
Mix two solutions containing ions that will form an insoluble salt. Filter the mixture to collect the precipitate. Wash and dry the precipitate.
35
Name three soluble salts and the ions they contain.
Sodium, potassium, and ammonium salts are soluble in water. Nitrates are soluble. Most chlorides are soluble (except silver and lead(II)). Most sulfates are soluble (except lead(II), barium, and calcium).
36
Name some common insoluble salts.
Most carbonates and hydroxides (except those of sodium, potassium, and ammonium). Lead(II) chloride, barium sulfate.
37
How can you make a soluble salt from an acid and a base?
Add excess insoluble base (e.g., copper oxide) to warm acid. Filter to remove excess base. Heat the filtrate to crystallise the salt. Leave to dry.
38
What is the importance of using excess base in this reaction?
To ensure all acid reacts and is neutralised, avoiding a contaminated product.
39
What is a strong acid?
A strong acid fully dissociates (ionises) in solution, releasing all H⁺ ions. ## Footnote Examples: Hydrochloric acid, sulfuric acid, nitric acid.
40
What is a weak acid?
A weak acid only partially dissociates in solution. ## Footnote Examples: Ethanoic acid, citric acid, carbonic acid.
41
How does pH relate to hydrogen ion concentration?
Every decrease of 1 on the pH scale represents a 10× increase in H⁺ ion concentration.
42
What is the general equation for acid + metal?
Acid + Metal → Salt + Hydrogen
43
What is the general equation for acid + metal oxide or hydroxide?
Acid + Metal oxide/hydroxide → Salt + Water
44
What is the general equation for acid + carbonate?
Acid + Metal carbonate → Salt + Water + Carbon dioxide
45
What are the products of neutralisation?
Salt and water
46
What is the ionic equation for neutralisation?
H⁺(aq) + OH⁻(aq) → H₂O(l)
47
Why are neutralisation reactions important in daily life?
Treating indigestion (antacids). Adjusting soil pH. Waste water treatment.
48
What is electrolysis?
Electrolysis is the breakdown of an ionic compound using electricity.
49
When can electrolysis occur?
When the ionic compound is molten or dissolved in water (so ions can move).
50
What is an electrolyte?
A liquid that conducts electricity and is broken down during electrolysis.
51
What happens at the electrodes?
Positive ions move to the cathode (gain electrons – reduction). Negative ions move to the anode (lose electrons – oxidation).
52
How is the product at the cathode determined in electrolysis of aqueous solutions?
If metal is more reactive than hydrogen, hydrogen gas forms. If metal is less reactive, the metal is deposited.
53
What happens at the anode in aqueous solutions?
If halide ions are present: halogen is formed. If no halide ions: oxygen is formed from OH⁻ ions.
54
What happens during the electrolysis of copper sulfate with carbon electrodes?
Copper metal forms at the cathode. Oxygen gas forms at the anode.
55
What happens during the electrolysis of copper sulfate with copper electrodes?
Anode loses mass as copper atoms become Cu²⁺ ions. Cathode gains mass as Cu²⁺ ions are reduced to copper.
56
(Six Marker) Describe how to investigate the products of electrolysis of aqueous solutions using inert electrodes.
Set up electrolysis apparatus with inert electrodes (carbon or platinum). Use a power supply connected to the electrodes. Choose aqueous solutions (e.g. sodium chloride, copper sulfate). Observe and test gases formed (e.g. pop test for hydrogen, damp blue litmus for chlorine). Record observations at both electrodes. Write half-equations for the reactions. Repeat for different solutions and compare results.

Chemistry Yr 10 (12 decks)

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