C4 Chemical Changes

Last updated about 2 months ago

260 questions

4.4.1.1 Metal Oxides

4.4.1.1

4.4.1.2 The Reactivity Series

4.4.1.2

4.4.1.3 Extraction of Metals and Reducion

Required

4.4.1.3

Required

4.4.1.3

4.4.1.4 Oxidation and Reduction in Terms of Electrons

Required

4.4.1.4

Required

4.4.1.4

4.4.2.1 Reactions of Acids with Metals

4.4.2.1

Required

4.4.2.1

4.4.2.2 Neutralisation of acids and salt production

4.4.2.2

4.3.1.1

4.4.2.2

Required

4.4.2.2

Required

4.4.2.2

Required

4.4.2.2

Required

4.4.2.2

4.4.2.3 Soluble Salts

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.3.1.1

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.3.2.4

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

Required

4.4.2.3

4.4.2.4 The pH scale and neutralisation

4.4.2.4

4.4.2.5 Titrations

4.4.2.5

WS2.3

4.4.2.6 Strong and weak acids

4.3.2.5

4.4.2.6

4.4.2.4

4.4.2.6

4.4.3.1 The Process of Electrolysis

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

4.4.3.5

4.4.3.1

4.4.3.2 Electrolysis of molten ionic compounds

4.4.3.2

4.2.3.2

4.4.3.2

4.4.3.3 Using electrolysis to extract metals

4.4.3.3

4.4.3.1

4.4.3.3

4.4.3.1

4.4.3.3

4.4.3.1

4.4.3.3

4.4.3.5

4.4.3.3

4.4.3.5

4.4.3.3

4.4.3.4 Electrolysis of aqueous solutions

Required

4.4.3.4

Required

4.4.3.4

Required

4.4.3.4

4.4.3.5 Representation of reactions at electrodes as half equations

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

Required

4.4.3.5

C4 Chemical Changes

Last updated about 2 months ago

260 questions

4.4.1.1 Metal Oxides

Magnesium + Oxygen --> ?

4.4.1.1

Calcium + Oxygen --> ?

4.4.1.1

Iron + Oxygen --> ?

4.4.1.1

Zinc + Oxygen --> ?

4.4.1.1

Copper + Oxygen --> ?

4.4.1.1

What do you predict when magnesium reacts with oxygen?

4.4.1.1

4.4.1.2 The Reactivity Series

Calcium + water --> ?

4.4.1.2

Sodium + water --> ?

4.4.1.2

Aluminum + water --> ?

4.4.1.2

Iron + water --> ?

4.4.1.2

Zinc + copper sulfate --> ?

4.4.1.2

Aluminum + lead nitrate --> ?

4.4.1.2

Copper + silver nitrate --> ?

4.4.1.2

Aluminum + lead(II) chloride --> ?

4.4.1.2

Iron + silver nitrate --> ?

4.4.1.2

Does this reaction happen?

Zinc + copper sulfate --> copper and zinc sulfate

4.4.1.2

Does this reaction happen?

Iron + magnesium oxide --> magnesium and iron oxide

4.4.1.2

Does this reaction happen?

Aluminum + iron(III) chloride --> iron and aluminum chloride

4.4.1.2

What happens when sodium reacts with water?

4.4.1.2

What are the products of iron reacting with copper sulfate?

4.4.1.2

What do you expect when iron interacts with water?

4.4.1.2

What results when copper displaces silver from silver nitrate?

4.4.1.2

4.4.1.3 Extraction of Metals and Reducion

Required

4.4.1.3

Required

Pure metals don't need extracting
Reduction using carbon (or carbon monoxide)
Electrolysis

4.4.1.3

4.4.1.4 Oxidation and Reduction in Terms of Electrons

Required

4.4.1.4

Required

4.4.1.4

4.4.2.1 Reactions of Acids with Metals

4.4.2.1

Required

4.4.2.1

4.4.2.2 Neutralisation of acids and salt production

4.4.2.2

What is the salt formed when potassium reacts with hydrochloric acid?

4.4.2.2

What do you get when copper oxide reacts with sulfuric acid?

4.4.2.2

Which salt is formed when sodium hydroxide is neutralized by hydrochloric acid?

4.4.2.2

When ammonia reacts with sulfuric acid, what type of salt is produced?

4.4.2.2

What is the name for the salt formed from the reaction of Hydrochloric acid and Sodium Hydroxide?

4.4.2.2

What is the salt produced when Sulfuric acid reacts with Zinc?

4.4.2.2

Which of the following salts is formed by the reaction of Nitric acid and Potassium Hydroxide?

4.4.2.2

Ammonia reacts with Hydrochloric acid to form which salt?

4.4.2.2

Calcium chloride is a salt that can be named from hydrochloric acid.

4.4.2.2

All salts need to come from a reaction with a Metal.

4.4.2.2

Potassium sulfate can be generated from sulfuric acid.

4.4.2.2

What is the name of the salt produced from hydrochloric acid and sodium carbonate?

4.4.2.2

What is the name of the salt formed when sulfuric acid reacts with calcium oxide?

4.4.2.2

What salt forms when nitric acid reacts with magnesium hydroxide?

4.4.2.2

What is the salt produced when ammonia reacts with hydrochloric acid?

4.4.2.2

What type of salt is created when hydrochloric acid reacts with sodium?

4.4.2.2

What is the common name for the salt created when sulfuric acid reacts with potassium?

4.4.2.2

What salt is formed when nitric acid reacts with calcium?

4.4.2.2

Calcium hydroxide solution reacts with an acid to form calcium chloride.

Complete the word equation for the reaction.

calcium hydroxide + _______  acid → calcium chloride + _______ 

4.4.2.2

Soluble salts are formed by reacting metal oxides with acids.(a)

Give one other type of substance that can react with an acid to form a soluble salt.

4.4.2.2

Name the salt produced by the neutralisation of hydrochloric acid with potassium hydroxide.

4.4.2.2

Write a balanced symbol equation for the reaction of dilute hydrochloric acid with calcium oxide.

4.3.1.1

4.4.2.2

Zinc + hydrochloric acid --> ?

4.4.2.2

Iron + sulfuric acid --> ?

4.4.2.2

Copper + nitric acid --> ?

4.4.2.2

Aluminum + hydrochloric acid --> ?

4.4.2.2

Predict the products of zinc reacting with hydrochloric acid.

4.4.2.2

What products are produced when zinc is placed in hydrochloric acid?

4.4.2.2

Required

What salt is produced when hydrochloric acid reacts with sodium hydroxide?

4.4.2.2

Required

What salt is produced from the reaction of sulfuric acid and potassium hydroxide?

4.4.2.2

Required

Which salt forms when nitric acid interacts with calcium hydroxide?

4.4.2.2

Required

When a metal reacts with oxygen, the common product is typically a type of metal oxide.

4.4.2.2

4.4.2.3 Soluble Salts

Required

Plan a method to make pure, dry crystals of zinc chloride from zinc carbonate and a dilute acid.

4.4.2.3

Required

What is the difference between hazard and risk? (1:06)

4.4.2.3

Required

What do these symbols mean and what precautions should be taken? (1:15)

4.4.2.3

Required

Identify any hazards associated with this experiment. (1:15)

4.4.2.3

Required

What can we do to minimize any risks during this experiment? (1:15, 2:49)

4.4.2.3

Required

To make copper sulfate, what will we need to react with the sulfuric acid? (2:00-2:12)

4.4.2.3

Required

Write the word and symbol equation for the reaction. (2:00, 3:19) Word Equation: ________ + → + Symbol Equation: _ + _ → _ + ____

4.3.1.1

4.4.2.3

Required

What substances are now present in the boiling tube? Identify any ions present. (2:32-3:19)

4.4.2.3

Required

Look at the boiling tube. Name the particle responsible for: (2:49) (a) The blue color: _ (b) The black color:

4.4.2.3

Required

Explain what is meant by a limiting reactant. (3:35)

4.3.2.4

4.4.2.3

Required

How can we separate the product from the unreacted copper oxide? (3:43)

4.4.2.3

Required

What is the benefit of using fluted filter paper over a conical filter? (4:01)

4.4.2.3

Required

Describe what you see happening during the separation process. Explain your observations. (5:02-5:13)

4.4.2.3

Required

How and why do we need to remove excess water from the filtrate? (5:14-5:20)

4.4.2.3

Required

Why do we add anti-bumping crystals to the solution before heating? (5:24-5:40)

4.4.2.3

Required

What health and safety problems do you think may result if the solution is allowed to boil dry? (6:12)

4.4.2.3

Required

If there are no heat proof gloves available, what other safety precautions could be taken? (6:27)

4.4.2.3

Required

What conditions are needed to produce larger crystals? What conditions are needed to produce smaller crystals? (6:58)

4.4.2.3

Write a method for preparing a sample of pure dry zinc sulfate crystals from a metal oxide and acid.

4.4.2.3

4.4.2.4 The pH scale and neutralisation

Categorize the following pH values as acidic, neutral, or basic.

pH 7
pH 2
pH 5
pH 9

Neutral
Acidic

4.4.2.4

Pair each term with its definition

Draggable item		Corresponding Item
Indicator		Reaction between an acid and a base
Neutralisation		Measure of acidity or alkalinity
pH		Substance that changes color in an acid or base

4.4.2.4

Match the pH value with its description

Draggable item		Corresponding Item
pH 7		Neutral
pH 2		Strongly acidic
pH 10		Moderately alkaline

4.4.2.4

Match the substances with their pH levels

Draggable item		Corresponding Item
Vinegar		pH 7
Baking Soda		pH 3
Distilled Water		pH 9

4.4.2.4

Pair the reaction type with its effect on pH

Draggable item		Corresponding Item
Neutralisation Reaction		Brings pH to 7
Adding a Base		Raises pH
Adding an Acid		Lowers pH

4.4.2.4

What does a pH value of 7 represent?

4.4.2.4

What does the neutralisation process involve?

4.4.2.4

Acids have a pH...

4.4.2.4

Strong acids are closest to...

4.4.2.4

Alkalis have a pH...

4.4.2.4

Strong Alkalis have a pH closest to....

4.4.2.4

What color indicates a strong acid in universal indicator?

4.4.2.4

What color indicates a weak alkali in universal indicator?

4.4.2.4

What color shows a strong alkali in universal indicator?

4.4.2.4

What color indicates a weak acid in universal indicator?

4.4.2.4

Which ion do all acids produce in aqueous solution?

4.4.2.4

Write an ionic equation for the neutralisation of hydrochloric acid with potassium hydroxide.

_______  +  _______   →  _______ 

4.4.2.4

Name the type of reaction that takes place when dilute hydrochloric acid reacts with calcium oxide.

4.4.2.4

4.4.2.5 Titrations

Name apparatus A.

4.4.2.5

What is the reading on apparatus A?

4.4.2.5

How does the pH scale change with each unit?

4.4.2.6

If a solution has a Hydrogen ion concentration ([H+]) of 10^-7 M, what is its pH?

4.4.2.6

A sample of orange juice has a pH of 5. If lemon juice is 100 times more acidic, what is the pH of the lemon juice?

4.4.2.6

Ethanoic acid is a weak acid.

What is meant by ‘weak acid’?

Answer in terms of ionisation

4.4.2.6

Explain why the pH of an acid depends on:

the strength of the acid

the concentration of the acid.

4.4.2.4

4.4.2.6

A 1.0 × 10−3 mol/dm3 solution of hydrochloric acid has a pH of 3.0

What is the pH of a 1.0 × 10−5 mol/dm3 solution of hydrochloric acid?

4.4.2.6

4.4.3.1 The Process of Electrolysis

4.4.3.1

Required

What is the basic process during electrolysis?

4.4.3.1

Required

What are two main components required for electrolysis?

4.4.3.1

Required

Identify whether the following are cations or anions:

Oxygen (O2-)

4.4.3.1

On this diagram, label the anode, cathode, electrolyte, wires, and power source

4.4.3.1

In this example, water (H2O) is being electrolysed. What are the 2 gases being produced?

4.4.3.1

What is electrolysis?

4.4.3.1

What is the name of the electrode that positive ions move to?

4.4.3.1

What is the name of the electrode that the negative ions move to?

4.4.3.1

What is meant by the term ‘cation’?

4.4.3.1

What is the anode made of?

4.4.3.1

Match the term with its description

Draggable item		Corresponding Item
Anode		Positive electrode where oxidation occurs.
Cathode

4.4.3.1

What will the electrolysis of Sodium Chloride produce?

4.4.3.1

What will the electrolysis of Copper Chloride produce?

4.4.3.1

What will the electrolysis of Potassium Iodide produce?

4.4.3.1

What will the electrolysis of Magnesium Fluoride produce?

4.4.3.1

What does the electrolysis of Potassium Chloride produce?

4.4.3.1

What will the electrolysis of Sodium Iodide result in?

4.4.3.1

What are the products of the electrolysis of Copper Chloride?

4.4.3.1

What will the electrolysis of Calcium Bromide lead to?

4.4.3.1

Explain why electrolysis would not take place in the apparatus shown in Figure 1.

4.4.3.1

Explain why graphite conducts electricity.

Answer in terms of the structure and bonding in graphite.

4.2.3.2

True or false: Electrolysis is the separation of a compound using electricity?

4.4.3.1

What is the name for the positive electrode in electrolysis?

4.4.3.1

What type of current is used in electrolysis?

4.4.3.1

What is the charge on the cathode?

4.4.3.1

True or false: Electricity is used to separate a compound during electrolysis?

4.4.3.1

What is the charge on the anode?

4.4.3.1

What is the substance that is broken down during electrolysis called?

4.4.3.1

What is the negative electrode in electrolysis known as?

4.4.3.1

What state does the electrolyte need to be in for electrolysis?

4.4.3.1

What charge are the metal ions in an ionic compound?

4.4.3.1

Why do ionic compounds conduct electricity when molten or dissolved?

4.4.3.1

What substances form negative ions?

4.4.3.1

Which electrode do the negative ions move towards?

4.4.3.1

What is the name given to positive ions?

4.4.3.1

Which electrode do the cations move towards?

4.4.3.1

What is the name given to negative ions?

4.4.3.1

Which electrode do the anions move towards?

4.4.3.1

Which electrode do positive ions move to?

4.4.3.1

What charged ions do non-metals form?

4.4.3.1

Which electrode do positive ions move to?

4.4.3.1

Which electrode do the anions move towards?

4.4.3.1

Which electrode do the anions move towards?

4.4.3.1

Required

What is the basic process during electrolysis?

4.4.3.1

Required

Match the term with its definition.

Draggable item		Corresponding Item
Anode		Electrode where reduction occurs in an electrolytic cell.
Electrolyte		Electrode where oxidation occurs in an electrolytic cell.
Cathode		A substance that produces an electrically conducting solution when dissolved in a polar solvent.

4.4.3.1

True or false: Electrolysis is the separation of a compound using electricity?

4.4.3.1

What type of current is used in electrolysis?

4.4.3.1

What is the name for the positive electrode in electrolysis?

4.4.3.1

What is the charge on the anode?

4.4.3.1

What is the negative electrode in electrolysis known as?

4.4.3.1

What state does the electrolyte need to be in for electrolysis?

4.4.3.1

Which electrode do the negative ions move towards?

4.4.3.1

Which electrode do the cations move towards?

4.4.3.1

Which electrode do positive ions move to?

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

Required

4.4.3.1

4.4.3.5

4.4.3.1

4.4.3.2 Electrolysis of molten ionic compounds

What is produced at the cathode when lead bromide is electrolysed?

4.4.3.2

What is produced at the anode when lead bromide is electrolysed?

4.4.3.2

What would form at the cathode in the electrolysis of magnesium bromide?

4.4.3.2

What would form at the anode in the electrolysis of lithium chloride?

4.4.3.2

What would form at the anode in the electrolysis of molten sodium bromide?

4.4.3.2

What would form at the cathode in the electrolysis of molten aluminium chloride?

4.2.3.2

What would form at the cathode in the electrolysis of magnesium bromide?

4.4.3.2

What will the electrolysis of Magnesium Fluoride produce?

4.4.3.2

What will the electrolysis of Copper Chloride produce?

4.4.3.2

What would form at the anode in the electrolysis of molten sodium bromide?

4.4.3.2

What would form at the cathode in the electrolysis of molten aluminium chloride?

4.4.3.2

Identify the products of molten electrolysis for Calcium Bromide.

4.4.3.2

4.4.3.3 Using electrolysis to extract metals

Why is electrolysis used to extract aluminium form its ore?

4.4.3.3

Why is electrolysis an expensive way to extract metal from its ore?

4.4.3.3

Name the compound from which aluminium is extracted.

4.4.3.3

What is this compound dissolved in before electrolysis?

4.4.3.3

Describe what happens at the positive electrode during the electrolysis of aluminium oxide.

4.4.3.3

What is produced at the cathode?

4.4.3.1

4.4.3.3

What is (or should be) produced at the anode?

4.4.3.1

4.4.3.3

What are the electrodes made of?

4.4.3.1

4.4.3.3

1. Why is it more economical to extract aluminium from ores rather than minerals that are not ores?

4.4.3.3

To extract aluminium, molten bauxite and another ore, cryolite, undergo electrolysis.

Explain, in terms of the environment, why cryolite is added to the electrolyte.

4.4.3.3

Explain, in terms of the economic reasons, why cryolite is added to the electrolyte.

4.4.3.3

Some people think that extracting aluminium contributes negatively to climate change.
Explain why someone might think this, without discussing energy use.

4.4.3.3

What is the half equation at the cathode?

4.4.3.3

4.4.3.5

What is the half equation at the anode?

4.4.3.3

4.4.3.5

What would be the products of molten electrolysis for Aluminum Oxide?

4.4.3.3

What will be the products of molten electrolysis for Potassium Iodide?

4.4.3.3

Explain why the electrolysis of Aluminium oxide contributes to climate change. (hand mark)

4.4.3.3

4.4.3.4 Electrolysis of aqueous solutions

Required

4.4.3.4

Required

4.4.3.4

Required

4.4.3.4

What is produced at the cathode is the metal in the solution is more reactive than hydrogen?

4.4.3.4

What is produced at the anode if the solution does not contain halide ions?

4.4.3.4

Predict the products of electrolysis of copper sulfate solution

4.4.3.4

Trim End | 06:44

Question 220 | 00:00

Question 221 | 00:15

Question 222 | 00:30

Questions 223 & 224 | 00:59

Question 225 | 01:32

Question 226 | 01:51

Question 227 | 02:01

Question 228 | 02:49

Question 229 | 03:37

Questions 230 & 231 | 03:56

Question 232 | 04:28

Question 233 | 04:50

00:00/00:00

Question 220

00:00

Question 221

00:15

Question 222

00:30

Questions 223 & 224

00:59

Question 225

01:32

Question 226

01:51

Question 227

02:01

Question 228

02:49

Question 229

03:37

Questions 230 & 231

03:56

Question 232

04:28

Question 233

04:50

4.4.3.5 Representation of reactions at electrodes as half equations

HT Only: Write half equations for the reactions that happen at the
electrodes during the electrolysis of molten copper chloride.

4.4.3.5

HT Only: Write a half equation for the reactions that happen at the
electrodes during the electrolysis of copper bromide solution

4.4.3.5

HT Only: Write half equations for the reactions that occur at the positive and negative electrodes during the production of aluminium.

4.4.3.5

Required

What is reduction in terms of electrons?

4.4.3.5

Required

What does oxidation involve in terms of electrons?

4.4.3.5

Required

An atom that loses an electron during a reaction is...

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

Cu2+ (aq) --> Cu (s)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

Mg2+ (aq) --> Mg (s)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

Al3+ (aq) --> Al (s)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

Li+(l) -->Li(s)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

H+(aq) -->H2(g)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

Br-(aq) --> Br2(g)

4.4.3.5

Required

Rewrite the equation with number of electrons on the correct side:

O2-(aq) --> O2(g)

4.4.3.5

Magnesium chloride can be electrolysed.The diagram below shows two experiments for electrolysing magnesium chloride.

Explain why magnesium chloride must be molten or dissolved in water to be electrolysed.

4.4.3.1

Explain how magnesium is produced at the negative electrode in Experiment 1.

4.4.3.5

Cu2+ + _______  --> Cu

4.4.3.5

Mg2+ + _______  --> Mg

4.4.3.5

Al3+ + _______  --> Al 

4.4.3.5

Li1+ +_______  -->Li

4.4.3.5

2H1+ + _______  -->H2

4.4.3.5

2Br1- --> Br2 + _______ 

4.4.3.5

2O2- --> O2 + _______ 

4.4.3.5

Zinc chloride is an ionic substance.

Complete the sentence.

When zinc chloride is molten, it will conduct _______ 

4.4.3.1

4.4.3.5

Required

What does oxidation involve in terms of electrons?

4.4.3.5

C4 Chemical Changes

C4 Chemical Changes

Magnesium + Oxygen --> ?

Calcium + Oxygen --> ?

Iron + Oxygen --> ?

Zinc + Oxygen --> ?

Copper + Oxygen --> ?

What do you predict when magnesium reacts with oxygen?

Calcium + water --> ?

Sodium + water --> ?

Aluminum + water --> ?

Iron + water --> ?

Zinc + copper sulfate --> ?

Aluminum + lead nitrate --> ?

Copper + silver nitrate --> ?

Aluminum + lead(II) chloride --> ?

Iron + silver nitrate --> ?

Does this reaction happen?Zinc + copper sulfate --> copper and zinc sulfate

Does this reaction happen?Iron + magnesium oxide --> magnesium and iron oxide

Does this reaction happen?Aluminum + iron(III) chloride --> iron and aluminum chloride

What happens when sodium reacts with water?

What are the products of iron reacting with copper sulfate?

What do you expect when iron interacts with water?

What results when copper displaces silver from silver nitrate?

What is the salt formed when potassium reacts with hydrochloric acid?

What do you get when copper oxide reacts with sulfuric acid?

Which salt is formed when sodium hydroxide is neutralized by hydrochloric acid?

When ammonia reacts with sulfuric acid, what type of salt is produced?

What is the name for the salt formed from the reaction of Hydrochloric acid and Sodium Hydroxide?

What is the salt produced when Sulfuric acid reacts with Zinc?

Which of the following salts is formed by the reaction of Nitric acid and Potassium Hydroxide?

Ammonia reacts with Hydrochloric acid to form which salt?

Calcium chloride is a salt that can be named from hydrochloric acid.

All salts need to come from a reaction with a Metal.

Potassium sulfate can be generated from sulfuric acid.

What is the name of the salt produced from hydrochloric acid and sodium carbonate?

What is the name of the salt formed when sulfuric acid reacts with calcium oxide?

What salt forms when nitric acid reacts with magnesium hydroxide?

What is the salt produced when ammonia reacts with hydrochloric acid?

What type of salt is created when hydrochloric acid reacts with sodium?

What is the common name for the salt created when sulfuric acid reacts with potassium?

What salt is formed when nitric acid reacts with calcium?

Soluble salts are formed by reacting metal oxides with acids.(a) Give one other type of substance that can react with an acid to form a soluble salt.

Name the salt produced by the neutralisation of hydrochloric acid with potassium hydroxide.

Write a balanced symbol equation for the reaction of dilute hydrochloric acid with calcium oxide.

Zinc + hydrochloric acid --> ?

Iron + sulfuric acid --> ?

Copper + nitric acid --> ?

Aluminum + hydrochloric acid --> ?

Predict the products of zinc reacting with hydrochloric acid.

What products are produced when zinc is placed in hydrochloric acid?

What salt is produced when hydrochloric acid reacts with sodium hydroxide?

What salt is produced from the reaction of sulfuric acid and potassium hydroxide?

Which salt forms when nitric acid interacts with calcium hydroxide?

When a metal reacts with oxygen, the common product is typically a type of metal oxide.

Plan a method to make pure, dry crystals of zinc chloride from zinc carbonate and a dilute acid.

What is the difference between hazard and risk? (1:06)

What do these symbols mean and what precautions should be taken? (1:15)

Identify any hazards associated with this experiment. (1:15)

What can we do to minimize any risks during this experiment? (1:15, 2:49)

To make copper sulfate, what will we need to react with the sulfuric acid? (2:00-2:12)

Write the word and symbol equation for the reaction. (2:00, 3:19) Word Equation: ____________________ + ____________________ → ____________________ + ____________________ Symbol Equation: _______________ + _______________ → _______________ + __________

What substances are now present in the boiling tube? Identify any ions present. (2:32-3:19)

Look at the boiling tube. Name the particle responsible for: (2:49) (a) The blue color: _________________________________________ (b) The black color: ________________________________________

Explain what is meant by a limiting reactant. (3:35)

How can we separate the product from the unreacted copper oxide? (3:43)

What is the benefit of using fluted filter paper over a conical filter? (4:01)

Describe what you see happening during the separation process. Explain your observations. (5:02-5:13)

How and why do we need to remove excess water from the filtrate? (5:14-5:20)

Why do we add anti-bumping crystals to the solution before heating? (5:24-5:40)

What health and safety problems do you think may result if the solution is allowed to boil dry? (6:12)

If there are no heat proof gloves available, what other safety precautions could be taken? (6:27)

What conditions are needed to produce larger crystals? What conditions are needed to produce smaller crystals? (6:58)

Write a method for preparing a sample of pure dry zinc sulfate crystals from a metal oxide and acid.

Categorize the following pH values as acidic, neutral, or basic.

Pair each term with its definition

Match the pH value with its description

Match the substances with their pH levels

Pair the reaction type with its effect on pH

What does a pH value of 7 represent?

Does this reaction happen?

Zinc + copper sulfate --> copper and zinc sulfate

Does this reaction happen?

Iron + magnesium oxide --> magnesium and iron oxide

Does this reaction happen?

Aluminum + iron(III) chloride --> iron and aluminum chloride

Soluble salts are formed by reacting metal oxides with acids.(a)

Give one other type of substance that can react with an acid to form a soluble salt.

Write the word and symbol equation for the reaction. (2:00, 3:19) Word Equation: ________ + → + Symbol Equation: _ + _ → _ + ____

Look at the boiling tube. Name the particle responsible for: (2:49) (a) The blue color: _ (b) The black color:

Ethanoic acid is a weak acid.

What is meant by ‘weak acid’?

Answer in terms of ionisation

Explain why the pH of an acid depends on:

the strength of the acid

the concentration of the acid.

A 1.0 × 10−3 mol/dm3 solution of hydrochloric acid has a pH of 3.0

What is the pH of a 1.0 × 10−5 mol/dm3 solution of hydrochloric acid?

Explain why graphite conducts electricity.

Answer in terms of the structure and bonding in graphite.