Caustic Soda Learning Objectives:

Slides:

Advertisements

Similar presentations

Electrolysis of solutions solutions can be electrolysed; gases are usually produced gases produced can be collected in test tubes; identified later by.

Advertisements

IC S4 P1+2 – First hand investigation and analyse information from secondary sources to predict and explain different products of aqueous and molten NaCl.

What is the name of the scientist who investigated the theory of electrolysis in 1830? Definition of Electrolyis Electrolysis is the conduction of electricity.

6.3 Electrolysing brine Brine is salty water. It’s chemical name is sodium chloride, NaCl aq. Both elements are useful in thousands of products. 04 May.

Electrolysis Of Brine Noadswood Science, 2012.

Let’s read! Pages 82 to 89. Objectives To know how to carry out electrolysis experiments. To work out what happens to ions at each electrode. To be able.

6. Electrochemistry Candidates should be able to: (a)Describe and explain redox processes in terms of electron transfer and/or of changes in oxidation.

Chemistry C Atomic Structure

Electrochemistry making elements using electricity

Electrolysis project Electrode: Is an electrical conductor that is used to pass current through an electrolyte.

I am learning to understand redox reactions EXAM TIPS: You may be asked to apply your understanding to industrial processes such as hair removal, plating.

CLASS PRACTICE 3 a. What four ions are present in sodium chloride solution? Na+(aq), Cl-(aq), H+(aq), OH-(aq) b. In Figure 21.3, write the ionic equation.

1 Chapter 3 Oceans 3.1 Introducing oceans and seas 3.2 Composition of sea water 3.3 Extraction of common salt from sea water 3.4 Tests for sodium and.

THE CHLOR-ALKALI INDUSTRY. Chlorine is manufactured by the electrolysis of brine. Sodium hydroxide is produced at the same time. Three different methods.

Sodium Hydroxide Experiment With Electrolysis

Option C12.  The chlor-alkali industry refers to the production of chlorine, sodium hydroxide and sodium carbonate.  Cl2 and NaOH are made from the.

Acids, Bases, and pH Unit 7: Acids and Bases. What are Acids? Definition: Ionic compounds that produce hydrogen ions (H+) when dissolved in water What.

ACIDS AND BASES. ACIDS & BASES Acids are substances that produce hydrogen ion in solution. (H + (aq) ) Bases are substances that produce hydroxide ions.

Solutions, Acids, and Bases Chapter 8. What Are Acids? acid - a compound that dissolves in water to increase the number of hydronium ions, H 3 O +, in.

13:19 Syllabus/Unit: code: C2 Chemical Resources Lesson number: 8 Lesson Title: Chemicals from the sea - Chemistry of NaCl Learning OutcomesHow I didTargets.

12.6 – How can we use ions in solutions?

Making Changes Topic overview. The topic can be conveniently split into six interrelated sections  Oxidation/Reduction  Salts  Preparation of gases.

Content page Introduction of Electrolysis Properties of sea water Compositions of sea water Electrode Electrolysis of sea water Chlorine gas Hydrogen.

Explain the process of electrolysis and its uses

Electrolytic cell: Converts electrical energy to chemical energy. Electrolysis – Electrolytic Cell Copper chloride CuCl Cu 2+ Cl - Cu 2+ (aq) +

Electrolysis To revise electrolysis of molten compounds: aluminium oxide To revise electrolysis of aqueous solutions: brine and copper sulfate.

Ions in Solution. Electrolysis During electrolysis ions move towards the electrodes. At the anode (+) Negatively charged ions are oxidised and lose electrons.

Acids and Bases (3).  Bases are the oxides or hydroxides of metals.  Contains either oxide ions (O 2- ) or hydroxide ions (OH - ) BaseFormulaIons present.

ACIDS AND BASES. What is acid? a substance that ionizes in water to produce hydrogen ions, H + What is base? a substance that reacts with an acid to form.

Splitting up ionic compounds (F) Molten compounds

ELECTROCHEMISTRY AS  Redox reactions  Oxidation : loses electrons/oxidation number increases /loses hydrogen/accepts oxygen  Reduction : accepts electrons/oxidation.

CHEMICALS AND THE EARTH Electrolysis of brine (salty water)

Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.

Electrolysis Decide on the answer(s) then click and a rectangle will surround the correct answer(s).

Topic 19 Oxidation and reduction

The purpose of electrolysis is to split up ionic compounds using electricity to produce useful products. Electrolysis is used a lot in industry and is.

Electrolysis L.O: To be able to describe the uses and predict the products of electrolysis.

Revision Quiz Acids 1 1.What is the pH scale? 2.What numbers on the pH scale show an acid? 3.What is an indicator? 4.What number is neutral? 5.What colour.

C2 REVISION – CHAPTER 1 – STRUCTURES & BONDING

1. Where would vinegar come on the Ph scale? 2. Where would normal rain come on the Ph scale? 3. Where would Bleach come? 4. Where would Washing up liquid.

Electro Chemistry. Conductors pass electricity (metals and ionic compounds (melted or in solution)) Insulators do not pass electricity (Plastics, wood,

Electrolysis Noadswood Science, 2012.

14.3 Electrolytic Cells  Electrolysis is the process of converting electrical energy into chemical energy.  Voltaic cells produce electrical energy and.

Electrolysis. What is electrolysis? Electrolysis means “breaking up a compound with electricity” From the Greek Electro – electricity Lysis – breaking.

IGCSE CHEMISTRY LESSON 4. Section 1 Principles of Chemistry a)States of matter b)Atoms c)Atomic structure d)Relative formula mass e)Chemical formulae.

IGCSE CHEMISTRY SECTION 5 LESSON 4. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

AQA GCSE C2.7.  When an ionic substance is melted or dissolved in water (to make a solution) the ions become free to move.  Electrolysis can then be.

What are the two equations used to calculate rates? Rate of reaction = amount of reactant used Time And Rate of reaction = C2 REVISION – Section C2.4.1.

ready Electrolysis anode cathode The cathode (-) attracts cations (+). The cations gain electrons and become neutral. The anode (+) attracts anions (-).

Some metals react with;

C2 REVISION – Section C2.4.1 – Rates of Reaction

TEXAS EDUCATION AGENCY POINT OF VIEW

The membrane keeps the chlorine gas away

Handle acid with care!.

6.1 Electrolysis Electrolysis: splitting up using electricity Ionic substance - molten ……… - dissolved ……… Non-metal ion Metal ion.

12.6 – How can we use ions in solutions?

Redox Reactions and Electrolysis

C3.4 – Electrolysis and cells

Make sure you revise the following:

Electrolytic processes EDEXCEL TOPIC 3: CHEMICAL CHANGES 2 Acids

1. What is the reaction between acid and alkalis called?

Chemistry Chapter 4 – Chemical changes – reactivity series, reduction and oxidation Write the reactivity series in order from most reactive to the least.

Presentation transcript:

Caustic Soda Learning Objectives: Describe the process of the electrolysis of brine Describe the uses of sodium hydroxide

Draw the practical set up you would need for electrolysis

INDUSTRIAL USES OF ELECTROLYSIS To extract reactive metals such as ALUMINIUM, sodium, magnesium etc from their compounds. This is EXPENSIVE due to the large amounts of electrical energy needed. Aluminium is extracted from bauxite (Al2O3). 2. Electrolysis of BRINE (salt solution) to produce CHLORINE (for disinfectants and plastics) HYDROGEN (for ammonia fertilisers, margarine) SODIUM HYDROXIDE (for soap and cleaning agents) 3. Purifying copper. The copper for wiring etc needs to be more pure than that produced in a blast furnace. Electrolysis is used to convert impure copper to pure copper see below see below

Electrolysis of Brine Practical

Questions 1 What did the universal indicator show you about the type of substance formed in: a the anode dish b the cathode dish? 2 Chlorine gas is given off at the anode. How can you tell? 3 Suggest the name of an acid that might be formed in the anode dish. 4 Chlorine is an important ingredient in bleach. What observation can you make that shows the bleaching property of chlorine? 5 Why would the experiment not have worked without the filter paper between the two dishes? 6 What would be the problem with connecting the two dishes up with a piece of metal wire? 7 Give the formulae of the two ions found in sodium chloride. 8 Which of these ions will be attracted to: a the anode b the cathode?

Electrolysis of brine The NaCl will split into Na+ ions and Cl- ions. Water splits into H+ ions and OH- (hydroxide) ions. So what do we think will happen during electrolysis? Remember – Na is VERY reactive, it is much more likely to exist as an ion than hydrogen.

Now let’s see what actually happens

Electrolysis of brine The H+ and Cl- ions are discharged at the electrodes.

Electrolysis of brine Hydrogen comes off at the cathode ( - ) 2H+(aq) + 2e- H2(g) Hydrogen is …… oxidised or reduced?

Electrolysis of brine Chlorine comes off at the anode ( + ) 2Cl(aq) - 2e- Cl2(g) Chlorine is …… oxidised or reduced?

Electrolysis of brine The Na+ and OH- ions stay in solution. They join together to form sodium hydroxide. This is a very important alkali

CATHODE ANODE H+ and Na+ OH- and Cl- INDUSTRIAL ELECTROLYSIS OF BRINE Chlorine gas Hydrogen gas BRINE (NaCl solution) CATHODE H+ and Na+ ANODE OH- and Cl- 2H+ + 2e- H2 2Cl- 2e- + Cl2 OH- left in solution so concentration grows Start: Sodium chloride solution (neutral) End: sodium hydroxide solution (alkaline) Na+ left in solution so concentration grows

Industrial chlorine production from electrolysis of brine

Hydrogen Used to make margarine (helps to make the oils in the margarine spread on your bread) Used as a fuel (already important in space rockets, but may be the fuel of cars after the oil age)

Sodium hydroxide Detergents and soap Paper

Sodium hydroxide Purifying bauxite to extract aluminium Rayon and acetate fibres

Chlorine Bleach Killing bacteria in water

Chlorine Solvents (used in dry cleaning) Hydrochloric acid (HCl)

Summary What are the 3 products? What they used for? Why do the dishes need to kept separate?