Sodium Hydroxide Experiment With Electrolysis

Slides:

Advertisements

Similar presentations

Acids, Bases, and Solutions

Advertisements

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

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

The chlor-alkali industry

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.

Electrolytic Cells Is a Galvanic Cell forced to operate in reverse Process is called electrolysis This occurs if a voltage greater than that produced by.

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

Electrochemistry making elements using electricity

Hydrogen electrolysis Hydrogen electrolysis is the process of running an electrical current through water (H 2 O) and separating the hydrogen from the.

Third Nine Weeks- 9 weeks review

Caustic Soda Learning Objectives:

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.

IC Products from sodium chloride © Oxford University Press 2011 Products from sodium chloride.

Bleach 21 What is a bleach? What has caused this colour change?

CHLORINE AND ITS COMPOUNDS HALOGENS. HHe Rn Xe Kr Ar Ne RaAcRfDbSgBhHsMtDsRg??????? BaLaHfTaWReOsIrPtAuHgTlPbBiPoAt SrYZrNbMoTcRuRhPdAgCdInSnSbTeI CaScTiVCrMnFeCoNiCuZnGaGeAsSeBr.

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

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

Today’s lesson The allotropes of sulphur

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

The Preparation and Collection Of Non-Metals.

Electrolysis. –A redox reaction that is made to occur by passing a direct electric current through an electrolyte Electrolyte –is a liquid that conducts.

Lecture 41 - Electrochemistry V. Review Galvanic Cells: Reaction is spontaneous E o cell > 0 The “product” is an electrical current Some can be reversed.

1 Lec. 2 Faraday’s Laws Lec. 2 Faraday’s Laws Industrial Electrolytic Processes “Electrolysis”

12.6 – How can we use ions in solutions?

When bleach is treated with an acid, evolution of chlorine gas ensues Preparation of Chlorine Gas from Bleach.

Reactions of chlorine with water and sodium hydroxide.

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

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)

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

Topic 19 Oxidation and reduction

Electrochemistry (Ch 11) 1. Define: a. galvanic (voltaic) cell b. electrolytic cell.

18.8 Electrolysis 2 Types of electrochemistry 1.Battery or Voltaic Cell – Purpose? 2.Electrolysis - forces a current through a cell to produce a chemical.

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

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.

C3 Chemicals in Our Lives – Risks & Benefits Lesson 9: Electrolysis of Brine.

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.

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

CHEMICAL PROCESS INDUSTRIES-1 ( )

Chapter  The electrochemical cells require the INPUT of energy rather than creating energy.

Teknik Elektrokimia Instructor: Rama Oktavian

Electrolysis 3 Electrolysis An electrolysis is the inverse of an electrochemical cell. A non-spontaneous reaction is caused by the passage of an.

TEXAS EDUCATION AGENCY POINT OF VIEW

The membrane keeps the chlorine gas away

Predicting products of electrolysis

12.6 – How can we use ions in solutions?

ELECTROLYSIS Products of Electrolysis

Make sure you revise the following:

Chemistry 21.3.

An electrolytic cell uses electricity to do a chemical reaction.

Chapter 17: Electrochemistry

Laboratory Chemistry vs. Industrial Chemistry There are fundamental differences between the design of a chemical synthesis for industry and.

Q: What is the acid produced in the stomach?

REDOX sodium metal is added to water. Na + 2H2O  Na+ + 2OH- + H2

CHLORINE AND ITS COMPOUNDS

C4 – Chemical changes Key Concepts.

Presentation transcript:

Sodium Hydroxide Experiment With Electrolysis Mükremin Buğdacı

What is Brine? Brine is a concentrated solution of sodium chloride. During electrolysis, the overall reaction is: 2NaCl(aq)+ 2H2O(l) 2NaOH(aq)+ Cl2(g)+H2(g)

The Electrolysis

At the Cathode Hydrogen is discharged in preference to sodium: 2H+(aq) + 2e- H2(g) As usuan at the cathode, this is reduction.

At the Anode Chlorine is discharged in preference to Oxygen: 2Cl- (aq) Cl2 + 2e- As usual at the anode, this is oxidation.

Sodium Hydroxide The two gases bubble off. Na+ and OH- ions are left behind, giving a solution of sodium hydroxide. Some of the solution is evaporated to a give more concentrated solution, end some is evaporated to dryness, giving solid sodium hydroxide.

What the products are used for

Chlorine, a poisonous yellow-green gas Used for making… The plastic PVC Solvents for degreasing and drycleaning Medical drugs Weedkillers and pesticides Paints and dyestuffs Bleaches Hydrogen chloride and hydrochloric acid It is also used as a sterilising agent, to kill bacteria in water supplies and swimming pools

Hydrogen, a colourless flammable gas Used… In making nylon To make hydrogen peroxide To harden vegetable oils to make margarine As a fuel in hydrogen fuel cells

Sodium hydroxide solution, alkaline and corrosive Used in making… Soaps Detergents Viscose and other textiles Paper Ceramics Dyes Medical drugs

Sources http://aquarius.nasa.gov/pdfs/electrolysis.pdf http://www.gcsescience.com/ex4.htm http://www.science.uwaterloo.ca/~cchieh/cact/c123/el tlysis.html http://answers.yahoo.com/question/index?qid=20070 813195931AAttlJU http://www.elkadot.com/en/chemistry/Electrolysis%2 0of%20Molten%20Sodium%20Chloride.htm