Alkaline permanganate and hydrogen sulfite

Slides:

Advertisements

Similar presentations

Balancing Redox Equations in Acidic Conditions

Advertisements

Writing Reactions --for unbalanced students. A few things to recall-- Synthesis Decomposition Single replacement Double replacement Other redox.

Biochemical Tests Reducing sugars Non-Reducing sugars Starch Lipid

Tests for cations in solution

Oxidation of alcohols.

Writing ion electron half equations…. ….and balanced redox equations (……. polyatomic ions or molecules are involved….) …in acidic and neutral solutions.

Reactions of alcohols.

Some reactions involving iodine/iodide. Potassium iodide solution (right) is colourless. Here we are about to oxidise the iodide using orange bromine.

Qualitative Analysis Chemistry. What is qualitative analysis Qualitative analysis is used to determine the chemical composition of an unknown substance.

TESTING FOR CATIONS QUALITATIVE ANALYSIS.

Cu 1+ Cu 2+ MnO 4 1- CrO 4 2- Cr 2 O 7 2- The presence of different ions in aqueous solution can be identified in a number of ways. One method is to.

Reaction of Potassium permanganate.  Speakers: 21709, 10, 21  Teacher:

Standardising potassium permanganate solution using oxalic acid

Chemical tests for redox species. Test for SO 4 2–, the sulfate ion The sulfate ion is colourless.

Unit 1 PPA 2 The effect of temperature on reaction rate.

Permanganate and hydrogen peroxide. Hydrogen peroxide solution is colourless. Permanganate in neutral conditions.

Draw the structural formula of: 1.3,3-dimethylbutan-1-ol. 2.2-methyl-butan-2-ol. Review of data exercise: 1.Explain the trend of BP of staight chain primary.

Calderglen High School

CHEMISTRY DEPARTMENT WAID ACADEMY Standard Grade Topic 9.

Ions In Solution.

Test for Anions. What is an anion? We will look at 1.The Chloride Ion Cl - 2.The sulfate ion SO The sulfite ion SO The carbonate ion CO.

SO 2 gas and BrO 3 -. Sulfur dioxide gas is generated by reacting dilute hydrochloric acid with solid sodium sulfite. 2HCl(aq) + Na 2 SO 3 (s) → SO 2.

MAKING SALTS 27/08/2015. Making Soluble Salts There are 3 types of reaction that can be used to make soluble salts. All 3 involve: An Acid A metal or.

Formation of a molecular species  It is the same as precipitates or gases except a liquid is formed.  Acid base neutralization reactions will produce.

 Acid-Base Reactions A “Basic” Introduction. Acids  Ionize in aqueous solutions to form H + ions  Memorize the 7 strong acids (completely ionize, never.

ACIDS & BASES module i.An acid is a chemical substance that …………………in water to produce ………………. ions. ii.A base is a chemical substance that ………………in.

 All chemical reactions have two parts: Reactants and Products.

Manganate(V11) and Dichromate(V1) as oxidizing agents

Salts By Amy Badger.

Acid reactions. Metals and acid reaction Example Magnesium Metal (Mg) reacts with Hydrochloric acid (HCl) to produce Hydrogen Gas and Magnesium Chloride.

Predicting redox reactions Single replacement reactions we went over a few chapters ago are all redox reactions. Here are the same examples, this time.

Oxidised state MnO 4 - Purple (aq) Permanganate Oxidised state Cr 2 O 7 2- Orange (aq) Dichromate Reduced state Cr 3+ Green (aq) Chromium ion Oxidised.

Study Guide, for Wed tutorial

2j Preparing and analysing. Last lesson - Precipitation reactions Reactions that produce an INSOLUBLE SALT.

2j Preparing and analysing

Quiz on Neutralization. 1. What happens when sodium hydroxide with litmus solution are added with hydrochloric acid slowly? The solution turns yellow.

What does soluble and insoluble mean?

Permanganate reactions. Manganese exists in many different oxidation states, each with a characteristic colour including: Mn VII: MnO 4 – purple Mn VI:

Identifying Ions Noadswood Science, 2013.

Solubility Noadswood Science, 2012.

Standardising potassium permanganate solution using oxalic acid.

Ch 8 Single replacement reactions  A + BX  AX + B  You will have a chart of activity series  More active metals will replace less active metals from.

AS Revision Lessons Identification tests.

Inorganic Analysis Fish!. Pick a question!

 Which of the following is an empirical formula? a. C 2 H 6 O 2 b. C 4 H 8 O 10 c. C 2 H 2 O 2 d. C 2 H 3 O 2.

Acids and Alkalis.

Universal Indicator can be used to find the pH of a solution

Universal Indicator can be used to find the pH of a solution

And the Indicators that tell the story….

Tests for Oxidising / Reducing Agents

Chemical Reactions #2.

Sulphate Anion Tests.

8.3 Preparation of salts Demonstrate knowledge and understanding of preparation, separation and purification of salts as examples of some of the techniques.

Do Now Knowing what you already know… write out the reaction between hexaaquachromium(III) ion and aqueous sodium hydroxide. Knowing what you already.

Inorganic Analysis Fish!.

Salt: an ionic substance. soluble: something that dissolves in water

Predicting Single Replacement, Double Replacement, & Combustion

Transition elements Manganese

Barium chloride reacts with sulfuric acid to produce barium sulfate and hydrochloric acid. If 98.2g of hydrochloric acid is needed how much barium chloride.

TESTING FOR CATIONS QUALITATIVE ANALYSIS.

MAKING SALTS 21/06/2019.

28th June 2012 Carboxylic acids

Hydrochloric Acid Hydrochloric acid solution (approximately 1 M):Beware of acid mist, do not wear contact lenses, wear safety glasses. In a fume cupboard,

7.1 ACIDS AND BASES.

Chemistry: Chemical Word Equations Directions: Write a balanced chemical equation for each of the word equations below. Refer to pages 165, 171 and.

Presentation transcript:

Alkaline permanganate and hydrogen sulfite

In the HSO3- ion, sulfur is in the +4 oxidation state. Sodium hydrogen sulfite is a white solid which dissolves in water to form a colourless solution.

Sodium hydroxide solution is added to make the solution alkaline.

Purple potassium permanganate solution is added. The purple solution turns green.

MnO4- + e- → MnO42-

The alkaline solution is acidified by adding hydrochloric acid. The green solution turns brown, then orange, and finally colourless as the excess HSO3- further reduces the green MnO42- to brown MnO2 and then colourless Mn2+.

Finally we add barium chloride solution, which reacts to form a white precipitate. This confirms that the HSO3- has been oxidised to SO42-. The solution had to be acidified first, because Ba(OH)2 is only slightly soluble.

MnO4- + e- → MnO42- purple green HSO3- + H2O → SO42- + 3H+ + 2e- 2MnO4- + HSO3- + H2O → 2MnO42- + SO42- + 3H+