Learning Objectives: Describe and explain the tests for ions using sodium hydroxide solution Explain how precipitation reactions can be used to test for.

Slides:

Advertisements

Similar presentations

Halogen ion lab.

Advertisements

Reactions in Aqueous Solutions

Testing for halide ions

Reactions in Aqueous Solutions

What happens when you put

Tests for cations in solution

Writing Equations for Reactions in Solution Nia Gilliam 5/6 periods Chem. II, 3 rd tutorial.

Calculating Reacting Masses

Author: J R Reid Qualitative Analysis Qualitative – definitions of solubility Solubility rules Identifying ions Balancing ionic equations Complex ions.

Lesson 5 Learning Objectives: Describe the test for specific negative ions Explain how precipitation reactions can be used as the test for some ions.

Precipitate Reactions L.O. I can state which are spectator ions in a precipitation reaction. I can make a clean dry precipitate and write the ionic equation.

AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?

Topic E conservation of atoms and mass

Section 8-1 Describing Chemical Reactions. Chemical Reactions Watch closely Record all indications of a chemical reaction.

Calderglen High School

Testing for cations Lesson 11.5.

Sample Titration Problems

C4 Lesson 16 – Testing Water. After studying this topic, you should be able to: recall the tests for sulfate ions and halide ions in water write word.

Chapter 7: Reactions in aqueous solutions Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

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.

Complex Ions and stuff like that..

Unit 2 - Chemical Reactions. Double displacement occurs between ions in aqueous solution. A reaction will occur when a pair of ions come together to produce.

Lesson  We used sodium hydroxide and ammonia to identify positive ions.  We can carry out test to identify negative ions.  Negative ions are.

CHAPTER 8 Writing Chemical Equations © 2013 Marshall Cavendish International (Singapore) Private Limited.

Precipitates and Solubility

Ms Stephens Carry out procedures to identify ions present in solution Qualitative – definitions of solubility Solubility rules Identifying ions Balancing.

Identifying ions present in solution. A colourless solution is analysed to determine the cation and anion present. To separate samples of this solution.

C2- Chemistry Analysing substances, making salts, acids and bases

 DO NOW:  1. Watch the following video  2. Write your observations  3. Predict the products of AgNO 3 and NaCl.

1.Define displacement reaction. 2.Predict what will happen when: a)Magnesium is put into Silver Nitrate solution b)Zinc is put into Magnesium Nitrate solution.

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

Chemical tests to identify anions

Types of Reactions. In Chemistry, we can identify a lot of different types of chemical reactions. We can put these chemical reactions into groups, so.

Some Terminology Soluble – Will dissolve in a solvent Insoluble – Will not dissolve in a solvent Solvent – The substance that dissolves the solute Solute.

Making salts (3): precipitation. Soluble or insoluble? Insoluble salts are made by mixing two soluble compounds. The solid obtained when solutions of.

MEASURING CONCENTRATION OF IONS IN SOLUTION Molarity is ONE way to do this…we will learn others later in the year!!!

Dissolving of an Ionic Compound 1. Figure 7-2 p124.

A cids Bases & Salts (Salts) an e-learning series by ycs.

Identifying Ions Noadswood Science, 2013.

Precipitation Reactions

Precipitation Reactions

Net ionic equations Na + Al 3+ S 2– 2Ca 2+ PO 4 3– 3Cl –

Net Ionic Equations.

CH 8 Solubility Rules & Net Ionic Equations. Chemical Reactions Many chemical reactions take place in solution. This means that the ionic compounds are.

Ionic Equations. Net Ionic Equations AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?

If 36.2 mL of M CaCl 2 solution is added to 37.5 mL of M Na 2 CO 3, what mass of calcium carbonate, CaCO 3, will be precipitate? CaCl 2 (aq)

AS Revision Lessons Identification tests.

Pick up a Packet and write down the following Essential Question: How are precipitation reactions written and how is a compound determined to be soluble.

Precipitation Reactions (Reactions that form a precipitate)

Precipitation Reactions & Solubility Rules Thursday, February 18 th, 2016.

Qualitative Analysis- Solubility and Precipitation A.S (2.2) Year 12 Chemistry.

How to write an answer for AS 2.1. *Important You must write down all Observations You must back these observations up with all ionic equations.

 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.

EDEXCEL C2 Lesson 5 – Solubility Mrs Barnes CCYD

Precipitation Reactions

Balanced Equations 2H2 + O2  2H2O

Identifying Cations.

Halide Anion Tests.

To Precipitate or not 6-6.

And Net Ionic Equations

Qualitative Analysis Qualitative – definitions of solubility

Testing for ions and gases

Topic 9.1 Solutions.

Ionic Equations.

Question: How do we know what ions are present in a solution?

What happens when you put

Solubility Rules (Page 170)

Clicker #1 When aqueous silver nitrate and aqueous sodium chromate are mixed, what are the formulas of the products? A) Na2NO3 and AgCrO4 B) NaNO3 and.

Title: Acids and bases Complete the activities listed below

Presentation transcript:

Learning Objectives: Describe and explain the tests for ions using sodium hydroxide solution Explain how precipitation reactions can be used to test for some ions Lesson 3

Silver nitrate and sodium chloride dissolve in water. The solutions are colourless. Mix the solutions and a white precipitate forms.

A solution of sodium chloride contains sodium ions, Na +, and chloride ions, Cl -.

A solution of silver nitrate contains silver ions, Ag +, and nitrate ions, NO 3 -.

Mixing the two solutions puts all the ions together. The silver and chloride ions immediately form a white precipitate of solid silver chloride. The sodium and nitrate ions remain in solution.

AgNO 3 (aq) + NaCl(aq)  AgCl(s) + NaNO 3 (aq) Silver nitrate + sodium chloride  silver chloride + sodium nitrate A chemical equation summarises this precipitation reaction.

Practical – Testing for Cations A Put 1 cm depth of each of the cation solutions into six different test tubes. BAdd a few drops of sodium hydroxide solution to each test tube, and observe what happens. CIf a precipitate forms, add a further 1 cm of sodium hydroxide. Again observe any changes that might occur.

CationSymbolPrecipitate AmmoniumNH 4 + (aq)none AluminiumAl 3+ (aq)White CalciumCa 2+ (aq)White Copper(II)Cu 2+ (aq)blue Iron(II)Fe 2+ (aq)Green Iron(III)Fe 3+ (aq)brown 1. In the cation column what does the number in the bracket correspond to? 2. Which of the cation(s) need further testing ? Reactions of adding Sodium hydroxide

Further testing Ammonium Ions Heat the sample with concentrated sodium hydroxide. A smelly alkaline gas (ammonia) will be produced. It turns universal indicator paper blue/purple.

Aluminium and Calcium Ions If you add excess (more!) sodium hydroxide to a calcium precipitate and aluminium precipitate, different things will happen. Aluminium precipitate Calcium precipitate no change, will remain white Will dissolve Excess NaOH

Task Worksheet – C3.3 3b ‘More about Cations’ Only questions 1, 2 and 3. DO NOT WRITE ON THE SHEET!