reacting with their ions:

Slides:

Advertisements

Similar presentations

Halogen ion lab.

Advertisements

Testing for halide ions

Reactions in Aqueous Solutions

Chemical Reactions.

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

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

 Result when two soluble compounds mix and an insoluble (solid) compound is produced. AgNO 3 (aq) + NaCl (aq)  This is the insoluble compound (precipitate).

SCH 3U1 1. Solubility of Ionic Compounds 2 All solutes will have some solubility in water. “Insoluble” substances simply have extremely low solubility.

Monday, April 11 th : “A” Day Agenda  Homework questions/collect  Finish section 14.2: “Systems At Equilibrium”  Homework: Section 14.2 review, pg.

Solubility Rules.

Stoichiometry with Solutions Combining what you’ve just learned with what you are already good at.

Mix the following solutions in pairs Write down the solution pairs and record your results  Potassium Iodide  Barium Nitrate  Lead Nitrate  When finished,

Objectives To learn more about some of the results of chemical reactions To learn to predict the solid that forms in a precipitation reaction To learn.

Topic 9 Reactions of Acids.

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.

Salt soluble? yes, then choose an acid and a base base soluble? yestitrationno excess base no precipitation choose two soluble salts.

Ions In Solution.

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

Chemical Reactions 9.3: Reactions in Aqueous Solutions.

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.

Friday, March 21 st : “A” Day Monday, March 24 th : “B” Day Agenda  Homework questions/collect  Finish section 14.2: “Systems At Equilibrium”  Homework:

Precipitates and Solubility

Daily Science January 13 Predict the products of the following reactions and balance them:  C 3 H 8 + O 2   Sodium and nitrogen react  Calcium Fluoride.

Types of Chemical Reactions and Solution Stoichiometry.

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.

 Determine the type of reaction and predict the products: NaOH  Li + Br 2  C 2 H 4 + O 2 

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

Solubility Rules. The terms soluble and insoluble are relative terms. soluble insoluble solute Solubility: the maximum amount of solute needed to make.

©2003 Mark S. Davis Chapter 4 Aqueous Reactions Solution Stoichiometry.

Net Ionic Equations And A Little Review.

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

Chapter 11 – Chemical Reactions There are many types of chemical reactions. We will study 5 of these. By being able to identify the type of chemical reaction.

Solubility Rules. Precipitation Reactions If you’re not part of the solution You’re part of the precipitate.

Precipitation Reactions. Precipitation When two aqueous solutions combine to form an insoluble or only slightly soluble salt.

Warm-Up Nitrogen and hydrogen gas react to form ammonia according to the reaction N2 (g) + 3H2 (g) –> 2NH3 (g) If a flask contains the mixture of reactants.

Reactions in Aqueous Solution:. Double Replacement Reactions AB + CD  AD + CB AB + CD  AD + CB.

Precipitation Reactions

1) C + H 2 → C 3 H 8 2) C 6 H 12 + O 2 → H 2 O + CO 2 3) NaI + Pb(SO 4 ) 2 → PbI 4 + Na 2 SO 4 4) HgI 2 + O 2 → HgO + I 2 5)List the 7 diatomic molecules.

Ch (Net Ionic Equations)

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

Pg. 173 #11. Pg. 173 #12 Pg. 173 #13a The reaction does not work because silver is less reactive than hydrogen. That is, it is lower on the activity.

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

Match up the substance with the pH Lemon juice Hydrochloric acid Soap Sodium hydroxide Water pH 14 pH 0 pH 3 pH 7 pH 9.

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

Precipitation Reactions (Reactions that form a precipitate)

 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.

K sp and the Solubility Product Constant. K sp The Solubility Product Constant The study of __________ _________ compounds.

Precipitation Reactions

3.2.3 Group 7, the Halogens.

Identifying Halides.

Net Ionic Equations The formation of an insoluble solid (a precipitate) drives a chemical reaction. Chemists use 3 types of equations to represent aqueous.

Halide Anion Tests.

To Precipitate or not 6-6.

And Net Ionic Equations

Stoichiometry with Solutions

AN INTRODUCTION TO GROUP VII.

Testing for ions and gases

Chemical Equations Writing and balancing.

The Solubility Product Constant (Ksp)

Title: Reactivity of Halide Ions

Chemical Reactions Unit

11.3 Net Ionic Equations A complete ionic equation is an equation that shows dissolved ionic compounds as dissociated free ions. A precipitate of silver.

Predicting precipitation problems

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

Chemical Reactions Test Review

A selectively permeable membrane separates the solutions in the arms of a U-tube. The membrane is permeable to water and substance B, but not substance.

Nature of reactants affect the rate

Ch (Net Ionic Equations)

Presentation transcript:

reacting with their ions: Group 17 atoms reacting with their ions: F,Cl,Br,I ions

First reaction

Now add calcium nitrate to each tube NaF NaCl NaBr NaI Now add calcium nitrate to each tube

Added calcium nitrate to each tube. NaF NaCl NaBr NaI Added calcium nitrate to each tube.

Calcium nitrate + sodium fluoride = a precipitate What could it be? Calcium nitrate + NaF === calcium fluoride + sodium nitrate which is the precipitate???” Now balance the equation!

Second Reaction

Now add silver nitrate to each tube NaI NaBr NaCl NaF Now add silver nitrate to each tube

Added silver nitrate to each tube NaCl NaF NaI NaBr Added silver nitrate to each tube

NaCl + silver nitrate = sodium nitrate + silver chloride What could be causing the precipitate in the tubes? Added silver nitrate NaI NaBr NaCl NaCl + silver nitrate = precipitate NaBr + silver nitrate = precipitate NaI + silver nitrate = precipitate NaCl + silver nitrate = sodium nitrate + silver chloride Which one is the precipitate?

Another reaction 1st add ammonium hydroxide to each of the tubes containing precipitates, then later add sodium thiosulfate to each one

1. Now add ammonium hydroxide to each tube. 2. Now add sodium thiosulfate to each tube.

AgCl + ammonium hydroxide = precipitate dissolves…. AgBr + sodium thiosulfate = precipitate dissolves AgI doesn’t dissolve with either solution. You can try to predict what the balanced equations might be.