Chem 1310: Introduction to physical chemistry Part 3: Equilibria Writing K expressions.

Slides:

Advertisements

Similar presentations

Unit 7: Reactions in Solution

Advertisements

Chemical Reactions The result of the chemical reaction is a new substance with unique physical and chemical properties. The result of the chemical reaction.

Reactions in Aqueous Solutions

Chapter 4 Solutions and Chemical Reactions

Types of Chemical Reactions and Solution Stoichiometry.

© 2012 Pearson Education, Inc. Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest.

Dissolving vs. Dissociating Sugar vs. Salt. Electrolytes: Charged particles or ions present in a solution can conduct an electric current. Ionic compounds.

The Language of Chemistry

Aqueous Reactions and Solution Stoichiometry. Aqueous Solutions Aqueous solutions are solutions in which water does the dissolving. –Solute – material.

Unit 3 – Chemical Reactions.  In many ionic reactions, not all of the chemical species undergo a change.  Those that do not change are called spectator.

Chemical Equilibrium. Reversible Reactions Reversible reactions are those in which the products can react to re-form reactants. Ex: 2HgO (s) + heat >

Chapter 18: Chemical Equilibrium

Precipitation reaction – reaction in which an insoluble product forms Precipitate – an insoluble solid that separates from the solution Solubility – maximum.

COMMUNICATING CONCENTRATION: Section 5.3.  Most solutions are similar in that they are colorless and aqueous, so there is no way of knowing, by looking.

Solutions are homogeneous mixtures consisting of two or more components. The major component of a solution is known as the solvent and the minor component.

Solubility Equilibria. Write solubility product (K sp ) expressions from balanced chemical equations for salts with low solubility. Solve problems involving.

Copyright © 2004 Pearson Education Inc., publishing as Benjamin Cummings Properties of Water 9.2 Solutions 9.3 Electrolytes and Nonelectrolytes.

Double Displacement Reactions

Types of Chemical Reactions and Solution Stoichiometry Chapter 4.

Equilibrium SCH4U organic photochromic molecules respond to the UV light.

II III I I. The Nature of Solutions Ch Solutions.

I. The Nature of Solutions Solutions. A. Definitions  Solution - homogeneous mixture Solvent - present in greater amount Solute - substance being dissolved.

Unit 11: Acids, Bases, and Solutions Introduction to Solutions.

1 Solutions Chemistry I2 – Chapters 7 & 8 2 Some Definitions A solution is a homogeneous mixture of 2 or more substances. One constituent is usually.

Chapter 13 Solutions. Solution Concentrations 3 Solution Concentration Descriptions dilute solutions have low solute concentrations concentrated solutions.

Balancing chemical equations. WRITING CHEMICAL EQUATIONS Chemical equations should show : (a) formulas of the reactants & products (b) their states of.

Concentration/Molarity/Molar Concentration A measure of the amount of solute that is dissolved in a measured amount of solvent. Dilute: a solution that.

 A process by which one or more substances are changed into one or more different substances. Reactants  Products.

Solutions: Molarity. A. Concentration – measure of the amount of solute that is dissolved in a given amount of solvent I. Concentration of Solutions Solutions:

4.4 Solution Concentration and Stoichiometry. Solution Key Terms What type of mixture is also considered a solution? Give an example. – A homogeneous.

INTRODUCTION TO SOLUTIONS/ACIDS AND BASES HONORS CHEMISTRY MAY 27 TH, 2014.

Reactions in Aqueous Solutions 1. Solutions (textbook p ) Aqueous Solution – A solution in which the solvent is water. Water is the solvent (does.

Reactions in Aqueous Solution. Reactions in aqueous solution Many reactions, esp. many double replacement reactions, occur in water. What happens when.

Aqueous Solutions Some solutes exist as molecules when dissolved in water (sugar, ethanol) Many solutes dissociate or form ions in water Acids form H +

Solubility Equilibrium Chapter 7. The Solubility Equilibrium Remember from SPH3U: Solubility is the amount of solute that dissolves in a given amount.

Chemical Equilibrium Physical Equilibrium AND. Describe physical and chemical equilibrium Describe the conditions needed for equilibrium. Write the equilibrium.

Electrical Conductivity

“Chemical Reactions”. All chemical reactions…  have two parts: 1.Reactants = the stuff you start with 2.Products = the stuff you end up with  The reactants.

Introduction & Net Ionic Equations

Electrical Conductivity. Questions (copy them out first) Give the definition and an example for the following terms: 1)A solution is__________________?

2 Word Equations. Phase Symbols Are subscripts that indicate the phase of the chemical.

Chemical Reactions.  In chemical reactions, one or more substances change into different substances. example: combustion.

S O L U T I O N S SOLUTION: HOMOGENEOUS MIXTURE OF 2 OR MORE CHEMICAL SUBSTANCES SOLUBILITY: MAXIMUM AMOUNT OF SOLUTE THAT CAN BE DISSOLVED AT A GIVEN.

Solutions Lesson #1 Vocabulary Dissolving. What is a Solution? It is a homogeneous mixture built from two or more components. The components may be elements.

Ionic Equations Most ionic compound dissociate (or break apart) when dissolved in water to form its component ions For example: NaCl (aq) really looks.

Solubility Chapter 17 & 18. Solutions  Solutions are made of a solute and a solvent.  In this chapter we are concentrating on solutions of water. 

Solution Chemistry solution of two or more substances homogeneous mix solvent = solute = substance present in major amount substance present in minor amount.

Concentration of Ions in Solution Remember: concentration IS molarity.

Chemical Equilibrium.  In principle, every chemical reaction is reversible:  Capable of moving in the forward or backward direction. Some reactions.

I. The Nature of Solutions

General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc. 1 Chapter 8 Solutions 8.1 Solutions.

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?

3.6Molar Concentration Molarity – A Useful Unit of Concentration Preparing a Standard Solution from a Solid Ions in Solution.

Reaction Prediction. You should already know... ionic, molecular, and acid nomenclature. how to balance chemical equations. the five common types of chemical.

Equilibrium Chemistry— Introduction. Chemical Equilibrium State for a chemical reaction where the reaction stops BEFORE all of the limiting reactant has.

Copyright © Houghton Mifflin Company. All rights reserved. 15 | 1 Solutions Solutions are uniform mixtures. Solvent: the substance present in the highest.

Chemistry Reaction Types. Superbowl Ads Anatomy of a Chemical Equation Flour Eggs Milk + Pancakes  Plus (reacts with) Produces (s)(l)(s) State of matter.

Basic Principles of Chemistry Unit 2: Chemical Reactions and Their Significance Lecture #11.

Solutions, Electrolytes, and Precipitation Reactions.

Review of Science 10 Dissociation and Word Equations.

Solubility PrecipitationMolalityEndothermicExothermic.

Unit 12 Solutions And you. OBJECTIVE To gain informed insights into reactions that take place in aqueous environments you need to have a solid conceptual.

TOPIC: WATER, the neutral substance Do Now. Water self-ionizes H 2 O(l) + H 2 O(l)  H 3 O +1 (aq) + OH -1 (aq) H 3 O +1 H 3 O +1 = hydronium ion OH -1.

Solution Concentration Chemistry. Ways to Express Solution Composition Molarity: Mass %: Volume %: Parts per million (ppm):

Particles in Solution.

Classification of Matter

On a Scale of 0 to 14 pH Notes.

Solution chemistry What are solutions?

Ionic Equations.

NaCl (aq.) + AgNO3 (aq.) → AgCl (s) + NaNO3 (aq.)

Presentation transcript:

Chem 1310: Introduction to physical chemistry Part 3: Equilibria Writing K expressions

Write out the chemical equation. Write out the K expression using concentrations whenever possible. Initially include all components, including solids etc. Then remove the pure solids, pure liquids and "nearly-pure" solvents.

Dissociation of an acid in water HNO 2 in water

Dissociation of an acid in water HNO 2(aq) + H 2 O ⇋ NO 2 - (aq) + H 3 O + (aq)

Dissociation of an acid in water HNO 2(aq) + H 2 O ⇋ NO 2 - (aq) + H 3 O + (aq)

Dissociation of an acid in water HNO 2(aq) + H 2 O ⇋ NO 2 - (aq) + H 3 O + (aq)

Dissolving a salt in water NaCl (s) ⇋ Na + (aq) + Cl - (aq)

Dissolving a salt in water NaCl (s) ⇋ Na + (aq) + Cl - (aq)

Evaporation of a solid I 2(s) ⇋ I 2(g)

Evaporation of a solid I 2(s) ⇋ I 2(g)

Dissolving a gas in water CO 2(g) ⇋ CO 2(aq)

Dissolving a gas in water CO 2(g) ⇋ CO 2(aq)

Dissolving a liquid in water Br 2(l) ⇋ Br 2(aq)

Dissolving a liquid in water Br 2(l) ⇋ Br 2(aq)