What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH -
|
|
- Anabel Harrington
- 7 years ago
- Views:
Transcription
1 Chemistry Date Period Name CW double replacement reactions doc Double Replacement Reactions Double replacement reactions are some of the most common reactions that are performed in the laboratory. They almost always occur in an aqueous (water) solution. They frequently result in the formation of one or more insoluble compounds which precipitate as a solid. Before going very far into double replacement reactions, it will be necessary to discuss aqueous solutions. Compounds can be broadly classified as being either soluble or insoluble in water. Those compounds which are soluble in water form aqueous solutions. Suppose that solid sodium hydroxide (NaOH) pellets are placed in water: What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH This chemical equations represents solid NaOH dissolving in water to form sodium ions and hydroxide ions. The solid NaOH breaks apart (dissociates) into two ions. (Ions are electrically charged atoms formed by either gaining or losing the electrons involved in bonding. Since ions and atoms are extremely small they cannot be seen with the eye.) IMPORTANT When a soluble salt dissolves in water it will dissociate (break apart) into a positively charged ion and a negatively charged ion. Here are some examples of the dissociation of salts producing two ions in solution: FeSO 4 (s) Fe 2+ + SO 4 2 MgCl 2 (s) Mg Cl Al(NO 3 ) 3 (s) Al NO 3 Na 2 CO 3 (s) 2 Na CO 3 There are many solids which are not soluble in water. AgCl, PbSO 4, FeS, Cu(OH) 2, CaCO 3, and CdS are some insoluble salts. These don t dissolve in water and don t dissociate to form ions. Insoluble salts can also be formed by combining two soluble salts. When the two ions of an insoluble salt come together, the insoluble salt will form and come out of solution as a solid precipitate. Such is the case when solutions of sodium sulfide and cadmium nitrate are combined. Yellow cadmium sulfide, CdS, is the insoluble product. Na 2 S(aq) + Cd(NO 3 ) 2 CdS(s) + 2NaNO 3 (aq)
2 Double Replacement Reactions Precipitation Reactions Consider the case where solutions of silver nitrate and sodium chloride are mixed. Both are soluble salts. But they form an insoluble product, silver chloride. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) Notice how the positive ion of one compound will combine with the negative ion of the other compound: AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) Since silver nitrate and sodium chloride are both soluble in water, silver nitrate actually exists as silver ions (Ag + ) and nitrate ions (NO 3 ), and sodium chloride actually exists as sodium ions (Na + ) and chloride ions (Cl ). When the two solutions are placed together in a beaker, all four ions have a chance to "mingle". When the silver ions (Ag + ) collide with chloride ions (Cl ), solid silver chloride precipitates. Silver chloride is NOT soluble in water. This reaction is called a "molecular equation" since all the compounds are written as molecules. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) But the molecular equation is not very accurate since the two salts exists as ions in solution. Therefore, a better way to represent the reaction the ionic equation. In the ionic equation all of the compounds which are dissociated into ions are written as ions, and the insoluble compounds are written as molecules. The ionic equation is more accurate because it represents what is actually in solution. The ionic equation for the silver nitratesodium chloride reaction is: Ag + + NO 3 + Na + + Cl AgCl(s) + Na + + NO 3 + If we look at the reaction that occurs, we see there are only two ions which actually react. Ag + + NO 3 + Na + + Cl AgCl(s) + Na + + NO 3 + The reaction produces solid AgCl which is insoluble. The sodium nitrate (NaNO 3 ) doesn't form an insoluble precipitate since it is soluble in water. Therefore, the sodium ions and nitrate ions stay just as they were. They are referred to as spectator ions. Before reaction After reaction Spectator ions Insoluble precipitate
3 We can represent the ions that actually react with the "net ionic equation": Ag + + Cl AgCl(s) The net ionic equation says that "in any reaction in which there is a silver ion and a chloride ion, the two ions will react and precipitate as solid silver chloride." In the net ionic equation the spectator ions are omitted. Consider another example where solutions of iron(ii) chloride and sodium phosphate are mixed together. Balanced molecular equation: 3FeCl 2 (aq) + 2Na 3 PO 4 (aq) Fe 3 (PO 4 ) 2 (s) + 6NaCl(aq) Balanced ionic equation: 3Fe Cl + 6Na + + 2PO 4 3 Fe 3 (PO 4 ) 2 (s) + 6Na + + 6Cl Balanced net ionic equation: 3Fe PO 4 3 Fe 3 (PO 4 ) 2 (s) Double Replacement Reactions AcidBase Reactions A acid is a solution which dissolves in water to produce an excess of hydrogen ions. A base is a compound which dissolves in water to produce an excess of hydroxide ions. Usually acids contain hydrogen and produce hydrogen ions by dissociating. Bases can dissociate in water to produce hydroxide ions, OH. HCl H + + Cl HNO 3 H + + NO 3 H 2 SO 4 H + + HSO 4 NaOH Na + + OH KOH K + + OH Ca(OH) 2 Ca OH Some substances produce basic solutions by reacting with water. Na(s) + H 2 O Na + + OH + H 2 (g) MgO(s) + H 2 O Mg OH K 2 CO 3 (s) + H 2 O 2K + + 2OH + CO 2 (aq) When an acid reacts with a base (a compound that contains a hydroxide ion), water is produced. Water is a molecular liquid and does not dissociate into ions*. Water does NOT split apart into H + and OH. In an acidbase reaction water is the "insoluble product." Molecular equation: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) Ionic equation: H + + Cl + Na + + OH Na + + Cl + H 2 O(l) Net ionic equation: H + + OH H 2 O(l) The formation of water is the main reaction in an acid/base reaction. Consider the reaction between sulfuric acid and aluminum hydroxide: Molecular equation: Ionic equation: Net ionic equation 3H 2 SO 4 (aq) + 2Al(OH) 3 (s) Al 2 (SO 4 ) 3 (aq) + 6H 2 O(l) 3H + + HSO 4 + 2Al(OH) 3 (s) 2Al SO H 2 O(l) 3H + + HSO 4 + 2Al(OH) 3 (s) 2Al SO H 2 O(l) Sulfuric acid dissociates in water to make H + and HSO 4 ions. Aluminum hydroxide is insoluble in water and does not dissociate into ions. The net ionic equation is the same as the ionic equation since there are no spectator ions.
4 Exercise 1 Write balanced ionic and net ionic equations for the following reactions. 1. BaCl 2 (aq) + (NH 4 ) 2 CO 3 (aq) BaCO 3 (s) + 2NH 4 Cl(aq) 2. 2AgNO 3 (aq) + CuCl 2 (aq) 2AgCl(s) + Cu(NO 3 ) 2 (aq) 3. 3FeCl 2 (aq) + 2Na 3 PO 4 (aq) Fe 3 (PO 4 ) 2 (s) + 6NaCl(aq) 4. 2Fe(OH) 3 (s) + 3H 2 SO 4 (aq) Fe 2 (SO 4 ) 3 (aq) + 6HOH(l) Exercise 2. Predict the possible products of these double replacement reactions and write them to the right of the arrow. Use the solubility rules to predict whether the possible products are soluble in water. If there is no reaction, write NR and continue to the next problem. (You don t need to balance an equation if no reaction actually occurs.) Where there is an insoluble product and therefore, a reaction, balance the molecular equation and write the balanced net ionic equation in the space below. All of the reactants are soluble in water. Include the state symbols of the products: (s) or (l) for an insoluble solid or liquid; (aq) if it is in aqueous solution. 1. NaCl + AgNO 3 2. BaCl 2 + Na 2 CO 3 3. KNO 3 + LiCl 4. Pb(C 2 H 3 O 2 ) 2 + Cu(NO 3 ) 2
5 5. FeI 2 + NaCl 6. CaCl 2 + K 3 PO 4 7. CaCl 2 + Pb(NO 3 ) 2 8. Na 2 S + NH 4 Br 9. FeSO 4 + KOH 10. NaF + CaCl Cs 3 PO 4 + Pb(NO 3 ) HCl + Sr(OH) ZnCl 2 + Al(C 2 H 3 O 2 ) Cu(NO 3 ) 2 + NH 4 OH 15. Bi(NO 3 ) 3 + Na 2 SO 4
6 Chemistry Date Period Name Answers to Exercise 1: Double Replacement Reactions CW double replacement reactions doc 1. BaCl 2 (aq) + (NH 4 ) 2 CO 3 (aq) BaCO 3 (s) + 2 NH 4 Cl(aq) Ba Cl + 2 NH CO 3 BaCO 3 (s) + 2 NH Cl Ba CO 3 BaCO 3 (s) 2. 2 Fe(OH) 3 (s) + 3 H 2 SO 4 (aq) Fe 2 (SO 4 ) 3 (aq) + 6 HOH(l) 2Fe OH + 3 H HSO 4 2 Fe SO HOH(l) H + + OH HOH(l) HSO 4 + OH 2 HOH(l) + SO AgNO 3 (aq) + CuCl 2 (aq) 2 AgCl(s) + Cu(NO 3 ) 2 (aq) 2 Ag + 2 NO 3 + Cu Cl 2 AgCl(s) + Cu NO 3 Ag + + Cl AgCl(s) Sulfuric acid, H 2 SO 4 is a strong acid, which means that it dissociates completely, but it does not dissociate into 2H + and SO 4 2. It dissociates to form H + and HSO 4, the bisulfate ion, which is a weak acids. Weak acids do not completely dissociate in water. H 2 SO 4 H + + HSO 4 HSO 4 H + + SO FeCl 2 (aq) + 2 Na 3 PO 4 (aq) Fe 3 (PO 4 ) 2 (s) + 6 NaCl(aq) 3 Fe Cl + 6 Na PO 4 Fe 3 (PO 4 ) 2 (s) + 6 Na Cl 3 Fe PO 4 Fe 3 (PO 4 ) 2 (s) Answers to Exercise 2: 1. NaCl(aq) + AgNO 3 (aq) NaNO 3 (aq) + AgCl(s). (BAW) 2. BaCl 2 (aq) + Na 2 CO 3 (aq) BaCO 3 (s) + 2 NaCl (aq) 3. KNO 3 (aq) + LiCl(aq) NR.. KCl(aq) + LiNO 3 (aq) both soluble in water 4. Pb(C 2 H 3 O 2 ) 2 (aq) + Cu(NO 3 ) 2 (aq) NR. Pb(NO 3 ) 2 (aq) + Cu(C 2 H 3 O 2 ) 2 (aq) 5. FeI 2 (aq) + 2 NaCl(aq) NR. FeCl 2 aq) + NaI(aq) both soluble in water 6. 3 CaCl 2 (aq) + 2 K 3 PO 4 (aq) Ca 3 (PO 4 ) 2 (s) + 6 KCl(aq) 7. CaCl 2 (aq) + Pb(NO 3 ) 2 (aq) Ca(NO 3 ) 2 (aq) + PbCl 2 (s).. (BAW) 8. Na 2 S(aq) + NH 4 Br(aq) NR.. NaBr(aq) + (NH 4 ) 2 S(aq) both soluble in water 9. FeSO 4 (aq) + 2 KOH(aq) Fe(OH) 2 (s) + K 2 SO 4 (aq) NaF(aq) + CaCl 2 (aq) 2 NaCl(aq) + CaF 2 (s) Cs 3 PO 4 (aq) + 3 Pb(NO 3 ) 2 (aq) 6 CsNO 3 (aq) + Pb 3 (PO 4 ) 2 (s) HCl(aq) + Sr(OH) 2 (aq) 2 HOH(l) + SrCl 2 (aq) 13. ZnCl 2 (aq) + Al(C 2 H 3 O 2 ) 3 (aq) NR.. Zn(C 2 H 3 O 2 ) 2 (aq) + AlCl 3 (aq) both soluble in water 14. Cu(NO 3 ) 2 (aq) + 2 NH 4 OH(aq) Cu(OH) 2 (s) + 2 NH 4 NO 3 (aq) 15. Bi(NO 3 ) 3 (aq) + Na 2 SO 4 (aq) NR. Bi 2 (SO 4 ) 3 (aq) + NaNO 3 (aq) both soluble in water
Steps for balancing a chemical equation
The Chemical Equation: A Chemical Recipe Dr. Gergens - SD Mesa College A. Learn the meaning of these arrows. B. The chemical equation is the shorthand notation for a chemical reaction. A chemical equation
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationChapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction
Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,
More informationReactions in Aqueous Solution
CHAPTER 7 1. Water is the most universal of all liquids. Water has a relatively large heat capacity and a relatively large liquid range, which means it can absorb the heat liberated by many reactions while
More information2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )
TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationNET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:
NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants
More informationWriting, Balancing and Predicting Products of Chemical Reactions.
Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationChapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
More informationstoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
More informationExperiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
More informationUNIT (4) CALCULATIONS AND CHEMICAL REACTIONS
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More information4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes
Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the
More informationWriting Chemical Equations
Writing Chemical Equations Chemical equations for solution reactions can be written in three different forms; molecular l equations, complete ionic i equations, and net ionic equations. In class, so far,
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationChapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
More informationSolution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:
More informationTutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution.
T-27 Tutorial 4 SOLUTION STOICHIOMETRY Solution stoichiometry calculations involve chemical reactions taking place in solution. Of the various methods of expressing solution concentration the most convenient
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
More informationBalancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
More informationStoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
More informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationCommon Ion Effects. CH 3 CO 2 (aq) + Na + (aq)
Common Ion Effects If two reactions both involve the same ion, then one reaction can effect the equilibrium position of the other reaction. The ion that appears in both reactions is the common ion. Buffers
More informationTypes of Reactions. CHM 130LL: Chemical Reactions. Introduction. General Information
Introduction CHM 130LL: Chemical Reactions We often study chemistry to understand how and why chemicals (reactants) can be transformed into different chemicals (products) via a chemical reaction: Reactants
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationDepartment of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources
Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Introduction This document is intended to help you review the basics of writing
More informationWriting and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationExperiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
More informationH 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.
CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,
More informationAqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
More informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationChapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More informationChapter 5 Chemical Quantities and Reactions. Collection Terms. 5.1 The Mole. A Mole of a Compound. A Mole of Atoms.
Chapter 5 Chemical Quantities and Reactions 5.1 The Mole Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans 1
More informationMolarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationStoichiometry and Aqueous Reactions (Chapter 4)
Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationBalancing Chemical Equations Practice
Science Objectives Students will describe what reactants and products in a chemical equation mean. Students will explain the difference between coefficients and subscripts in chemical equations. Students
More information4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.
CHAPTER 9 1. The coefficients of the balanced chemical equation for a reaction give the relative numbers of molecules of reactants and products that are involved in the reaction.. The coefficients of the
More informationChapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
More informationChemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
More informationCHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
More informationMoles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
More informationMolar Mass Worksheet Answer Key
Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol
More informationNAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide
NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate
More information2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
More informationCHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
More informationChemical Reactions 2 The Chemical Equation
Chemical Reactions 2 The Chemical Equation INFORMATION Chemical equations are symbolic devices used to represent actual chemical reactions. The left side of the equation, called the reactants, is separated
More informationEXPERIMENT 8: Activity Series (Single Displacement Reactions)
EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete
More informationCHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS
1 CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS The Chemical Equation A chemical equation concisely shows the initial (reactants) and final (products) results of
More informationGeneral Chemistry II Chapter 20
1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water
More informationAnswers and Solutions to Text Problems
Chapter 7 Answers and Solutions 7 Answers and Solutions to Text Problems 7.1 A mole is the amount of a substance that contains 6.02 x 10 23 items. For example, one mole of water contains 6.02 10 23 molecules
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More informationPART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
More informationI N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
More informationBalancing Chemical Equations Worksheet Intermediate Level
Balancing Chemical Equations Worksheet Intermediate Level Neutralization Reactions Salts are produced by the action of acids. Salts are written metal first, then non-metal. Eg. NaCl not ClNa Acid + Base
More informationPhysical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
More informationChapter 6: Writing and Balancing Chemical Equations. AB A + B. CaCO3 CaO + CO2 A + B C. AB + C AC + B (or AB + C CB + A)
78 Chapter 6: Writing and Balancing Chemical Equations. It is convenient to classify chemical reactions into one of several general types. Some of the more common, important, reactions are shown below.
More informationREVIEW QUESTIONS Chapter 8
Chemistry 51 ANSWER KEY REVIEW QUESTIONS Chapter 8 1. Identify each of the diagrams below as strong electrolyte, weak electrolyte or non-electrolyte: (a) Non-electrolyte (no ions present) (b) Weak electrolyte
More informationChapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More informationAtomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
More informationAppendix D. Reaction Stoichiometry D.1 INTRODUCTION
Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules
More informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More informationTOPIC 11: Acids and Bases
TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationMOLARITY = (moles solute) / (vol.solution in liter units)
CHEM 101/105 Stoichiometry, as applied to Aqueous Solutions containing Ionic Solutes Lect-05 MOLES - a quantity of substance. Quantities of substances can be expressed as masses, as numbers, or as moles.
More informationYIELD YIELD REACTANTS PRODUCTS
Balancing Chemical Equations A Chemical Equation: is a representation of a chemical reaction in terms of chemical formulas Example: 1. Word Description of a Chemical Reaction When methane gas (CH 4 ) burns
More informationChemical Reactions. Section 9.1 Reactions and Equations pages 282 288 SOLUTIONS MANUAL. Practice Problems pages 284 287
CHAPTER 9 Chemical Reactions Section 9.1 Reactions and Equations pages 282 288 Practice Problems pages 284 287 Write skeleton equations for the following word equations. 1. Hydrogen and bromine gases react
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationChapter 4. Review Skills
Chapter 4 An Introduction to Chemical Reactions ow that you understand the basic structural differences between different kinds of substances, you are ready to begin learning about the chemical changes
More informationStoichiometry. Unit Outline
3 Stoichiometry Unit Outline 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis
More information4.1 Writing and Balancing Chemical Equations
176 Chapter 4 Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations By the end of this section, you will be able to: Derive chemical equations from narrative descriptions of
More informationSAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK
Solutions of Electrolytes and Nonelectrolytes SAMPLE PROBLEM 8.1 Indicate whether solutions of each of the following contain only ions, only molecules, or mostly molecules and a few ions: a. Na 2 SO 4,
More informationNumber of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
More information= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
More informationCHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
More informationChemistry Ch 15 (Solutions) Study Guide Introduction
Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual
More informationLiquid phase. Balance equation Moles A Stoic. coefficient. Aqueous phase
STOICHIOMETRY Objective The purpose of this exercise is to give you some practice on some Stoichiometry calculations. Discussion The molecular mass of a compound is the sum of the atomic masses of all
More informationSanta Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationChapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
More informationCHEMISTRY COMPUTING FORMULA MASS WORKSHEET
CHEMISTRY COMPUTING FORMULA MASS WORKSHEET Directions: Find the formula mass of the following compounds. Round atomic masses to the tenth of a decimal place. Place your final answer in the FORMULA MASS
More informationTopic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
More informationSolubility of Salts - Ksp. Ksp Solubility
Solubility of Salts - Ksp We now focus on another aqueous equilibrium system, slightly soluble salts. These salts have a Solubility Product Constant, K sp. (We saw this in 1B with the sodium tetraborate
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationGeneral Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
More informationWRITING CHEMICAL FORMULA
WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.
More informationCopyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.
Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of
More informationWord Equations and Balancing Equations. Video Notes
Word Equations and Balancing Equations Video Notes In this lesson, you will: Use the law of conservation of mass and provide standard rules for writing and balancing equations. Write and balance equations
More informationMonatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
More informationDecomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
More informationSolubility Product Constant
Solubility Product Constant Page 1 In general, when ionic compounds dissolve in water, they go into solution as ions. When the solution becomes saturated with ions, that is, unable to hold any more, the
More information