Chemistry 132 NT. Solubility Equilibria. The most difficult thing to understand is the income tax. Solubility and Complex-ion Equilibria
|
|
|
- Paula Potter
- 7 years ago
- Views:
Transcription
1 Chemistry 13 NT The most difficult thing to understand is the income tax. Albert Einstein 1 Chem 13 NT Solubility and Complex-ion Equilibria Module 1 Solubility Equilibria The Solubility Product Constant Solubility and the Common-Ion Effect Precipitation Calculations Effect of ph on Solubility Reaction of zinc metal with hydrochloric acid. Solubility Equilibria Many natural processes depend on the precipitation or dissolving of a slightly soluble salt. In the next section, we look at the equilibria of slightly soluble, or nearly insoluble, ionic compounds. Their equilibrium constants can be used to answer questions regarding solubility and precipitation. 3 1
2 The Solubility Product Constant When an excess of a slightly soluble ionic compound is mixed with water, an equilibrium is established between the solid and the ions in the saturated solution. For the salt calcium oxalate, CaC O, you have the following equilibrium. CaC O (s) H O Ca + + C O - The Solubility Product Constant When an excess of a slightly soluble ionic compound is mixed with water, an equilibrium is established between the solid and the ions in the saturated solution. The equilibrium constant for this process is called the solubility product constant. sp = [Ca + ][C O - ] 5 The Solubility Product Constant In general, the solubility product constant is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound. It equals the product of the equilibrium concentrations of the ions in the compound. Each concentration is raised to a power equal to the number of such ions in the formula of the compound. 6
![sp = [Ca + ][C O - ] 5 The Solubility Product Constant In general, the solubility product constant is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly](/docs-images/47/20640459/images/page_2.jpg "insoluble) ionic compound. It equals the product of the equilibrium concentrations of the ions in the compound.")
3 The Solubility Product Constant In general, the solubility product constant is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound. For example, lead iodide, PbI, is another slightly soluble salt. Its equilibrium is: PbI (s) H O Pb + + I - 7 The Solubility Product Constant In general, the solubility product constant is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound. The expression for the solubility product constant is: + - sp = [Pb ][I ] 8 Calculating sp from the Solubility A 1.0-L sample of a saturated calcium oxalate solution, CaC O, contains g of the salt at 5 o C. Calculate the sp for this salt at 5 o C. We must first convert the solubility of calcium oxalate from g/liter to moles per liter. 1molCaCO M CaC O = (0.0061g CaCO / L) 18g CaC O -5 =.8 molcaco / L 9 3
![Its equilibrium is: PbI (s) H O Pb + + I - 7 The expression for the solubility product constant is: + - sp = [Pb ][I ] 8 Calculating sp from the Solubility A 1.](/docs-images/47/20640459/images/page_3.jpg "0-L sample of a saturated calcium oxalate solution, CaC O, contains 0.0061-g of the salt at 5 o C. Calculate the sp for this salt at 5 o C.")
4 Calculating sp from the Solubility A 1.0-L sample of a saturated calcium oxalate solution, CaC O, contains g of the salt at 5 o C. Calculate the sp for this salt at 5 o C. When.8 x -5 mol of solid dissolve it forms.8 x -5 mol of each ion. Starting Change Equilibrium CaC O (s) H O + - Ca + C O x -5.8 x x -5.8 x -5 Calculating sp from the Solubility A 1.0-L sample of a saturated calcium oxalate solution, CaC O, contains g of the salt at 5 o C. Calculate the sp for this salt at 5 o C. You can now substitute into the equilibriumconstant expression. + - sp = [Ca ][CO ] sp = ( sp =.3 )(.8-5 ) 11 Calculating sp from the Solubility By experiment, it is found that 1. x -3 mol of lead(ii) iodide, PbI, dissolves in 1.0 L of water at 5 o C. What is the sp at this temperature? Note that in this example, you find that 1. x -3 mol of the solid dissolves to give 1. x -3 mol Pb + and ( x (1. x -3 )) mol of I -. 1
5 Calculating sp from the Solubility By experiment, it is found that 1. x -3 mol of lead(ii) iodide, PbI, dissolves in 1.0 L of water at 5 o C. What is the sp at this temperature? The following table summarizes. Starting Change Equilibrium PbI (s) H O Pb + + I x -3 + x (1. x -3) 1. x -3 x (1. x -3) - 13 Calculating sp from the Solubility By experiment, it is found that 1. x -3 mol of lead(ii) iodide, PbI, dissolves in 1.0 L of water at 5 o C. What is the sp at this temperature? Substituting into the equilibrium-constant expression: + - sp = [Pb ][I ] -3-3 sp = (1. )( (1. )) -9 sp = Calculating sp from the Solubility By experiment, it is found that 1. x -3 mol of lead(ii) iodide, PbI, dissolves in 1.0 L of water at 5 o C. What is the sp at this temperature? A table in your text lists the solubility product constants for various ionic compounds. If the solubility product constant is known, the solubility of the compound can be calculated. 15 5
![x -3) - 13 Substituting into the equilibrium-constant expression: + - sp = [Pb ][I ] -3-3 sp = (1. )( (1. )) -9 sp = 6.](/docs-images/47/20640459/images/page_5.jpg "9 1 A table in your text lists the solubility product constants for various ionic compounds. If the solubility product constant is known, the solubility of the compound can be calculated. 15 5")
6 Calculating the Solubility from sp The mineral fluorite is calcium fluoride, CaF. Calculate the solubility (in grams per liter) of calcium fluoride in water from the sp (3. x -11 ) Let x be the molar solubility of CaF. H CaF (s) O + Ca Starting Change Equilibrium + F x +x x x 16 Calculating the Solubility from sp The mineral fluorite is calcium fluoride, CaF. Calculate the solubility (in grams per liter) of calcium fluoride in water from the sp (3. x -11 ) You substitute into the equilibrium-constant equation + - [Ca ][F ] = sp (x)(x) x 3 = 3. = Calculating the Solubility from sp The mineral fluorite is calcium fluoride, CaF. Calculate the solubility (in grams per liter) of calcium fluoride in water from the sp (3. x -11 ) You now solve for x x 3 - = =.0 mol CaF /L 18 6
![H CaF (s) O + Ca Starting Change Equilibrium + F - 0 0 +x +x x x 16 x -11 ) You substitute into the equilibrium-constant equation + - [Ca ][F ] = sp (x)(x) x 3 = 3.](/docs-images/47/20640459/images/page_6.jpg "= 3. -11-11 17 x -11 ) You now solve for x. -11 3. x 3 - = =.0 mol CaF /L 18 6")
7 Calculating the Solubility from sp The mineral fluorite is calcium fluoride, CaF. Calculate the solubility (in grams per liter) of calcium fluoride in water from the sp (3. x -11 ) Convert to g/l (CaF 78.1 g/mol). - solubility =.0 mol/ L - = 1.6 g CaF /L 78.1g CaF 1 mol CaF 19 Solubility and the Common-Ion Effect In this section we will look at calculating solubilities in the presence of other ions. The importance of the sp becomes apparent when you consider the solubility of one salt in the solution of another having the same cation. 0 Solubility and the Common-Ion Effect In this section we will look at calculating solubilities in the presence of other ions. For example, suppose you wish to know the solubility of calcium oxalate in a solution of calcium chloride. Each salt contributes the same cation (Ca + ) The effect is to make calcium oxalate less soluble than it would be in pure water. 1 7
8 A Problem To Consider What is the molar solubility of calcium oxalate in 0.15 M calcium chloride? The sp for calcium oxalate is.3 x -9. Note that before the calcium oxalate dissolves, there is already 0.15 M Ca + in the solution. Starting Change Equilibrium CaC O (s) H O + - Ca + C O x +x x x A Problem To Consider What is the molar solubility of calcium oxalate in 0.15 M calcium chloride? The sp for calcium oxalate is.3 x -9. You substitute into the equilibrium-constant equation + - [Ca ][CO ] = sp ( x)(x) = A Problem To Consider What is the molar solubility of calcium oxalate in 0.15 M calcium chloride? The sp for calcium oxalate is.3 x -9. Now rearrange this equation to give -9.3 x = We expect x to be negligible compared to
![15 + x x You substitute into the equilibrium-constant equation + - [Ca ][CO ] = sp (0.15 + x)(x) =.3-9 3 Now rearrange this equation to give -9.3 x = 0.15 + x.3 @ 0.](/docs-images/47/20640459/images/page_8.jpg "15 We expect x to be negligible compared to 0.15. -9 8")
9 A Problem To Consider What is the molar solubility of calcium oxalate in 0.15 M calcium chloride? The sp for calcium oxalate is.3 x -9. Now rearrange this equation to give -.3 x = x x = A Problem To Consider What is the molar solubility of calcium oxalate in 0.15 M calcium chloride? The sp for calcium oxalate is.3 x -9. Therefore, the molar solubility of calcium oxalate in 0.15 M CaCl is 1.5 x -8 M. In pure water, the molarity was.8 x -5 M, which is over 3000 times greater. 6 Precipitation Calculations Precipitation is merely another way of looking at solubility equilibrium. Rather than considering how much of a substance will dissolve, we ask:will precipitation occur for a given starting ion concentration? 7 9
10 Criteria for Precipitation To determine whether an equilibrium system will go in the forward or reverse direction requires that we evaluate the reaction quotient, Q c. To predict the direction of reaction, you compare Q c with c (Equilibrium Chapter). The reaction quotient has the same form as the sp expression, but the concentrations of products are starting values. 8 Criteria for Precipitation To determine whether an equilibrium system will go in the forward or reverse direction requires that we evaluate the reaction quotient, Q c. Consider the following equilibrium. PbCl (s) H O Pb + + Cl - 9 Criteria for Precipitation To determine whether an equilibrium system will go in the forward or reverse direction requires that we evaluate the reaction quotient, Q c. The Q c expression is Q + - c = [Pb ] i [Cl ] i where initial concentration is denoted by i. 30
11 Criteria for Precipitation To determine whether an equilibrium system will go in the forward or reverse direction requires that we evaluate the reaction quotient, Q c. If Q c exceeds the sp, precipitation occurs. If Q c is less than sp, more solute can dissolve. If Q c equals the sp, the solution is saturated. 31 Predicting Whether Precipitation Will Occur The concentration of calcium ion in blood plasma is M. If the concentration of oxalate ion is 1.0 x -7 M, do you expect calcium oxalate to precipitate? sp for calcium oxalate is.3 x -9. The ion product quotient, Q c, is: + Q = [Ca c - i [CO ] i ] Qc = (0.005) (1.0 Q c = ) 3 Predicting Whether Precipitation Will Occur The concentration of calcium ion in blood plasma is M. If the concentration of oxalate ion is 1.0 x -7 M, do you expect calcium oxalate to precipitate? sp for calcium oxalate is.3 x -9. This value is smaller than the sp, so you do not expect precipitation to occur. - Q c =.5 < sp 33 11
12 Fractional Precipitation Fractional precipitation is the technique of separating two or more ions from a solution by adding a reactant that precipitates first one ion, then another, and so forth. For example, when you slowly add potassium chromate, CrO, to a solution containing Ba + and Sr +, barium chromate precipitates first. 3 Fractional Precipitation Fractional precipitation is the technique of separating two or more ions from a solution by adding a reactant that precipitates first one ion, then another, and so forth. After most of the Ba + ion has precipitated, strontium chromate begins to precipitate. It is therefore possible to separate Ba + from Sr + by fractional precipitation using CrO. 35 Effect of ph on Solubility Sometimes it is necessary to account for other reactions aqueous ions might undergo. For example, if the anion is the conjugate base of a weak acid, it will react with H 3 O +. You should expect the solubility to be affected by ph. 36 1
13 Effect of ph on Solubility Sometimes it is necessary to account for other reactions aqueous ions might undergo. Consider the following equilibrium. CaC O (s) H O Ca + + C O - Because the oxalate ion is conjugate to a weak acid (HC O - ), it will react with H 3 O +. - H O + C O + H3O HCO + HO(l) - 37 Effect of ph on Solubility Sometimes it is necessary to account for other reactions aqueous ions might undergo. According to Le Chatelier s principle, as C O - ion is removed by the reaction with H 3 O +, more calcium oxalate dissolves. Therefore, you expect calcium oxalate to be more soluble in acidic solution (low ph) than in pure water. 38 Separation of Metal Ions by Sulfide Precipitation Many metal sulfides are insoluble in water but dissolve in acidic solution. Qualitative analysis uses this change in solubility of the metal sulfides with ph to separate a mixture of metal ions. By adjusting the ph in an aqueous solution of H S, you adjust the sulfide concentration to precipitate the least soluble metal sulfide first. Qualitative analysis is covered in your text
14 Operational Skills Writing solubility product expressions Calculating sp from the solubility, or vice versa. Calculating the solubility of a slightly soluble salt in a solution of a common ion. Predicting whether precipitation will occur Determining the qualitative effect of ph on solubility Time for a few review questions 0 1 1
Solubility 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
General 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
Copyright 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
MOLARITY = (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.
Solubility 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
Solubility Product. Application of Equilibrium concepts
Solubility Product Application of Equilibrium concepts Introduction In even the most insoluble compounds, a few ions at the least dissolve. We can treat dissolving as a mini reaction in which the cation(s)
Solution 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:
Molarity 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.
Chemistry 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
Chapter 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
IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
Common 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
Experiment 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
Number 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
Name: 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
Chemistry 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
stoichiometry = 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
Chemical 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
UNIT (6) ACIDS AND BASES
UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that
6 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
Equilibrium Constants The following equilibrium constants will be useful for some of the problems.
1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO
An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
ph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
Experiment 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
Chapter 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
CHEMICAL 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,
APPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
CHEM 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
Chapter 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
Aqueous 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
Experiment 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
SAMPLE 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,
Aqueous 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
Tutorial 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
Success criteria You should be able to write the correct formula for any ionic compound
Chemical Formulas and Names of Ionic Compounds WHY? Going back to pre-historic times, humans have experimented with chemical processes that helped them to make better tools, pottery and weapons. In the
Answer Key, Problem Set 5 (With explanations)--complete
Chemistry 122 Mines, Spring 2016 Answer Key, Problem Set 5 (With explanations)complete 1. NT1; 2. NT2; 3. MP; 4. MP (15.38); 5. MP (15.40); 6. MP (15.42); 7. NT3; 8. NT4; 9. MP; 10. NT5; 11. NT6; 12. MP;
Stoichiometry 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.
Chapter 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
Properties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases
CAPTER Acids, Bases and Salts Properties of Aqueous Solutions of Acids and Bases Strong and Weak Acids Acids are substances that generate in aqueous solutions. Strong acids ionize 0% in water. That is,
Chemistry 106 Fall 2007 Exam 3 1. Which one of the following salts will form a neutral solution on dissolving in water?
1. Which one of the following salts will form a neutral solution on dissolving in water? A. NaCN B. NH 4 NO 3 C. NaCl D. KNO 2 E. FeCl 3 2. Which one of the following is a buffer solution? A. 0.10 M KCN
Chapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
Equilibria Involving Acids & Bases
Week 9 Equilibria Involving Acids & Bases Acidic and basic solutions Self-ionisation of water Through reaction with itself: The concentration of water in aqueous solutions is virtually constant at about
One problem often faced in qualitative analysis is to test for one ion in a
Chemistry 112 Laboratory: Silver Group Analysis Page 11 ANALYSIS OF THE SILVER GROUP CATIONS Ag + Pb Analysis of a Mixture of Cations One problem often faced in qualitative analysis is to test for one
Chemical 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.
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
80. Testing salts for anions and cations
Classic chemistry experiments 203 80. Testing salts for anions and cations Topic Qualitative analysis. Timing Description 12 hours. Students attempt to identify the anions and cations present in a salt
AP CHEMISTRY 2013 SCORING GUIDELINES
AP CHEMISTRY 2013 SCORING GUIDELINES Question 4 (15 points) For each of the following three reactions, write a balanced equation for the reaction in part (i) and answer the question about the reaction
1. 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
1. 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)
Chemical 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
Practical Lesson No 4 TITRATIONS
Practical Lesson No 4 TITRATIONS Reagents: 1. NaOH standard solution 0.1 mol/l 2. H 2 SO 4 solution of unknown concentration 3. Phenolphthalein 4. Na 2 S 2 O 3 standard solution 0.1 mol/l 5. Starch solution
Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
Chem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
Chem 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
Unit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find
Colligative Properties
CH302 LaBrake and Vanden Bout Colligative Properties PROBLEM #1: Give the molecular formula, the van t hoff factor for the following Ionic Compounds as well as guess the solubility of the compounds. If
CHM1 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
Experiment 16-Acids, Bases and ph
Definitions acid-an ionic compound that releases or reacts with water to form hydrogen ion (H + ) in aqueous solution. They taste sour and turn litmus red. Acids react with certain metals such as zinc,
Name period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
Unit 4 Conservation of Mass and Stoichiometry
9.1 Naming Ions I. Monatomic Ions A. Monatomic ions 1. Ions formed from a single atom Unit 4 Conservation of Mass and Stoichiometry B. Naming Monatomic Ions 1. Monatomic cations are a. Identified by the
ATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
n molarity = M = N.B.: n = litres (solution)
1. CONCENTRATION UNITS A solution is a homogeneous mixture of two or more chemical substances. If we have a solution made from a solid and a liquid, we say that the solid is dissolved in the liquid and
HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
PART 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
Chemistry 12 Tutorial 10 Ksp Calculations
Chemistry 12 Tutorial 10 Ksp Calculations Welcome back to the world of calculations. In Tutorial 10 you will be shown: 1. What is meant by Ksp. 2. How to write a "Ksp expression" from a net ionic equation.
Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
Chapter 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
NET 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
MOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
Chapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
W1 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
Complexometric Titrations
Complexometric Titrations Complexometric titrations are based on the formation of a soluble complex upon the reaction of the species titrated with the titrant. M + L ML In the module Chemistry 2 you were
SCH 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
Chapter 14 - Acids and Bases
Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry
Appendix 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
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS Purpose: It is important for chemists to be able to determine the composition of unknown chemicals. This can often be done by way of chemical tests.
Santa 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
REVIEW 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
CHEMISTRY II FINAL EXAM REVIEW
Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas
Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50
Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs
UNIT (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
Chapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND
#3. Acid - Base Titrations 27 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric
Unit 7 Stoichiometry. Chapter 12
Unit 7 Stoichiometry Chapter 12 Objectives 7.1 use stoichiometry to determine the amount of substance in a reaction 7.2 determine the limiting reactant of a reaction 7.3 determine the percent yield of
Chemistry Assessment Unit AS 1
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]
H 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,
Acid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!!
Acid/Base Reactions some covalent compounds have weakly bound H atoms and can lose them to water (acids) some compounds produce OH in water solutions when they dissolve (bases) acid/base reaction are very
2. 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
EXPERIMENT 7 Reaction Stoichiometry and Percent Yield
EXPERIMENT 7 Reaction Stoichiometry and Percent Yield INTRODUCTION Stoichiometry calculations are about calculating the amounts of substances that react and form in a chemical reaction. The word stoichiometry
Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-
AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +
Aqueous Chemical Reactions
Name: Date: Lab Partners: Lab section: Aqueous Chemical Reactions The purpose of this lab is to introduce you to three major categories of reactions that occur in aqueous solutions: precipitation reactions,
Chemistry: 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,
Chemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
Chapter 14 Solutions
Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute
4.1 Stoichiometry. 3 Basic Steps. 4. Stoichiometry. Stoichiometry. Butane Lighter 2C 4 H 10 + 13O 2 10H 2 O + 8CO 2
4. Stoichiometry 1. Stoichiometric Equations 2. Limiting Reagent Problems 3. Percent Yield 4. Limiting Reagent Problems 5. Concentrations of Solutes 6. Solution Stoichiometry 7. ph and Acid Base Titrations
6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must
AP Chemistry 2006 Free-Response Questions
AP Chemistry 006 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college
Chemistry 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
Formulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be