Lect. 2: Chemical Water Quality
|
|
- Bruno Green
- 6 years ago
- Views:
Transcription
1 The Islamic University of Gaza Faculty of Engineering Civil Engineering Department M.Sc. Water Resources Water Quality Management (ENGC 6304) Lect. 2: Chemical Water Quality ١
2 Chemical water quality parameters Water is called a universal Solvent Chemical parameters of water are: 1. Total dissolved solids, 2. Alkalinity, 3. Hardness, 4. Fluorides, 5. Metals, 6. Organics, 7. Nutrients. ٢
3 Chemistry of solutions Atom the smallest unit of element Molecules of elements or compounds are constructed of atoms. H + H H 2 H 2 + O H 2O Molecular mass is the sum of the atomic mass of all atoms in molecule For example : Atomic mass of oxygen (O) = 16, for Hydrogen (H) =1 Molecular mass for water (H 2 O) =18 ٣
4 A mole of an element or compound is its molecular mass in gm. For example : one mole of oxygen (O 2 ) = 32, water (H 2 O) =18 One mole of a substance dissolved in sufficient water to make one liter of solution is called a one molar solution. The charged species is called ions. Produced when compounds dissociate in water. +ve ions called cations, -ve ions called anions Neutrality means the number of cations = the number of anions. NaCl Na + + Cl ٤
5 The valence is the number of charges on an ion. The valence of (Na + )=1, The valence of (Cl - )=1 The equivalence of an element is the number of hydrogen atoms that element can hold in combination or can replace in a reaction (= valence in most cases) An equivalent of an element is its gram molecular mass (mole) divided by its equivalence. A milliequivalent of an element is its milligrams molecular mass divided by its equivalence. ٥
6 Example How many grams of calcium will be required to combine with 90 g of carbonate to form calcium carbonate? Solution: 1- One equivalent of Carbonate (CO 3 2- ) = equivalent mass equivalence = (16) 2 = 30g / equiv One equivalent of Calcium(Ca 2+ ) = = 20g / equiv 2 3- The no. of equivalents of Carbonate must equal to the no. of equivalents of calcium. 4- No. of equivalents of calcium equiv ٦ 90g = 30g / equiv = 3 5- So, we need 3 equiv of carbonate = 3 equiv X 20 g/equiv = 60 g.
7 The concentration of substance A can be expressed as an equivalent concentration to substance B as the following: ( g / L) A ( g / equiv) A ( g / equiv) B = ( g / L) A exp ressed as B Generally, the constituents of dissolved solids are reported in terms of equivalent calcium carbonate concentrations ٧
8 Example What is the equivalent calcium carbonate concentration of: 117 mg/l of NaCl? 2x10-3 mol/l of NaCl? 1- One equivalent of Calcium Carbonate (CaCO 3 ) equivalent mass (16) = = = 50g / equiv equivalence One equivalent of Sodium Chloride (NaCl) = = 58.5g / equiv 1 117( mg / L) NaCl 58.5( g / equiv) A 50( g / equiv) CaCo = mg L 3 100( / ) NaCl as CaCo 3 ٨ 3- One mole of a substance divided by its valence is one equivalent mol / L 1mol / equiv thus, = equiv / L equiv / L 50( g / equiv) CaCo 3 = 100( mg / L) NaCl as CaCo 3
9 Ionization of solids substances with crystalline structure Water is a reactant CaO H O Ca OH Water is not a reactant NaCl + H O Na + Cl + H O Dissolution : the solid form may be dissociated into its ionic component ٩ Precipitation: the ionic components may be recombining into the solid form.
10 Dynamic Equilibrium is reached when the rate of dissolution and the rate of precipitation is exactly equal. Mass action equation A x B y xa y + + yb x Solid compound Ionic components [ A] [ A x x [ B] B y ] y = K K is an equilibrium constant for a given substance in pure water at given temperature The brackets [ ] indicate molar concentration. ١٠
11 EQUILIBRIUM SYSTEMS RATE OF DISSOLUTION = RATE OF PRECIPITATION ١١
12 At equilibrium, the solid phase does not change concentration (precipitation = dissolution) [ Ax By ] = K s = const [ x y A ] [ B] = KK s = K sp Where K sp is the solubility product. If the concentration of either or both of the ions is increased, the product of the ionic concentration will exceed the K sp and precipitation will occur to maintain the equilibrium conditions. ١٢ See table 2-3 (solubility product values)
13 ١٣ SOLUBILITY PRODUCTS OF SOME COMMON SALTS AT 25 0 C
14 For example: Ca 3 (PO 4 ) 2 3Ca PO 4 3- The products of ionic concentrations of both ions is always a constant for a given compound at a given temperature, i.e. [Ca 2+ ] 3 [PO 4 3- ] 2 = 1x10-27 = Ksp = constant What Does Solubility Product (ksp) Mean?? 1. When [A] x [B] y < Ksp, the compound continue to dissociate and the solubilization continue to take place until [A + ] a [B - ] b = Ksp 2. When [A] x [B] y > Ksp, the compound will start to precipitate ١٤
15 Based on Ks value, we can actually calculate the solubility of any particular compound BaSO 4 Ba 2+ + SO 4 2- The no. of moles of Ba 2+ resulting from dissociation = x, and there are x moles of SO 4 2-, Then there are x moles of solid (BaSO 4 ) [Ba 2+ ] [SO 4 2- ] = (x). (x) = x 2 = Ksp = 1 x (table 2-3) x = 1x10-5 Therefore, the solubility of BaSO 4 is 1x10-5 M. CaF 2 Ca F - The no. of moles of Ca 2+ resulting from dissociation = x, and there are 2x moles of F -, Then there is x moles of solid (CaF 2 ) [Ca 2+ ] [F - ] 2 = (x) (2x) 2 = Ksp = 3 x x = 1.96x10-4 The solubility of CaF 2 is 1.96x10-4 M. ١٥
16 Example: Calculating Concentrations From Ksp Find the concentration of dissolved Al(OH) 3 in a saturated solution. Given: Ksp = 1.0 x Al(OH) 3 Al OH - Solution : Ksp = [Al +3 ]. [OH - ] 3 Each mole dissolved Al(OH) 3 gives one mole Al +3 and three moles OH - ions therefore, if [Al +3 ] = X, [OH - ] = 3X and Ksp = X. (3X) 3 = 27 X 4 = 1.0 x X = (1.0 x / 27) 1/4 = 4.4 x 10-9 M ١٦
17 Example The solubility product for the dissociation of Mg(OH) 2 is 9x Determine the concentration of Mg 2+ and OH - at equilibrium, Solution: Mg( OH ) [ Mg 2+ 2 ][ OH ] Mg 2 2+ = OH 12 The no of moles of Mg 2+ resulting from dissociation = x, Then there are 2x moles of OH - ١٧ x = x = mol / L x.(2x) ( Mg) mol / L ( OH ) 2 =
18 Total Dissolved solids The material remaining in the water after filtration for the suspended solid analysis is considered to be dissolved solids. Source Results from the solvent action of water on solids, liquids, and gases. Inorganic dissolved solids; minerals, metals, gases. Organic ; decay products of vegetation, organic chemicals and gases. ١٨
19 Impacts Produce tastes, colors, and odor, Some chemicals are toxic or carcinogenic, Some dissolved solids may combine to form a compound of more dangerous than the original materials, Not all dissolved solids are undesirable. Measurement See sec. 2-2 Suspended Solids By measuring the electrical conductivity of the water, Conductivity measures the ability of water to conduct an electrical current. ١٩
20 Conductivity is a good way to determine the ionic strength of water because the ability of water to conduct a current is proportional to the number of ions in the water Freshwater generally has low conductivity measured in microsiemens (us) Marine systems have much higher conductivity measured in millisiemens (ms) which can easily be converted to salinity Humans and other terrestrial animals require fresh water for survival as do plants and animals normally found in freshwater Use TDS parameter is important in the analysis of water and wastewater to know more about the composition of the solids in water ٢٠
21 Ion Balance The dissolved solids content of natural water is classified to: Major constituents (1-1000mg/L) sodium (Na + ), calcium (Ca 2+ ), magnesium (Mg 2+ ), bicarbonate (HCO3 - ), sulfate (SO4 2- ), chloride (CL - ) - Called common ions, - Measured individually and summed on an equivalent basis to represent the approximate TDS, - The sum of anions must equal the sum of cations (as a check) Secondary constituents..( mg/l). Iron, potassium, carbonate, nitrate, fluoride, boron, silica ٢١
22 Testing for ion balance The results of common ions for a sample of water are shown below, If 10% error in the balance is acceptable, should the analysis be considered complete? sodium (Na + ) = 98mg/L, calcium (Ca 2+ ) =55mg/L, magnesium (Mg 2+ )= 18mg/L, bicarbonate (HCO3 - )= 250mg/L, sulfate (SO4 2- ) =60mg/L, chloride (CL - ) = 89 mg/l ٢٢
23 Ion Concentration (mg/l) Equiv, (mg/mequiv) Equiv conc, (mequiv/l) (Na + ) 98 23/ (Ca 2+ ) 55 40/ (Mg 2+ ) / (HCO 3- ) /1 4.1 (SO 4 2- ) 60 96/ (CL - ) / ٢٣
24 Calculate the percent of error = ( )*100/7.86= 8% < 10%. Accept analysis (Ca 2+ ) (Mg 2+ ) (Na + ) (HCO 3- ) (SO 4 2- ) (CL - ) Bar diagram ٢٤
AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationMay 09, Ksp.notebook. Ksp = [Li + ] [F + ] Find the Ksp for the above reaction.
example: Constant Product K sp Solubility Product Constant Some compounds dissolve in water Some compounds dissolve better than others The more that a compound can dissolve, the more soluble the compound
More informationV(STP) No.of mequivalents = n. Analytical chemistry
Analytical chemistry 1-qualitative analysis. Is concerned with the identification of ions molecules elements and compounds present in sample 2- Quantitative analysis :- Is concerned with the Determination
More informationSolubility and Complex Ion Equilibria
Solubility and Complex Ion Equilibria a mineral formed by marine organisms through biological precipitation CALCITE CaCO 3(s) Ca + (aq)+ CO 3 - (aq) K K sp [Ca + ][CO 3 - ].8 x 10-9 K sp solubility product
More informationSolubility and Complex Ion Equilibria
CALCITE Solubility and Complex Ion Equilibria a mineral formed by marine organisms through biological precipitation CaCO (s) Ca + (aq)+ CO (aq) K K sp [Ca + ][CO ].8 x 10-9 K sp solubility product constant
More informationPart A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
More informationSolutions Solubility. Chapter 14
Copyright 2004 by Houghton Mifflin Company. Solutions Chapter 14 All rights reserved. 1 Solutions Solutions are homogeneous mixtures Solvent substance present in the largest amount Solute is the dissolved
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 17 Additional Aspects of James F. Kirby Quinnipiac University Hamden, CT Effect of Acetate on the Acetic Acid Equilibrium Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq)
More informationSolubility Equilibria
Solubility Equilibria Heretofore, we have investigated gas pressure, solution, acidbase equilibriums. Another important equilibrium that is used in the chemistry lab is that of solubility equilibrium.
More informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More information1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)
Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca
More informationIONIC CHARGES. Chemistry 51 Review
IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from
More informationSolubility Equilibrium
2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationSolubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization
Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3
More informationWe CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit.
Solubility Equilibrium The Basics (should be mostly review) Solubility is defined as the maximum amount of a substance which can be dissolved in a given solute at a given temperature. The solubility of
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationCHEM J-6 June 2014
CHEM1102 2014-J-6 June 2014 A solution is prepared that contains sodium chloride and sodium chromate (both 0.10 M). When a concentrated solution of silver nitrate is added slowly, white AgCl(s) begins
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More informationIII.1 SOLUBILITY CONCEPT REVIEW
III.1 SOLUBILITY CONCEPT REVIEW Read Hebden p. 73 76 and review basic solubility definitions. Soluble means Insoluble means The Dissolving Process IONIC Solutions MOLECULAR Solutions (Covalent compounds)
More informationWhat is the ph of a 0.25 M solution of acetic acid (K a = 1.8 x 10-5 )?
1 of 17 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationChapter 16: Applications of Aqueous Equilibrium Part 3. Solubilities of Ionic Compounds and K sp
Chapter 16: Applications of Aqueous Equilibrium Part 3 Solubilities of Ionic Compounds and K sp You ve already learned that not all ionic compounds are water soluble. You memorized the solubility rules
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationReference: Chapter 4 in textbook. PART 6B Precipitate. textbook
PART 6A Solution Reference: Chapter 4 in textbook PART 6B Precipitate Reference: Chapter 16.5 16.8 in the textbook 1 Solution Solute, Solvent, and Solution Saturated solution and Solubility Saturated solution:
More informationStoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change.
Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. In order to do this, we need to be able to talk about numbers of atoms. The key concept is
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationUnit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
More informationPart One: Solubility Equilibria. Insoluble and slightly soluble compounds are important in nature and commercially.
CHAPTER 17: SOLUBILITY AND COMPLEX ION EQUILIBRIA Part One: Solubility Equilibria A. Ksp, the Solubility Product Constant. (Section 17.1) 1. Review the solubility rules. (Table 4.1) 2. Insoluble and slightly
More informationCh 17 Solubility Equilibria. Brown & LeMay
Ch 17 Solubility Equilibria Brown & LeMay When a typical ionic solid is dissolved in water that dissolved material can be assumed to be present as separate hydrated anions & cations. For example: CaF 2
More informationCalifornia Standards Test (CST) Practice
California Standards Test (CST) Practice 1. Which element has properties most like those of magnesium? (a) calcium (b) potassium (c) cesium (d) sodium 5. Which pair of atoms will share electrons when a
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationSolubility Equilibria
Chapter 17 SOLUBILITY EQUILIBRIA (Part II) Dr. Al Saadi 1 Solubility Equilibria The concept of chemical equilibrium helps to predict how much of a specific ionic compound (salt) will dissolve in water.
More informationSolubility and Complex Ion. Equilibria
Solubility and Complex Ion a mineral formed by marine organisms through biological precipitation CALCITE Equilibria CaCO 3(s) Ca 2+ (aq) + CO 3 2- (aq) K = K sp = [Ca 2+ ][CO 3 2- ] = 2.8 x 10-9 K sp =
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationProperties of Compounds
Chapter 6. Properties of Compounds Comparing properties of elements and compounds Compounds are formed when elements combine together in fixed proportions. The compound formed will often have properties
More informationLearning Outcomes: At the end of this assignment, students will be able to:
Chemical Equilibria & Sample Preparation Purpose: The purpose of this assignment is to predict how solute concentrations are controlled by chemical equilibria, understand the chemistry involved with sample
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationNaOH + HCl ---> NaCl + H 2 O
EXERCISES, LESSON 2 INSTRUCTIONS. Write the word, words, symbols, or numbers that properly completes the statement in the space provided or mark the correct word/phrase from those given. After you complete
More information5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3
Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice:
More informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationEmpirical formula C 4 H 6 O
AP Chem Test- Titration and Gravimetric Analysis p. 2 Name date 4. Empirical Formula A compound is analyzed and found to contain 68.54% carbon, 8.63% hydrogen, and 22.83% oxygen. The molecular weight of
More informationCh.7 ACTIVITY & SYSTEMATIC TREATMENT OF EQ
Ch.7 ACTIVITY & SYSTEMATIC TREATMENT OF EQ 7. Activity Effective concentration under ionic surroundings 7-. The effect of Ionic Strength on Soluility of salts. * Consider a saturated sol. Hg (IO 3 ), concentration
More informationCHAPTER 3 Ionic Compounds. General, Organic, & Biological Chemistry Janice Gorzynski Smith
CHAPTER 3 Ionic Compounds General, Organic, & Biological Chemistry Janice Gorzynski Smith CHAPTER 3: Ionic Compounds Learning Objectives: q Octet Rule & Predicting ionic Charges q Ionic Bonds q Formation
More informationDOUBLE DISPLACEMENT REACTIONS. Double your pleasure, double your fun
DOUBLE DISPLACEMENT REACTIONS Double your pleasure, double your fun Industrial processes produce unwanted by-products. Dissolved toxic metal ions-copper, mercury, and cadmium-are common leftovers in the
More informationChemistry. Approximate Timeline. Students are expected to keep up with class work when absent.
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationChapter 17: Solubility Equilibria
Previous Chapter Table of Contents Next Chapter Chapter 17: Solubility Equilibria Sections 17.1-17.2: Solubility Equilibria and the K sp Table In this chapter, we consider the equilibrium associated with
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria 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
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationModified Dr. Cheng-Yu Lai
Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant
More informationChapter 4 Three Major Classes of Chemical Reactions
Chapter 4 Three Major Classes of Chemical Reactions Solution Stoichiometry Many reactions (biochemical, marine, etc.) take place in solution. We need to be able to express the number of moles of particles
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationChapter 9: Acids, Bases, and Salts
Chapter 9: Acids, Bases, and Salts 1 ARRHENIUS ACID An Arrhenius acid is any substance that provides hydrogen ions, H +, when dissolved in water. ARRHENIUS BASE An Arrhenius base is any substance that
More informationChapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)
Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationUnit (2) Quantitative Chemistry
Unit (2) Quantitative Chemistry Chapter (1) :The mole & chemical equation Lesson (1) Mole and chemical equation Chemical equation: The chemical symbols and formulas of the reactants and products which
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationSolutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules
Solutions Solution: A homogenous mixture consisting of ions or molecules -Assignment: Ch 15 Questions & Problems : 5, (15b,d), (17a, c), 19, 21, 23, 27, (33b,c), 39, (43c,d),45b, 47, (49b,d), (55a,b),
More informationI. Multiple Choice Questions (Type-I) is K p
Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant 2. Solubility and the Common-Ion Effect 3. Precipitation Calculations 4. Effect of ph
More informationFlashback - Aqueous Salts! PRECIPITATION REACTIONS Chapter 15. Analysis of Silver Group. Solubility of a Salt. Analysis of Silver Group
Page III-15-1 / Chapter Fifteen Lecture Notes Flashback - Aqueous Salts! If one ion from the Soluble Compd. list is present in a compound, the compound is water soluble. PRECIPITATION REACTIONS Chapter
More informationSolubility & Equilibrium Unit Review
Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with
More informationName AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria
Name AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria Solutions of Acids or Bases Containing a Common Ion A common ion often refers to an ion that is added by two or more species. For
More informationSaturated vs. Unsaturated
Solubility Equilibria in Aqueous Systems K sp (Equilibria of Slightly Soluble Salts, Ionic Compounds) Factors that Affect Solubility (Common Ion Effect, AcidBase Chemistry) Applications of Ionic Equilibria
More informationReactions in aqueous solutions Precipitation Reactions
Reactions in aqueous solutions Precipitation Reactions Aqueous solutions Chemical reactions that occur in water are responsible for creation of cenotes. When carbon dioxide, CO2, dissolves in water, the
More informationChapter 16. Solubility Equilibria 10/14/2010. Solubility Equilibria. Solubility Product (Constant), K sp. Solubility and the Solubility Product
Solubility Equilibria These are associated with ionic solids dissolving in water to form aqueous solutions Chapter 16 Solubility Equilibria It is assumed that when an ionic compound dissolves in water,
More informationEquation Writing for a Neutralization Reaction
Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants
More informationAP Chapter 14: Chemical Equilibrium & Ksp
AP Chapter 14: Chemical Equilibrium & Ksp Warm-Ups (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 14: Chemical Equilibrium & Ksp 2 Warm-Ups
More informationChapter Outline. Ch 8: Aqueous Solutions: Chemistry of the Hydrosphere. H 2 S + Cu 2+ CuS(s) + 2H + (Fe, Ni, Mn also) HS O 2 HSO 4
Ch 8: Aqueous Solutions: Chemistry of the Hydrosphere H 2 S + Cu 2+ CuS(s) + 2H + (Fe, Ni, Mn also) HS - + 2 O 2 HSO 4 - + energy (supports life) Figure taken from Principles of Biochemistry, 2nd Ed. By
More informationCh. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2
Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution
More informationHomework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)
More informationChemistry 12 Unit III Solubility Notes
Chemistry 12 Unit III Solubility Notes III.1 A Review Of Solubility There are only three classes of compounds that form ionic solutions: ACIDS, BASES and SALTS. This unit will deal only with SALTS. Acids
More informationCh 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated
More informationSolubility Products. Solubility Products. Solubility Products. Solubility Products. Slide 2 / 57. Slide 1 / 57. Slide 3 / 57.
Slide 1 / 57 Slide 2 / 57 Products queous equilibria II Products onsider the equilibrium that exists in a saturated solution of aso 4 in water: aso 4 (s) a 2+ (aq) + SO 4 2- (aq) Slide 3 / 57 Products
More informationGive 6 different types of solutions, with an example of each.
Warm up (Jan 5) Give 6 different types of solutions, with an example of each. 1 Warm Up (Jan 6) 1. Write the reaction showing the dissolving of the following solids (be sure to note whether they are covalent
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A solution containing a large concentration of dissolved ions can be classified as a(n).
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationUnit 6 ~ Learning Guide Name:
Unit 6 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
More informationChapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
More informationChemistry 12 Solubility Equilibrium I. Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3.
Chemistry 12 Solubility Equilibrium I Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3. Writing Equations Solutions Vocab & Calculations What is a solution? A homogenous
More informationCHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry
More information2/4/2016. Chapter 15. Chemistry: Atoms First Julia Burdge & Jason Overby. Acid-Base Equilibria and Solubility Equilibria The Common Ion Effect
Chemistry: Atoms First Julia Burdge & Jason Overby 17 Acid-Base Equilibria and Solubility Equilibria Chapter 15 Acid-Base Equilibria and Solubility Equilibria Kent L. McCorkle Cosumnes River College Sacramento,
More informationName period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
More informationWhat is the correct name and bonding of BF 3? What is the correct name and bonding of BF 3?
What is the correct name and bonding of BF 3? 1. boron trifluoride, covalent compound 2. boron trifluoride, ionic compound 3. boron fluoride, covalent compound 4. boron fluoride, ionic compound What is
More informationSolutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)
Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3
More informationChapter 02 The Chemical Basis of Life I: Atoms, Molecules, and Water
Chapter 02 The Chemical Basis of Life I: Atoms, Molecules, and Water Multiple Choice Questions 1. The atomic number of an atom is A. the number of protons in the atom. B. the number of neutrons in the
More information