CEE November 2011 SECOND EXAM. Answer all questions. Please state any additional assumptions you made, and show all work.
|
|
- Augustus Dixon
- 5 years ago
- Views:
Transcription
1 EE 680 November 0 SEOND EXAM losed book, two pages of notes allowed. Answer all questions. Please state any additional assumptions you made, and show all work.. arbonate System. (50% for A & B) wo different drinking water supplies are used to provide a total plant flow of 5 MGD. Water # is a badly polluted surface water that has elevated levels of ammonia. Water # is a relatively pristine groundwater. he two are characterized as follows: Water Flow (MGD) alinity Ammonia p (mg/l as ao 3 ) (mg-n/l) # # 5 50 ~0 8.0 A. Water # is pre-treated with sodium hypochlorite to oxidize the ammonia to nitrogen gas prior to blending with water #. What is the p of water # after sodium hypochlorite (NaOl) addition. Assume the reaction with chlorine is stoichiometric (see equation below) and assume there are no other reactions occurring. N 3NaOl N 3Na 3l 3 O 4 ( g ) here are several ways to solve this. I based my alkalinity change on the amount of ammonia to be removed, but you could also base it on the requisite chlorine dose Ammonia = B A = (3 ) (3 0) = eq M he amount of ammonia lost is equal to the amound present in the raw water Ammonia = mg-n/l = /4,000= 0043 M Note thas sodium hypochlorite solutions usually come with some NaO, but for purposes of this problem, let s assume that the solution added is pure NaOl Although we call this ammonia, it is really present as ammonium ion (N 4 ) at all ps below 9.
2 Note that a high level of precision is needed to get an accurate p. For this reason, I will retain many more significant figures than I would normally. And so: alinity = eq/m * 0043 M = 0043 equ And now the final alkalinity is: f = i = = equ L So now we calculate the for this water (which does not change with chlorine addition) Recall that: = O α α α = { α = and for p =6.5, we have (using 6.35 and 0.33 as the two pa s): α = α = 8. 66x0 5 = 0.x (8.66x0 5 ) = 0.7x0 3 M Now we expect that with a drop in alkalinity, the p will go well below the first p, and the apha s can be simplied for the case where p<p α = = α = =
3 = W { And if we assume that α will be very small = W { = W ( W ) = 0 Solving this with the quadratic formula get us: p = 4.35 B. What will the p of the blended water be immediately after mixing water # (remember that this has just been treated with sodium hypochlorite) and water #? his is a closed system problem. herefore the total carbonate concentrations ( 's) must be determined and treated as conservative. Likewise the alkalinities are conservative, and then the final p can be determined from the blended and alkalinity. for either water: = O α α first, I would determine the alpha's at the two p's. Recall the general equations for a diprotic acid are: 3
4 α = α = his results in the following values (assuming ps of 6.3 and 0.3: p α α x so, for water #: = {(-.4/50,000) - ( ) ( )}/(0993 *.04x0-8 ) = 007 M But we didn t have to calculate this again, as it was already determined in part B and for water #: = {(50/50,000) - ( ) (0-8.0 )}/( *0757) = M now we need to calculate the blended alkalinities and total carbonates: = (0*(-.4) 5*50)/5/50,000 = 079 equ/l = (0*007 5*05035)/5 = 0638 M Now calculate the p from the earlier equation for total carbonates, and making any one of the following three sets of simplifying assumptions:. is large compared to O and 4
5 5 O = α α which becomes: α α ( ) ) ( α α Now use the quadratic equation: ( ) ( ) ( ) 4 ± = which is simplified to: ( ) ( ) ( ) ( ) ( ) ( ) 4 ± = and ( ) is = and ( ) is 079 (0638) = ( ) ( ) * x x x x ± = =
6 or p = O 3 - >> O 3 -, p >> p and is large compared to O and = O α α which becomes: α ( α ) But if p>>p, then we can ignore the first terms in the denominator of the alpha quotient. So this equation simplifies to: Now we can solve directly for : ( - ) 0 = = 4.75x0 or p =
7 or, 3. Make no assumptions and solve for the exact solution. his gives: p = omplexation (40% total for both parts) hloride forms few strong complexes. Mercury is one exception. he following two part problem concerns complexes of this metal-ligand combination. A. (0%) Attached is an accurate graph of alpha values (vs log l-) for the Mercuric hloride system. Using this graph determine the complete mercury speciation in sea water where free chloride is about M and total mercury is about 0-9 M. Assume the only mercury species are free g and the various mercuric chloride complexes (i.e., gl x ). B. (0%) Now determine the complete compsition of a 0-7 M solution of sodium chloride to which you have added 0-7 M of gl. Ignore all other mercury complexes except for the chloride ones (i.e., gl x ). 7
8 ...0 α 0 α α Alpha α α Log L A. Draw a verticle line at L =M or logl = hen read off the alpha values and determine concentrations. Below is an expanded view of the graph to aide in finding the best values. For the purposes of your exam, you only needed to draw the line over the full sized graph and locate the points as best you can by eye. he correct values are presented in the table below. 8
9 n-bar (equ) Alpha n-bar Log L Graph Variable Value Species onc (M) L l - α 7 gl 7x0 - α gl 3 4.7x0-0 α gl 4 4.7x0-0 B. Draw the two n-bar lines (equilibrium line and mass balance line). Find the intersection of the two lines and draw a vertical at that point. hen read off the alpha values and determine concentrations. Below is an expanded view of the graph to aide in finding the best values. For the purposes of your exam, you only needed to draw the line over the full sized graph and locate the points as best you can by eye. he correct values are presented in the table below. n mb L L x L L = = = M 7 7 9
10 Alpha n-bar (mass balance) n-bar (equ) n-bar Log L Alpha n-bar (mass balance) n-bar (equ).0.5 n-bar Log L 0
11 Graph Variable Value Species onc (M) L l -.7x0-7 α 0 g.5x0-8 α gl 4.0x0-8 α gl 4.5x Multiple hoice. (0%) Answer all 0 of the following questions. Indicate which of the options is the best choice. Question #6 was a bit ambiguous, so I didn t consider this one in the grade. he sum of total acidity and total organic carbon on any given sample is equal to a. the UV absorbance b. twice the total carbonate c. the value one d. half of the hardness e. none of the above. alinity is said to be conservative when: a. the system being studied is open to the atmosphere b. the system being studied is isolated in the subsurface c. the system being studied is at alkaline ps d. all of the above e. none of the above 3. Phenolphthalein a. is a hexadentate ligand b. is rarely used because noone can spell it c. complexes calcium forming an insoluble salt d. is the drug of choice for malaria e. changes from colorless to red as p increases 4. O 3 *: a. is composed mostly of aqueous O b. is conservative in closed systems c. is am ampholyte d. all of the above e. none of the above
12 5. A ligand atom: a. is always charged b. forms coordinate covalent bonds with metals c. is almost never dissolved d. only forms outer-sphere complexes e. none of the above 6. he ligand number: a. is usually 6 or less b. is related to the molecular weight of the central atom c. is a function of the size of the ligand d. all of the above e. none of the obove 7. he buffer intensity of the acetate/acetic acid system: a. is independent of the p b. is independent of the total acetate ( ) c. is zero when the p is zero. d. is at a minimum when the p is equal to the p of a pure acetate solution e. is at a minimum when the p = p 8. Detergent surfactants are used to: a. help solubilize grease b. complex trace metals c. take hardness cations from the surfactants d. elevate the acidity e. reduce the caloric content 9. EDA a. stands for ethylene dioxo-tetraacetic acid b. is most commonly used as a p buffer c. is a higly potent carcinogen d. all of the above e. none of the above 0. he Irving Williams Series a. is a means of estimating alkalinity b. describes the inverse proportionality of acidity to alkalinity c. includes a number of books, such as he hapman Report, and he Prize d. follows the increase in ligand affinity from Mn(II) to u(ii) e. provides a comprehensive description of ligand structure
13 Selected Acidity onstants (Aqueous Solution, 5, I = 0) NAME FORMULA pa Perchloric acid lo4 = lo SRONG ydrochloric acid l = l - -3 Sulfuric acid SO4= SO (&) AIDS Nitric acid NO3 = NO ydronium ion 3O = O 0 richloroacetic acid l3oo = l3oo Iodic acid IO3 = IO3-0.8 Bisulfate ion SO4 - = SO4 - Phosphoric acid 3PO4 = PO4 -.5 (&7.,.3) itric acid 35O(OO)3= 35O(OO)OO (&4.77,6.4) ydrofluoric acid F = F - 3. Nitrous acid NO = NO Acetic acid 3OO = 3OO Propionic acid 5OO = 5OO arbonic acid O3 = O (&0.33) ydrogen sulfide S = S (&3.9) Dihydrogen phosphate PO4 - = PO4-7. ypochlorous acid Ol = Ol Boric acid B(O)3 O = B(O)4-9. (&.7,3.8) Ammonium ion N4 = N3 9.4 ydrocyanic acid N = N Phenol 65O = 65O m-ydroxybenzoic 64(O)OO - = 64(O)OO- 9.9 acid Bicarbonate ion O3 - = O Monohydrogen PO4 - = PO4-3.3 phosphate Bisulfide ion S - = S- 3.9 Water O = O Methane 4 =
14 Log L 4
15 O - Log p
CEE November 2012 SECOND EXAM. Answer all questions. Please state any additional assumptions you made, and show all work.
CEE 680 20 November 2012 SECOND EXAM Closed book, two pages of notes allowed. Answer all questions. Please state any additional assumptions you made, and show all work. Some useful constants: P CO2 = 10
More informationFIRST EXAM. Miscellaneous Information: R = cal/mole K = J/mole K Absolute zero = C 1 joule = calories -20 C = wicked cold
CEE 680 16 October 2012 FIRS EXAM Closed book, one page of notes allowed. Answer question #1 and #4, and either #2 or #3. Please state any additional assumptions you made, and show all work. You are welcome
More informationCEE March FIRST EXAM (Solutions)
CEE 680 5 March 015 FIRST EXAM (Solutions) Closed book, one page of notes allowed. Answer any 4 of the following 5 questions. Please state any additional assumptions you made, and show all work. You are
More informationMid-Term Exam. October 28, 2010
CEE 370 Fall 2010 Mid-Term Exam October 28, 2010 Closed Book, one sheet of notes allowed Please answer any 4 of the following 9 questions on separate sheets of paper (except for the T/F questions that
More information10.1 Acids and Bases in Aqueous Solution
10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces
More informationAdvanced Chemistry Final Review
Advanced Chemistry Final Review 1. What are the products of complete combustion of hydrocarbons? Hydrocarbons are compounds made of carbon and oxygen. When they burn (combine with oxygen) they form carbon
More information8. Relax and do well.
EM 1515.001 Exam III John III. Gelder November 7, 2001 Name TA's Name Lab Section INSTRUTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,
More information8/24/2018. Bio 1101 Lecture 2 (guided) Chapters 2: Essential Chemistry. Chapter 2: Essential Chemistry for Biology
1 2 3 4 5 Bio 1101 Lecture 2 (guided) Chapters 2: Essential Chemistry Chapter 2: Essential Chemistry for Biology Levels of biological organization Ecosystem (e.g. savanna) Community (e.g. the organisms
More informationCEE 370 Environmental Engineering Principles
Updated: 29 September 2015 Print version CEE 370 Environmental Engineering Principles Lecture #7 Environmental Chemistry V: Thermodynamics, Henry s Law, Acids-bases II Reading: Mihelcic & Zimmerman, Chapter
More informationWhich fertiliser would improve the quality of this soil most effectively?
1 farmer s soil is very low in both nitrogen (N) and phosphorus (P). Which fertiliser would improve the quality of this soil most effectively? 2 Which compound is not used as a fertiliser? ammonium sulfate
More informationCHEM 1105 S10 January 21, 2014
CHEM 1105 S10 January 21, 2014 Chapter 3: Compounds and Formulas Today: Types of compounds: Ionic vs. covalent Naming ionic compounds Naming binary covalent compounds (two elements only) Ionic Bonding
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 informationWednesday, February 25, Acid and Base Reactions
Acid and Base Reactions Dilute aqueous solution of acetic acid, C3COO Aqueous solution of sodium hydroxide, NaO The role of the ydrogen Ion Cl (aq) Æ + (aq) + Cl - (aq) What does the neutral atom consist
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
More informationCEE 370 Environmental Engineering Principles
Updated: 29 September 2015 Print version CEE 370 Environmental Engineering Principles Lecture #7 Environmental Chemistry V: Thermodynamics, Henry s Law, Acidsbases II Reading: Mihelcic & Zimmerman, Chapter
More informationMidterm Examination 2
CH 221 General Chemistry Spring 2012 Name: Midterm Examination 2 Useful Information is located on the last two pages of the Exam. Multiple Choice Questions A carton of Morton's Iodized Salt, NaCl with
More informationChapter 5 Classification and Balancing of Chemical Reactions
Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical
More informationBonding of atoms makes molecules
Atomic Bonding and Molecules Chapter 15 Bonding of atoms makes molecules The Formation of Ions and Ionic Bonds Types of bonds Metallic Bonds Covalent Bonds Polar Covalent Bonds Molecular Polarity and Molecular
More informationGeneral Chemistry Notes Name
Bio Honors General Chemistry Notes Name Directions: Carefully read the following information. Look for the ** directions in italics** for prompts where you can do some work. Use the information you have
More informationCh8 Test. Multiple Choice Identify the choice that best completes the statement or answers the question.
h8 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. n ionic bond is. a. attraction of an atom for its electrons. b. attraction of atoms for electrons
More informationChapter 5: Nomenclature
Chem 1025 Prof George W.J. Kenney, Jr Introductory Chemistry, Zumdahl Decoste, 6th ed Last Update: 21July09 Chapter 5: Nomenclature These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationMid-Term Exam. October 28, 2010
CEE 370 Fall 010 Mid-Term Exam October 8, 010 Closed Book, one sheet of notes allowed Please answer any 4 of the following 9 questions on separate sheets of paper (except for the T/F questions that may
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 informationGCE O' LEVEL PURE CHEMISTRY (5073/02) Suggested Answers for 2016 O Level Pure Chemistry Paper 2
Section A (50 M) Aa) trend The number of electron shell increases The number of valence electrons increases Proton number increases There is a change in character from metallic to non-metallic Only true
More informationChemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound.
Unit 6: Chemical Formulas & Chemical Compounds Chemical Names & Formulas Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Molecular compound - it s formula reveals
More informationU N I T T E S T P R A C T I C E
South Pasadena Honors Chemistry Name 6 Compounds Period Date U N I T T E S T P R A C T I C E Section 1: Multiple Choice. Select the best answer choice for each question. (1 point each) 1. Bonds between
More informationChapter 16. The Danger of Antifreeze. Buffers. Aqueous Equilibrium
hapter 16 Aqueous Equilibrium The Danger of Antifreeze Each year, thousands of pets and wildlife die from consuming antifreeze Most brands of antifreeze contain ethylene glycol sweet taste and initial
More information19.3 Strengths of Acids and Bases > Chapter 19 Acids, Bases, and Salts Strengths of Acids and Bases
Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base Theories 19.2 Hydrogen Ions and Acidity 19.3 Strengths of Acids and Bases 19.4 Neutralization Reactions 19.5 Salts in Solution 1 Copyright Pearson Education,
More informationTest- Teacher s Use Only Student s Name Question Max Point Number Score Scored Date Duration Grade Instructions
Physical Science Test- Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student
More informationChemistry. Test - Unit Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17. Total. Teacher s Use Only. Student s Name. Max Score. Question Number. Point Scored.
Chemistry Test - Unit Teacher s Use Only Student s Name Date 2016-2017 Academic Year- Term Question Number Max Score Point Scored Duration Grade minutes G Q1 Q2 Q3 Instructions Fill in your student ID
More informationChemical Bonds, Lewis Structures, Bond Order, and Formal Charge
Chemical Bonds, Lewis Structures, Bond Order, and Formal Charge PRELAB ASSIGNMENT Read the entire laboratory write up. Write an objective, any hazards associated with this lab, and answer the following
More informationCHAPTER 18 ACID-BASE EQUILIBRIA
CAPTER 18 ACID-BASE EQUILIBRIA FOLLOW UP PROBLEMS 18.1A Plan: Examine the formulas and classify each as an acid or base. Strong acids are the hydrohalic acids Cl, Br, and I, and oxoacids in which the number
More informationAcid/Base Theories The common characteristics of acids
Acid/Base Theories The common characteristics of acids describe them as: Acids aving a sour taste Being electrolytes (some weak) Reacting with metals to produce gas (usually 2 ) Reacting with bases to
More informationQ = Enthalpy change for the formation of calcium chloride (P). D Twice the enthalpy change of atomization of chlorine (S).
1 What is the equation for the first electron affinity of sulfur? S(s) + e S (g) S(g) + e S (g) S(s) S + (g) + e S(g) S + (g) + e 2 The diagram shows a orn-haber cycle for calcium chloride. It is not drawn
More informationF321: Atoms, Bonds and Groups Structure & Bonding
F321: Atoms, Bonds and Groups Structure & Bonding 1. This question is about different models of bonding and molecular shapes. Magnesium sulfide shows ionic bonding. What is meant by the term ionic bonding?
More informationAtoms with a complete outer shell do not react with other atoms. The outer shell is called the valence shell. Its electrons are valence electrons.
Bonding and the Outer Shell Use this table for reference: http://www.dreamwv.com/primer/page/s_pertab.html Atoms with incomplete shells react with others in a way that allows it to complete the outer shell.
More informationSafety Manual > Incompatible Chemicals Partial Listing
Safety Manual > Incompatible Chemicals Partial Listing C. Incompatible Chemicals Partial Listing Chemical Incompatible Chemicals Acetic acid Chromic acid, nitric acid, permanganates, and peroxides Acetic
More informationName Final Exam Spring 2002 Page (16 points) Acetylsalicylic acid, the molecule pictured here, is better known as aspirin.
Name Final Exam Spring 2002 Page 1 1. (16 points) Acetylsalicylic acid, the molecule pictured here, is better known as aspirin. 1 A D 2 B 3 4 Describing the bonding in aspirin, acetylsalicylic acid. (a)
More information116 PLTL Activity sheet / Intro Acid - Base equilibrium Set 8
Potentially Useful or useless information: Strong and Weak Acids and Bases Definitions Arrhenius acid a compound that releases hydrogen ions ( + ) in water Brønsted acid a proton, + ion, donor Lewis acid
More informationIonic_Bonding_&_Ionic_Compounds_Presentation_v_1.1.notebook. October 26, Chemical Bonds. Notebook 4 Ionic Compounds and Ionic Bonding
Ionic_onding_&_Ionic_ompounds_Presentation_v_1.1.notebook hemical onds Notebook 4 Ionic ompounds and Ionic onding There are three basic types of bonds: Ionic The electrostatic attraction between ions ovalent
More informationNomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:
1 Chemistry 047 Inorganic Nomenclature Nomenclature of inorganic compounds = naming non carbon (mostly) compounds Some definitions: Nomenclature = system used by chemists to name and identify compounds
More informationO + (aq) In this reaction, the water molecule is a Brønsted-Lowry base. It accepts a proton from HF to form H 3
AcidBase Reactions Key Terms conjugate base conjugate acid amphoteric neutralization salt In the previous sections, you learned about three acidbase theories: Arrhenius, BrønstedLowry, and Lewis. The BrønstedLowry
More informationOctet rule Naming and writing formulas
Octet rule Naming and writing formulas Definitions The octet rule states that atoms are most stable when they have a full shell of 8 electrons in the OUTERMOST shell Ionic bonding forms between a metal
More informationScience 30 Unit B Chemistry and the Environment
Science 30 Unit B Chemistry and the Environment Outcome 1: Students will analyze the sources of acids and bases and their effects on the environment. Specific Outcome 1.1: Define acids and bases in terms
More informationChapter 2: Acids and Bases
hapter 2: Acids and Bases 32 hapter 2: Acids and Bases Problems 2.1 Write each acid- reaction as a proton-transfer reaction. Label which reactant is the acid and which the, as well as which product is
More information... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3
1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross
More informationChem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice
Chem 103 Exam #1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationCHEM J-4 June 2014
CHEM1102 2014-J-4 June 2014 Calculate the ph of a 0.010 M solution of aspirin at 25 C. The pk a of aspirin is 3.5 at this temperature. 7 Ammonia, NH 3, is a weak base in water. Write the equation for the
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 informationTHE CATION MUST ALWAYS BE WRITTEN FIRST
Name Honors Chemistry / / Binary Ionic Compounds An ionic compound is a compound that is formed between a metal and a non-metal. (Metalloids can also be used in ionic compounds, sometimes as cations and
More informationDescription Computer Bonding. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Name: Period:
Chemistry: Hood River Valley High School Unit 4 Note Pack and Goals Name: Period: Unit 4 Metals, Non-Metals, Metalloids, Ions, and Ionic compounds. Unit Goals- As you work through this unit, you should
More informationCHEM J-4 June 2014
CHEM1102 2014-J-4 June 2014 The structures of the drugs aspirin and benzocaine are shown below. (a) Draw the conjugate base of aspirin and the conjugate acid of benzocaine. (b) Circle the form of each
More informationYou try: 2) HC 7H 6O 2 3) N 2O 5. 5) HClO 4. 7) Rb 2C 2O 4 8) H 3PO 4 9) AgI 10) Sr(OH) 2. What kind of compound is it? NON ELECTROLYTE (NE)
Solubility: Solubility is the measure of how much of a solute will dissolve in a solvent. In general chemistry, we usually talk about water as the solvent, so we are talking about what compounds will dissolve
More informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationPlease print: + log [A- ] [HA]
Please print: Last name: First name: Chem 1062 Exam 3 Spring 2005 Andy Aspaas, Instructor Thursday, April 7, 2005 Equations: K c = [C]c [D] d [A] a [B] b ph =! log[h 3 O + ] poh =! log[oh! ] ph + poh =
More informationChapter 2 The Chemical Context of Life
Chapter 2 The Chemical Context of Life Information in this chapter establishes a foundation for later discussion and elaboration of molecular-level events and processes in biological systems. Ensuring
More informationGilbert Kirss Foster. Chapter 4. Chemical Bonding. Understanding Climate Change
Gilbert Kirss Foster Chapter 4 Chemical Bonding Understanding Climate Change Chapter Outline 4.1 Types of Chemical Bonds 4.2 Naming Compounds and Writing Formulas 4.3 Lewis Structures 4.4 Electronegativity,
More informationCHAPTER 8 Ionic and Metallic Bonds
CHAPTER 8 Ionic and Metallic Bonds Shows the kind of atoms and number of atoms in a compound. MgCl 2 NaCl CaCO 3 Al 2 O 3 Ca 3 (PO 4 ) 2 Chemical Formulas Al: Cl: counting atoms AlCl 3 Pb: N: O: Pb(NO
More informationReagents for Chemical Test Kits
for Chemical Test Kits Acidity, methyl orange method ; 0 to 500 mg/l HI 3820-100 Reagent kit for 110 tests (CaCO 3 ) Acidity, olive oil, titration with hydroxide 0.00 to 1.00% HI 3897 Reagent kit for 6
More informationIons and Ionic Compounds
Ions and Ionic Compounds Elements combine in a specific ratio to form compounds. Compounds can be categorized as ionic or covalent depending on the type of bond present within the compound. Ionic compounds
More informationChemistry 142 (Practice) MIDTERM EXAM II November. Fill in your name, section, and student number on Side 1 of the Answer Sheet.
Chemistry 4 (Practice) MIDTERM EXAM II 009 November (a) Before starting, please check to see that your exam has 5 pages, which includes the periodic table. (b) (c) Fill in your name, section, and student
More information» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.
» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.» Separated chemically not physically» No overall charge; they
More informationExam 2. CHEM Spring Name: Class: Date:
CHEM-112-01 Spring 2012 Name: Class: Date: 1. Record your name and ID number on the scantron form. 2. Record the test ID letter in the top right box of the scantron form. 3. Record all of your answers
More informationPRACTICE EXAM III CCBC-Catonsville. TOTAL 100 Bonus p.5 7. Adjusted total to Exam III = Current Course Total = Chem 107
Chem 107 PRACTICE EXAM III CCBC-Catonsville *** ALWAYS ANSWER IN FULL SENTENCES! *** On numerical problems, you MUST show your set ups. When dimensional analysis is specified, you MUST set up the problem
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 informationThe Periodic Table. run vertically on the periodic table (up and down).
Lesson Objective: The Periodic Table Science 8.5B Interpret the arrangement of the Periodic Table, including groups and periods, to explain how properties are used to classify elements 8.2E Analyze data
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More informationChapter 9 Aqueous Solutions and Chemical Equilibria
Chapter 9 Aqueous Solutions and Chemical Equilibria At equilibrium, the rate of a forward process or reaction and that of the reverse process are equal. 9A The chemical composition of aqueous solutions
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationCh 4-5 Practice Problems - KEY
Ch 4-5 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
More informationEquilibrium Acids and Bases 6
1. Strong Acids and Bases Equilibrium Acids and Bases 6 Examples of strong acids are H 2 SO 4, HNO 3, HCl, HBr, and HI. (There are a few others, e.g. HClO 4, which we will not discuss.) Since strong acids
More informationGeneral Chemistry. Lecture 3
General Chemistry Lecture 3 Electrons Protons and neutrons are found in the nucleus Electrons surround the nucleus in energy levels or shell at certain distances around the nucleus The number of electrons
More informationPRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY
Name: Date: Class: PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY BUBBLE SHEETS AND PERIODIC TABLES ARE ATTACHED. PLEASE DETACH. YOU MAY WRITE ON THE PERIODIC TABLE. PART ONE: Multiple choice. Choose
More informationa. Always start with the species added to water.
Calculation of ph Proton Balance Equations According to the Brönsted Lowry theory, every proton donated by an acid must be accepted by a base. Thus, an equation accounting for the total proton transfers
More informationCHEM1902/ N-6 November 2014
CHEM1902/4 2014-N-6 November 2014 Boric acid, B(OH) 3, is a weak acid (pk a = 9.24) that is used as a mild antiseptic and eye wash. Unusually, the Lewis acidity of the compound accounts for its Brønsted
More informationMake a mixture of a weak acid and its conjugate base (as the SALT) Make a mixture of a weak base and its conjugate acid (as the SALT)
175 BUFFERS - resist ph change caused by either the addition of strong acid/base OR by dilution Made in one of two ways: Make a mixture of a weak acid and its conjugate base (as the SALT) Make a mixture
More informationTOPIC: Chemical Bonds
TOPIC: Chemical Bonds H O bond H a water molecule In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they
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 informationIonic Bonding (Ch.7) Covalent Bonding (Ch.8) Metallic Bonding
Unit 3: Chemical Bonding Outline Ionic Bonding (Ch.7) Valence electrons Positive and negative ions and transition metal ions Ionic bonding: Charge on compounds Ionic compounds characteristics Writing ionic
More informationChemistry--Unit 2: Chemical Names and Formulas Test Review
vocab anion binary compound cation chemical formula formula unit ion ionic compound law of definite proportions law of multiple proportions molecular formula polyatomic ion representative particle ternary
More informationNomenclature. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion
Nomenclature C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid 1 Forms of Chemical Bonds Most bonds are somewhere in between ionic There are 3 forms bonding atoms: Ionic complete transfer of 1 or more
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 informationName: Period: Score: Everything About Chemical Formulas
Name: Period: Score: Everything About Formulas Compounds have unique names that identify them for us when we study chemical properties and changes. Chemists have devised a shorthand way of representing
More informationChem 150, Spring Unit 4 - Acids & Bases. Introduction
Chem 150, Spring 2015 Unit 4 - Acids & Bases Introduction Patients with emphysema cannot expel CO2 from their lungs rapidly enough. This can lead to an increase of carbonic (H2CO3) levels in the blood
More informationThe following practice examination contains 32 questions. Thursday s examination will contain 32 questions valued at 3.
Chemistry 121 Exam 2 Practice Spring 2018 The following practice examination contains 32 questions. Thursday s examination will contain 32 questions valued at 3.5 points/question Name KEY 1. Which of the
More informationC. Incorrect! These are the correct symbols, but the charges must be balanced. D. Correct! The charges are balanced in this formula.
SAT Chemistry - Problem Drill 07: Writing Chemical Formulas No. 1 of 10 1. Which of the following is correct for sodium oxide? (A) SO (B) S 2 O (C) NaO (D) Na 2 O (E) NaO 2 Sodium is symbolized with Na.
More informationBonding-when atoms get it on. Ionic Compounds 9/22/2013. Chemical Formulas and Bonding
Bonding-when atoms get it on Chemical Formulas and Bonding There are two types of bonds that you need to know. The first kind of bond is Ionic bond. Ionic Bond = when a positive ion is attracted to a negatively
More information26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O
Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +
More informationThe chemical formulas of most of the elements are simply their elemental symbol:
Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.
More informationChemistry Final Exam Sample Items
Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons
More informationChapter Test B. Chapter: Acids and Bases
Assessment Chapter Test B Chapter: Acids and Bases PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the
More informationO ( ) are only used with polyatomic ions and only when there is more than one of any group. a. Examples: HNO 3. ) is incorrect; Al 2 ) 3 (SO 4
HONORS CHEMISTRY - CHAPTER 9 CHEMICAL NAMES AND FORMULAS NOMENCLATURE PACKET - V16 NAME: DATE: PAGE: I. Writing formulas of ionic compounds when given the component parts. 1. Many compounds are composed
More informationNomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion. Chemistry 1 Honors: Chapter 7: pp
Chemistry 1 Honors: Chapter 7: pp218-258 PO 4 3- phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 - acetate ion SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts"
More information2 Answer all the questions.
2 Answer all the questions. 1 A sample of the element boron, B, was analysed using a mass spectrometer and was found to contain two isotopes, 10 B and 11 B. (a) (i) Explain the term isotopes. Complete
More informationPage Points Score Total: 175
Name: Date: Page Points Score 2 14 3 16 4 26 5 22 6 30 7 14 8 28 9 25 Total: 175 Show all your work. Write in Pen. Check your significant figures and units. Please show all your work. Answers must be circled.
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) Oxidation is the and reduction is the. A) loss of oxygen, gain of electrons B) gain of
More informationChemical Reactions and Equilibrium Acid/Bases Redox. Revision What is a chemical reaction? What factors affect the rate of reaction?
Chemistry Fundamental Topics These notes will provide a brief coverage of topics that will be important for your Course in instrumentation. The notes are supplementary to the Instrumentation notes and
More information