I. Micro-nutrients in the oceans
|
|
|
- Lambert Sparks
- 6 years ago
- Views:
Transcription
1 Impact of global change on ocean biogeochemical cycles (N, P, C and trace elements) Palma de Mallorca, Oct 2011 I. Micro-nutrients in the oceans X. Antón Álvarez Salgado CSIC, Instituto de Investigacións Mariñas C/ Eduardo Cabello 6, Vigo
2 outline of this presentation C, N P and Si reservoirs in the oceans
3 outline of this presentation C, N P and Si reservoirs in the oceans Worsfold et al., Anal. Chim. Acta, 2008
4 outline of this presentation dissolved inorganic compounds in the oceans dissolved inorganic nitrogen in the oceans dissolved inorganic phosphorus in the oceans dissolved silicon in the oceans
![dissolved inorganic compounds in the oceans TA = [Na + ] + 2 [Mg 2+ ] + 2 [Ca 2+ ] + [K + ] + 2 [Sr 2+ ]](/docs-images/74/71361264/images/5-0.jpg "+. - [Cl - ] - 2 [SO 4 2- ] - [Br - ] - [F - ] - the concept of alkalinity Zeebe and Wolf-Gladrow (2001)")
5 dissolved inorganic compounds in the oceans TA = [Na + ] + 2 [Mg 2+ ] + 2 [Ca 2+ ] + [K + ] + 2 [Sr 2+ ] +. - [Cl - ] - 2 [SO 4 2- ] - [Br - ] - [F - ] - the concept of alkalinity Zeebe and Wolf-Gladrow (2001)
6 dissolved inorganic compounds in the oceans TA = [HCO 3 ] + 2 [CO 3 2 ] + [B(OH) 4 ] + [OH ] + [BASES] [H + ] [OH ] = [OH ] + [Mg(OH) + ] [H + ] = [H + ] + [HSO 4 2 ] + [HF] [H + ] = [HCO 3 ] + 2 [CO 3 2 ] + [B(OH) 4 ] + [OH ] + [BASES] phsws = 4.25 the concept of alkalinity
7 dissolved inorganic compounds in the oceans K 2 HCO 3 - CO H + pka K 1 CO 2 + H 2 O HCO H + K B H 3 BO 3 + H 2 O B(OH) H + 4,25 8, 0 8, 0 4, 25 HCO - 3 /CO ,000-1,000-1,000 CO /HCO ,000-2,000-2,000 B(OH) - 4 /H 3 BO ,000-0,213-0,213 STANDARD SEAWATER (phsws = 8.0; CO2 = 2100 µmol kg -1 ) K 1 (35, 15) = [CO 2 = 13.8 µmol kg -1 (0.7%) K 2 (35,15) = [HCO 3- = µmol kg -1 (91.3%) S (35,15) = [CO 3 2- = µmol kg -1 (8.0%) K B (35, 15) = [B(OH) 4- = 88.7 µmol kg -1 (21.3%) [H 3 BO 3 = µmol kg -1 (78.7%) A C = [HCO 3- ] + 2 [CO 3 2- ] = 2256 µmol kg -1 A B S B(OH) B 416 T μmol kg 35-1 the concept of alkalinity
8 dissolved inorganic nitrogen (DIN) dissolved inorganic nitrogen species Codispoti, Biogeosciences, 2007
9 dissolved inorganic nitrogen (DIN) K NO3 = 25 NO 3 H NO 3 + H + K NO2 NO 2 H NO H + pka 4,25 8, 0 8, 0 4, 25 - HNO 3 /NO 3-1,4-1,000-1,000 0,000 - HNO 2 /NO 2 3,25 0,909 1,000 0,091 NH 4+ /NH 3 9,23 +1,000 +0,915-0,085 (K NH4 ) -1 NH 3 (aq) + H + NH 4 + contribution of dissolved inorganic nitrogen to alkalinity
10 dissolved inorganic nitrogen (DIN) distribution of NO 3- in the oceans Schmitz, WHOI, 1995 Sarmiento & Gruber, 2006 (
11 dissolved inorganic nitrogen (DIN) distribution of NO 3- in the oceans Sarmiento & Gruber, 2006 (
12 dissolved inorganic nitrogen (DIN) distribution of NO 3- in the oceans Sarmiento & Gruber, 2006 (
13 dissolved inorganic nitrogen (DIN) distribution of NO 2- in the oceans: the primary maximum (< 1 μmol/kg) Lomas & Lipschultz, Limnol. Oceanogr., 2006
14 dissolved inorganic nitrogen (DIN) distribution of NO 2- in the oceans: the secondary maximum (1-10 μmol/kg) Codispoti et al., Sci. Mar., 2001
15 dissolved inorganic nitrogen (DIN) distribution of NH 4+ in the oceans
16 dissolved inorganic nitrogen (DIN) ΔN 2 O (natm) ΔN 2 O (mg N/m 2 /y) distribution of N 2 O in the oceans Nevison et al., Global Biogeochem. Cycles, 1995
17 dissolved inorganic nitrogen (DIN) distribution of N 2 O in the oceans Nevison et al., Global Biogeochem. Cycles, 2003
18 dissolved inorganic phosphorus (DIP) K 1P H 3 PO 4 H 2 PO H + STANDARD SEAWATER K 2P ph SWS = 8.0 phsws= 4.25 H 2 PO 4 - HPO H + H 3 PO 4 0.0% 0.2% K 3P HPO 4 2- PO H + H 2 PO 4 - HPO 2-4 PO % 88.4% 10.8% 97.7% 2.2% 0.0% A PO4 = (3 [PO 4 3- ] + 2 [HPO 4 2- ] + [H 2 PO 4- ]) 8.0- (3 [PO 4 3- ] + 2 [HPO 4 2- ] + [H 2 PO 4- ]) 4.25 pk 1 pk 2 pk 3 4,25 8, 0 8, 0 4, 25 H 3 PO 4 1,60 6,03 8,99 1,016 2,149 1,133 dissolved inorganic phosphorus species
19 dissolved inorganic phosphorus (DIP) distribution of dissolved inorganic phsophorus in the oceans Sarmiento & Gruber, 2006 (
20 dissolved silicon (SiO 2 ) STANDARD SEAWATER K si H 4 SiO 4 Si(OH) 3 O - + H + K Si (35,15)= phsws = 8.0 phsws = 4.25 H 4 SiO % 100 % Si(OH) 3 O - 4.2% 0.0% pka 4,25 8, 0 8, 0 4, 25 SiO 4 H 3- /SiO 4 H 4 9,52 0,000-0,042-0,042 dissolved inorganic silicon species
21 dissolved silicon (SiO 2 ) distribution of Si(OH) 4 in the oceans Sarmiento & Gruber, 2006 (
Conjugate Pairs Practice #1
Name: Key Skill: Learning to Draw Tie Lines Conjugate Pairs Practice #1 Look at each example drawn below. Sets of partners (called s) are matched with tie lines. HNO3 + OH - NO3 - + H2O CH3NH2 + H2O CH3NH3
INTRODUCTION TO CO2 CHEMISTRY
INTRODUCTION TO CO2 CHEMISTRY IN SEA WATER Andrew G. Dickson Scripps Institution of Oceanography, UC San Diego 410 Mauna Loa Observatory, Hawaii Monthly Average Carbon Dioxide Concentration Data from Scripps
INTRODUCTION TO CO2 CHEMISTRY
INTRODUCTION TO CO2 CHEMISTRY IN SEA WATER Andrew G. Dickson Scripps Institution of Oceanography, UC San Diego Mauna Loa Observatory, Hawaii Monthly Average Carbon Dioxide Concentration Data from Scripps
Nutrients; Aerobic Carbon Production and Consumption
Nutrients; Aerobic Carbon Production and Consumption OCN 623 Chemical Oceanography Reading: Libes, Chapters 8 and 9 Formation and respiration of organic matter DINutrients POM Primary Producers Autotrophs
Chapter 12: Acids and Bases: Ocean Carbonate System James Murray 4/30/01 Univ. Washington
Chapter 12: Acids and Bases: Ocean Carbonate System James Murray 4/30/01 Univ. Washington Last lecture was concerned with gas exchange and one example we looked at was the solubility of CO 2. Next we have
Chapter 7 ACIDS AND BASES. Exercises
Chapter 7 ACIDS AND BASES Exercises 7.2 (a) A nonpolar solvent because phosphorus pentachloride is a nonpolar covalent compound. (b) A polar protic solvent because cesium chloride is ionic. Ionic compounds
Nutrients; Aerobic Carbon Production and Consumption
Nutrients; Aerobic Carbon Production and Consumption OCN 623 Chemical Oceanography Reading: Libes, Chapters 8 and 9 Formation and respiration of organic matter DINutrients POM Primary Producers Autotrophs
a) most likely to gain two electrons Br O Al Mg b) greatest tendency to form a negative ion Na Li S Mg c) a non-metal Sr S Al K
1. (4 pts) Name the following compounds: Al 2 (SO 4 ) 3 N 2 O 3 2. (4 pts) Give the chemical formulas for the following compounds: chromium (III) carbonate magnesium phosphate 3. (16 pts) Circle the formula
Principles of Chemistry II Vanden Bout
Let s think about Acids What is in solution? Which of the following is amphiprotic? A. H3PO4 B. NaH2PO4 C. K3PO4 D. NaCl E. Na3PO4 What is in solution? If I add 0.1 moles of NaOH to 0.07 moles of H3PO4
Hydrological Cycle Rain and rivers OUTLINE
Hydrological Cycle Rain and rivers The Hydrosphere Rain and rivers OUTLINE 1 Generalizations (non-political conservatism) Conservative (not affected) and Non-Conservative (affected) Ions Distinction: whether
Solution chemistry of carbon dioxide in sea water
Page 1 of 15 Solution chemistry of carbon dioxide in sea water 1. Introduction This chapter outlines the chemistry of carbon dioxide in sea water so as to provide a coherent background for the rest of
ARTICLE IN PRESS. La Jolla, CA , USA. Received 13 February 2006; received in revised form 15 September 2006; accepted 4 January 2007
MARCHE-02440; No of Pages 14 ARTICLE IN PRESS + MODEL Marine Chemistry xx (2007) xxx xxx www.elsevier.com/locate/marchem Total alkalinity: The explicit conservative expression and its application to biogeochemical
Chemistry 12 Unit 4 Topic A Hand-in Assignment
1 Chemistry 12 Unit 4 Topic A Handin Assignment Answer the following multiplechoice and written response problems on your own paper. Submit your answers for marking. You do not need to show your work for
Acid / Base Properties of Salts
Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,
The Global Carbon Cycle Recording the Evolution of Earth, from the origin of life to the industrialization of the planet
The Global Carbon Cycle Recording the Evolution of Earth, from the origin of life to the industrialization of the planet Celebrating 5 years of world-leading collaborative and multidisciplinary research
Acid-Base Character of Salt Solutions. Cations. Cations are potentially acidic, but some have no effect on ph.
Acid-Base Character of Salt Solutions The ph of a salt solution will depend on the acidbase nature of both the cation and anion. Cations Cations are potentially acidic, but some have no effect on ph. M(H
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
Unit 12: Acids & Bases. Aim: What are the definitions and properties of an acid and a base? Properties of an Acid. Taste Sour.
Unit 12: Acids & Bases Aim: What are the definitions and properties of an acid and a base? Mar 23 12:08 PM Properties of an Acid 3. Are electrolytes. (Dissociate and conduct electricity when aq) 2. Turns
Arrhenius Acid-Base Concept Svante Arrhenius, 1884
Arrhenius Acid-Base Concept Svante Arrhenius, 1884 O Acids and bases are electrolytes. O Acids are substances that produce hydrogen ion, H + (aq), in solution. O Bases are substances that produce hydroxide
UNIT IV PPT #3 Ka and Kb KEY.notebook. November 23, WHAT IS Ka? UNIT IV. CALCULATIONS USING Ka. WHAT IS Ka? Nov 10 9:42 PM.
WHAT IS Ka? Recall: Find ph of 0.100 M HCl. But What is ph of 0.10 M HF? UNIT IV Ka and Kb CALCULATIONS USING Ka I. [H 3O + ] (or ph) from Ka Ex. Find the [H 3O + ] in 0.10 M HF. WHAT IS Ka? Look at equilibrium
Chemical Oceanography 14 March 2012 Points are in parentheses (show all your work) Final Exam
Ocean 400 Name: Chemical Oceanography 14 March 2012 Winter 2012 Points are in parentheses (show all your work) (give as much detail as you can) (use back if necessary) Final Exam 1. Sarmiento and Gruber
Chapter 16 Homework Solutions
//05 Chapter 16 Homework Solutions 6. a) H AsO b) CH 3 NH 3 + c) HSO d) H 3 PO 8. acid base conj. base conj. acid a) H O CHO OH CH O a) HSO HCO 3 SO H CO 3 b) H 3 O + HSO 3 H O H SO 3 10. a) H C 6 H 7
Chapter 5 - Homework solutions
Chapter 5 - Homework solutions Q Ex 1,2,3,4,5,7,9,13,18,20,21,23, 27,29 and Prob. 3,4,6,7 1) Li Be B C N O F acidic Na Mg Al Si P S Cl amphoteric K Ca Ga Ge As Se Br basic Rb Sr In Sn Sb Te I Cs Ba Tl
Chem 1102 Semester 1, 2011 ACIDS AND BASES
Chem 1102 Semester 1, 2011 ACIDS AND BASES Acids and Bases Lecture 23: Weak Acids and Bases Calculations involving pk a and pk b Strong Acids and Bases Lecture 24: Polyprotic Acids Salts of Acids and Bases
In the Brønsted-Lowry system, a Brønsted-Lowry acid is a species that donates H + and a Brønsted-Lowry base is a species that accepts H +.
16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 BrønstedLowry Acids and Bases In the BrønstedLowry system, a BrønstedLowry
I II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is
1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium
Formation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic
Formation of a salt (ionic compound): Neutralization reaction molecular Full ionic Eliminate spect ions to yield net ionic Hydrolysis/ reaction with water Anions of Weak Acids Consider the weak acid HF
Nutrients; Aerobic Carbon Production and Consumption
Nutrients; Aerobic Carbon Production and Consumption OCN 623 Chemical Oceanography Reading: Libes, Chapters 8 and 9 Why is organic matter such a good electron donor? Every (other) breath you take is a
Chemical Speciation. OCN 623 Chemical Oceanography. 30 January Reading Libes, Chapter Frank Sansone
Chemical Speciation OCN 623 Chemical Oceanography 30 January 2014 Reading Libes, Chapter 5 2014 Frank Sansone Outline Up until now, we have assumed that ionic solutesdissolve in their solvent(water) as
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
AP Chemistry: Acid-Base Chemistry Practice Problems
Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure
Equilibrium Lecture Examples
Equilibrium Lecture Examples Problem 1: Consider the reaction: J R 8.3145 T 98.15K K PCl 5 PCl 3 + Cl a.) Compute the standard Gibbs Free energy for this system at 98.15K. In which direction will the reaction
1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
Chapter 13 Acids and Bases
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 13 Acids and Bases Edward J. Neth University of Connecticut Outline 1. Brønsted-Lowry acid-base model 2. The
1. 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
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
Unit 9: Acid and Base Multiple Choice Practice
Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.
Fall 2014 Due: 10:30 a.m., Tuesday, Sept 16
GEOL330/634 Fall 2014 Due: 10:30 a.m., Tuesday, Sept 16 Problem Set #1 Key 1. What determines if an ion is a major ion in seawater? (5) Major ions are those that contribute to salinity. If salinity can
organisms CaCO 3 + H 2 O + CO 2 shallow water
Weathering and Reverse weathering Step I:Weathering of igneous rocks 1. Igneous rocks are mainly composed of Al, Si and O 2 with minor and varying quantities of Na, K, Ca and Mg composing pheldspar minerals
General Chemistry II CHM 1046 E Exam 2
General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of
Table 1. Solubility of gypsum and anhydrite adopted in this research and the predicted SI values
Supporting information: Table 1. Solubility of gypsum and anhydrite adopted in this research and the predicted SI values Sample T ID # ( o C) 16, 65, 74 P NaCl CaSO 4 nh 2 O SI System (psi) (mol/kg H 2
Unit 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
Dr. Diala Abu-Hassan, DDS, PhD Lecture 3 MD summer 2014
ph, DDS, PhD Dr.abuhassand@gmail.com Lecture 3 MD summer 2014 www.chem4kids.com 1 Outline ph Henderson-Hasselbalch Equation Monoprotic and polyprotic acids Titration 2 Measuring the acidity of solutions,
CHEMICAL REACTIONS IN SOLUTION AND NET IONIC EQUATIONS
CHEMICAL REACTIONS IN SOLUTION AND NET IONIC EQUATIONS Chemical reactions that occur in solution fall into two broad categories: Oxidation-reduction reactions: reactions in which ion charges change Metathesis
Acid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
CHEM 142 Exam 3 Study Guide Chapter 15: Acid-Base Equilibria
CHEM 142 Exam 3 Study Guide Chapter 15: AcidBase Equilibria A. Terminologies and Concepts 1. BronstedLowry definitions acids vs. bases; give examples 2. Amphoteric substances define and give examples 3.
Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)
Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers
acid : a substance which base : a substance which H +
4.4. BronstedLowry Theory of A&B acid : a substance which base : a substance which H Typical BronstedLowry AB rxn eqn: eg1) NH 3 H 2 O NH 4 base acid OH eg2) CH 3 COOH H 2 O CH 3 COO H 3 O H 2 O an acid
Term paper topics, due February 8
Term paper topics, due February 8 ODV mini-projects, due March 13 (10% final grade) Individuals or teams of two Using any available datasets, put together a ~7-10 minute talk to present in class on March
CHEMISTRY 102 Fall 2010 Hour Exam III Page My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
Hour Exam III Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml
Brønsted-Lowry Acid-Base Model. Chapter 13 Acids and Bases. The Nature of H + Outline. Review from Chapter 4. Conjugate Pairs
Brønsted-Lowry Acid-Base Model William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 13 Acids and Bases Brønsted-Lowry Johannes Brønsted (1879-1947) Thomas Lowry (1874-1936)
The ph of aqueous salt solutions
The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2
1. Properties of acids: 1. Contain the ion Bases: 1. Contain the ion. 4. Found on Table 4. Found on table
For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining it
MAR 510 Chemical Oceanography
Carbonate Equilibrium -Key Concepts- Major buffer system influencing ph (master variable) Linked to geological, biological and climatological cycles Complex chemistry involving gaseous, dissolved, and
Chapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a.
![Chapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a.](/thumbs/95/123080455.jpg "Chapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a.")
Chapter 17 Answers Practice Examples 1a. + [HO ] 0.018M, 1b. 0 drops [HF] = 0.8 M. [H O + ] = 0.10 M, HF = 0.97 M. a. + HO 1.10 M, CHO = 0.150 M. b. 15g NaCHO a. The hydronium ion and the acetate ion react
Practice Exam 1: Answer Key
CHM 2046 Practice Exam 1: Answer Key Important: Bubble in A, B or C as the test form code at the top right of your answer sheet. Useful information is provided at the end. VERSION A 1. The reaction A(aq)
Exam 3A Fetzer Gislason. Name (print)
Fetzer Gislason, December 1, 2003 Name (print) TA Directions: There are 25 multiple-choice problems @ 4 points each. Record these answers on your scantron sheet. Total possible score is 100 points. You
Equilibri 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.
2. What is the equilibrium constant for the overall reaction?
Ch 15 and 16 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
CHEM1902/ N-4 November 2004
CHEM190/4 004-N-4 November 004 Teeth are made from hydroxyapatite, Ca 5 (PO 4 ) 3 OH. Why does an acidic medium promote tooth decay and how can the decay be stopped using fluoridation of drinking water?
Chapter 16 exercise. For the following reactions, use figure 16.4 to predict whether the equilibrium lies predominantly. - (aq) + OH - (aq)
1 Chapter 16 exercise Q1. Practice exercise page 671 Write the formula for the conjugate acid of the following, HSO 3, F, PO 4 3 and CO. HSO 3 H H 2 SO 4 F H HF PO 4 3 H HPO 4 2 CO H HCO Q2. Practice exercise
mol of added base 36. Equal moles of which of the following chemicals could be used to make a basic (1 mark)
59. 34. Consider the following titration curve: 14 13 Consider the following titration curve: 14 1 13 11 14 1 1 13 119 1 18 ph 119 7 18 6 ph 97 5 86 4 ph 75 3 64 53 1 4 31 mol of added base Select a suitable
Biogeochemistry of the Earth System QMS Lecture 5 Dr Zanna Chase 16 June 2015
Biogeochemistry of the Earth System QMS512 2015 Lecture 5 Dr Zanna Chase 16 June 2015 Lecture 5: Inorganic carbon chemistry Outline Inorganic carbon speciation in seawater- conceptual overview Inorganic
Today. Solubility The easiest of all the equilibria. Polyprotic Acids determining something about an unknown by reacting it with a known solution
Today Solubility The easiest of all the equilibria Polyprotic Acids determining something about an unknown by reacting it with a known solution Solubility Equilibria Mg(OH)2 (s) Mg 2+ (aq) + 2OH - (aq)
Ch 15 and 16 Practice Problems
Ch 15 and 16 Practice Problems 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,
NH 3 (aq) + HF (aq) F (aq) + NH 4. NaOH (aq) + H 2 O (l) NaOH (aq) + H 2 O (l) KOH (aq) + H 2 CO 3 (aq) KHCO 3 (aq) + H 2 O (l)
Quiz 2.1 Acid-Base Definitions 1. The conjugate base of H 3O + is: A. H 3O B. H 2O C. H 3O D. H 3O + E. HO 2. What is the conjugate acid of C 6H 5NH 2? A. C 6H 5NH 3 + B. C 6H 5NH C. C 6H 5NH 4 + D. C
Chapter 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,
Term paper topics, due February 9
Term paper topics, due February 9 ODV mini-projects, due March 14 (10% final grade) Individuals or teams of two Using any available datasets, put together a ~7-10 minute talk to present in class on March
Activity Balancing Oxidation-Reduction Reactions
Activity 201 3 Balancing Oxidation-Reduction Reactions Directions: This GLA worksheet goes over the half-reaction method of balancing oxidation-reduction (redox) reactions. Part A introduces the oxidation
For problems 1-4, circle the letter of the answer that best satisfies the question.
CHM 106 Exam II For problems 1-4, circle the letter of the answer that best satisfies the question. 1. Which of the following statements is true? I. A weak base has a strong conjugate acid II. The strength
CHEMISTRY 1AA3 Tutorial 2 Answers - WEEK E WEEK OF JANUARY 22, (i) What is the conjugate base of each of the following species?
CHEMISTRY 1AA3 Tutorial 2 Answers - WEEK E WEEK OF JANUARY 22, 2001 M.A. Brook B.E. McCarry A. Perrott 1. (i) What is the conjugate base of each of the following species? (a) H 3 O + (b) NH 4 + (c) HCl
SUPPORTING INFORMATION FOR. Spectrophotometric measurements of the carbonate ion concentration: aragonite
SUPPORTING INFORMATION FOR Spectrophotometric measurements of the carbonate ion concentration: aragonite saturation states in the Mediterranean Sea and Atlantic Ocean Noelia M. Fajar, Maribel I. García-Ibáñez,,
Unit 4-1 Provincial Practice Questions Page 1
Page 1 Page 2 Page 3 Page 4 Page 5 1.00 Page 6 Page 7 Page 8 55. The conjugate base of HAsO 4 2 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO 4 56. Consider the following acidbase equilibrium: HC 6
FIRST 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
Acids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
How many carbon atoms are in 1 mol of sucrose (C 12 H 22 O 11 )? A) 7.23 x B) 6.02 x C) 5.02 x D) 12 E) 342
Question 1 How many carbon atoms are in 1 mol of sucrose (C 12 H 22 O 11 )? A) 7.23 x 10 24 B) 6.02 x 10 23 C) 5.02 x 10 22 D) 12 E) 342 3-1 Question 2 Calculate the mass % of hydrogen in ammonium bicarbonate.
Acid-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
Carbon Dioxide, Alkalinity and ph
Carbon Dioxide, Alkalinity and ph OCN 623 Chemical Oceanography 15 March 2018 Reading: Libes, Chapter 15, pp. 383 389 (Remainder of chapter will be used with the classes Global Carbon Dioxide and Biogenic
Answers for UNIT ONE NAT 5 Flash Cards
Answers for UNIT ONE NAT 5 Flash Cards 1. (a) rate increases (b) rate increases (c) rate increases (d) rate increases 2. Average rate = change in property / change in time Where property = concentration,
Chapter 10 - Acids & Bases
Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic
Honors General Chemistry Test 3 Prof. Shattuck, practice
Honors General Chemistry Test 3 Prof. Shattuck, practice Name R = 8.314 J mol -1 K -1 1 L atm = 101.3 J T(0 C) = 273.2 K Answer 8 of the following 10 questions. If you answer more than 8 cross out the
****************************************************************************
**************************************************************************** To quickly summarize: 1. The solubility of a compound is decreased when an ion which is the same as one of the ions in the compound
Chem12 Acids : Exam Questions M.C.-100
Chem12 Acids : Exam Questions M.C.-100 1) Given : HPO 4 2- (aq) + NH 4 + (aq) H 2 PO 4 - (aq) + NH 3 (aq), the strongest acid in the above equation is : a) NH 4 + b) HPO 4 2- c) NH 3 d) H 2 PO 4-2)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) What is a dominant equilibrium? How do we define major species? Reactions between acids and bases 1. Strong Acids + Strong Base The reaction
Ionic Compounds. And Acids
CHAPTER 7 LANGUAGE OF CHEMISTRY CLASSIFICATION OF COMPOUNDS Inorganic compounds does not contain the element carbon, but there are exception to this rule, CO 2 (carbon dioxide), CO 3 2 (carbonate), and
Chapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
Salinity. foot = 0.305m yard = 0.91m. Length. Area m 2 square feet ~0.09m2. Volume m 3 US pint ~ 0.47 L fl. oz. ~0.02 L.
Length m foot = 0.305m yard = 0.91m Area m 2 square feet ~0.09m2 Volume m 3 US pint ~ 0.47 L, L (liters) fl. oz. ~0.02 L Speed m/s mph Acceleration m/s 2 mph/s Weight kg, gram pound ~0.45kg Temperature
CHM 112 Dr. Kevin Moore
CHM 112 Dr. Kevin Moore Reaction of an acid with a known concentration of base to determine the exact amount of the acid Requires that the equilibrium of the reaction be significantly to the right Determination
Problem 1. What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10-5 )?
Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10-5 )? Problem 2 A 489mL sample of 0.5542M HNO 3 is mixed with 427mL sample of NaOH (which has a ph of 14.06).
OCN400 Problem Set #1 Winter 2015 Due: 9:30 a.m., Monday, Jan 12
OCN400 Problem Set #1 Winter 2015 Due: 9:30 a.m., Monday, Jan 12 1. What determines if an ion is a major ion in seawater? (5) - Major ions are those that contribute to salinity. - If salinity can be determined
Chapters 6 and 8. Systematic Treatment of Equilibrium
Chapters 6 and 8 Systematic Treatment of Equilibrium Equilibrium constants may be written for dissociations, associations, reactions, or distributions. Gary Christian, Analytical Chemistry, 6th Ed. (Wiley)
CHEMISTRY 102 Fall 2010 Hour Exam III. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
1. My answers for this Chemistry 10 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml of 0.30 M HCN by 0.10
Chemistry 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
Chapter 9 Acids & Bases
Chapter 9 Acids & Bases 9.1 Arrhenius Acids and Bases o Arrhenius Acid: substance that produces H + ions in aqueous solutions. HCl (aq) H + (aq) + Cl - (aq) o Arrhenius Base: substance that produces OH
Contents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
Chapter 2: Acids and Bases
1. Which of the following statements is a correct definition for a Brønsted-Lowry acid? A) Proton acceptor C) Electron pair acceptor B) Electron pair donor D) Proton donor 2. Which of the following statements
Acids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H ], (also thought of as hydronium ion, H O ) when dissolved in water. Acids
OCN 201. Chemistry & Physics of the Ocean. (but no need to panic) foot = 0.305m yard = 0.91m. Length. Area m 2 square feet ~0.09m2
Chemistry & Physics of the Ocean OCN 201 (but no need to panic) Length m foot = 0.305m yard = 0.91m Area m 2 square feet ~0.09m2 Volume m 3 US pint ~ 0.47 L, L (liters) fl. oz. ~0.02 L Speed m/s mph Acceleration
CHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
Ch 16 and 17 Practice Problems
Ch 16 and 17 Practice Problems 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,