CHEM N-8 November 2003
|
|
- Calvin Wells
- 7 years ago
- Views:
Transcription
1
2 CHEM N-8 November 2003 The H 2 PO 4 and HPO 4 2 ions play a major role in maintaining the intracellular ph balance. Write balanced equations to show how a solution containing these ions can act as a buffer. Marks 6 The presence of H 2 PO 4 (aq) means that the solution can remove OH (aq): H 2 PO 4 (aq) + OH (aq) HPO 2 4 (aq) + H 2 O(l) The presence of HPO 2 4 (aq) means that the solution can remove H + (aq): HPO 2 4 (aq) + H + (aq) H 2 PO 4 (aq) For phosphoric acid, K a1 = M, K a2 = M, K a3 = M. At what ph would the H 2 PO 4 / HPO 4 2 buffer system be most effective? Why? Buffers are most effective when [acid] = [base] at which point ph = pk a. For this system, this requires [H 2 PO 4 - (aq)] = [HPO 4 2- (aq)]. This acid / base equilibrium corresponds to K a2 : H 2 PO 4 - (aq) HPO 4 2 (aq) + H + (aq) Thus, ph = pk a2 = -log 10 ( ) = 7.20 Calculate the ratio of H 2 PO 4 / HPO 4 2 needed to give a solution buffered to a ph of Using the Henderson-Hasselbalch equation: [base] ph = pk a + log10 [acid] or [base] log10 [acid] = ph - pk a Thus: log 10 [base] [acid] = ph pk a2 = = 0.15 [base] [acid] or [acid] [base] 1.4
3 CHEM N-9 November 2004 Find the concentration of H 3 O + in a 0.60 M aqueous solution of nitrous acid. The acid dissociation constant of HNO 2 is K a = M. Marks 2 The reaction table is: HNO 2 H 2 O H 3 O + - NO 2 initial 0.60 large 0 0 change -x negligible +x +x final 0.60 x large x x The equilibrium constant K a is given by: K a 2 [H3O (aq)][no 2 (aq)] x [HNO (aq)] 0.60 x 2 = K a is very small compared to the initial concentration of HNO 2 so that 0.60 x ~ 0.60 and so: x 2 ~ ( ) (0.60) so x = [H 3 O + (aq)] = x = M Answer: M An aqueous solution of a weak acid has [H 3 O + ] = M. Find the ph and poh of the solution. 1 Using ph = -log 10 ([H 3 O + (aq)]) and ph + poh = 14.00: ph = -log 10 ( ) = 3.60 poh = = ph = 3.60 poh = Ammonia, NH 3, is a Brønsted-Lowry base and a Lewis base, but not an Arrhenius base. Why? 3 A Brønsted-Lowry base is a proton (H + ) acceptor: NH 3 + H + NH 4 + A Lewis base is a species that can donate a lone pair: :NH 3 + H + NH 4 + An Arrhenius base is one that contains OH ions that are released on dissolution in water. Ammonia generates OH ions in its reaction with water but does not contain them in its formula and hence it is not an Arrhenius base.
4 CHEM N-3 November 2006 Explain why the acidity of hydrogen halides increases with increasing halogen size (i.e., K a (HCl) < K a (HBr) < K a (HI)), while the acidity of hypohalous acids decreases with increasing halogen size (i.e., K a (HOCl) > K a (HOBr) > K a (HOI)). 3 For the hydrogen halides, the length of the H-X bond increases and hence gets weaker as the halogen gets bigger,. The weaker the bond, the more easily the H + dissociates. For the hypohalous acids, as the electronegativity of the halide increases, the more electron density it pulls from the O-H bond towards itself. This results in the O-H bond becoming more polar and increasing the ease with which the H + will be lost.
5 CHEM N-4 November 2006 The K a of benzoic acid is M at 25 C. Calculate the ph of a M aqueous solution of sodium benzoate (C 6 H 5 COONa). Marks 5 As benzoic acid is a weak acid, its conjugate base, C 6 H 5 COO -, is a weak base and so [OH ] must be calculated using the reaction table: C 6 H 5 COO H 2 O OH C 6 H 5 COOH initial large 0 0 change -x negligible +x +x final x large x x The equilibrium constant K b is given by: K b = [OH ][C6H5COOH] = [C H COO ] x x For an acid and its conjugate base in aqueous solution, K a K b = K w = Hence, K b = = As K b is very small, x ~ and hence: x 2 = ( ) or x = M = [OH (aq)] Hence, the poh is given by: poh = log 10 [OH ] = log 10 [ ] = 5.9 Finally, ph + poh = 14.0 so ph = = 8.1 Answer: ph = 8.1 Answer: ph = 4.1 ANSWER CONTINUES ON THE NEXT PAGE
6 CHEM N-4 November 2006 A buffer solution is prepared by adding 375 ml of this M aqueous solution of sodium benzoate to 225 ml of M aqueous benzoic acid. Calculate the ph of the buffer solution. 375 ml of a of benzoate contains, moles of benzoate = volume concentration = = mol 225 ml of a of benzoic acid contains, moles of benzoic acid = = mol The mixture has a volume of ( ) = 600 ml so the concentrations of benzoate (base) and benzoic acid (acid) are: [base] = number of moles volume = = M [acid] = = M As pk a = -log 10 K a, pk a = -log 10 ( ) = 4.2 The ph of the buffer can be calculated using the Henderson-Hasselbalch equation, [base] ph = pk a + log10 [acid] = log = 4.1 Answer: ph = 4.1
7 CHEM N-2 November 2007 A ml solution of HCl has a ph of Given that the pk a of iodic acid, HIO 3, is 0.79, how many moles of sodium iodate, NaIO 3, would need to be added to this solution to raise its ph to 2.00? 3 Using ph = -log 10 [H + (aq)], [H + (aq)] initial = = M [H + (aq)] final = = M Using ph = -log 10 [H + (aq)], [H + (aq)] initial = = M [H + (aq)] final = = M The change of ( M) = M occurs due to the reaction with IO 3 - (aq) to produce HIO 3 (aq). If [IO 3 - (aq)] = x, the reaction table is: H + (aq) + IO - 3 (aq) HIO 3 (aq) initial x 0 change final x As pk a = 0.79 = -log 10 K a : K a = + 3 [H (aq)][io (aq)] (0.010) ( x 0.050) = = 10 [HIO (aq)] Thus, x = 0.86 M = [IO 3 - (aq)] initial. This concentration corresponds to a ml solution so the number of moles that have been added is: number of moles = concentration volume = (0.86 M) ( L) = 0.26 mol Answer: 0.26 mol
8 CHEM N-11 November 2007 The ph of a solution can be controlled by adding small amounts of gaseous HCl. Assuming no change in volume, calculate what the ph of the solution must be to just dissolve 1.00 g of NiS suspended in 1.0 L of water. Data: H 2 S(aq) 2H + (aq) + S 2 (aq) K = M 2 K sp (NiS) = M 2 Marks 5 For the dissolution NiS(s) Ni 2+ (aq) + S 2- (aq), K sp = [Ni 2+ (aq)][s 2- (aq)]. For the acid dissociation, H 2 S(aq) 2H + (aq) + S 2- (aq), K = [H (aq)] [S (aq)] [H S(aq)] 2 Combining these two equilibria gives, for the overall reaction, NiS(s) + 2H + (aq) Ni 2+ (aq) + H 2 S(aq), K eq = [Ni (aq)][h K 2S(aq)] sp = = = K -20 [H (aq)] The formula mass of NiS is (58.69 (Ni) (S)) g mol -1 = g mol -1. The amount in 1.00 g is therefore, number of moles = mass(g) 1.00 g = = mol 1 1 molar mass(g mol ) 90.76gmol In the dissolution NiS(s) Ni 2+ (aq) + S 2- (aq), so if mol of NiS(s) completely dissolves in 1.0 L, [Ni 2+ (aq)] = M. From the overall reaction, each mole of NiS which dissolves produces one mole of H 2 S(aq) so [H 2 S(aq)] = M. Hence, [H + (aq)] 2 = (0.011M)(0.011M) or [H + (aq)] = 0.12 M ph = -log 10 [H + (aq)] = -log 10 (0.12) = 0.94 ph = 0.94
9 CHEM N-7 November 2008 Calculate the ph of a 0.10 mol L 1 solution of HF. (The pk a of HF is 3.17.) Marks 6 HF is a weak acid so the equilibrium concentrations need to be calculated using a reaction table: HF H + (aq) F - (aq) Initial Change -x +x +x Equilibrium 0.10 x x x As pk a = -log 10 K a, at equilibrium, K a = =. =. = As K a is so small, x will be tiny and 0.10 x ~ 0.10 and so x 2 = or x = [H + (aq)] = M As ph = -log 10 [H + (aq)], ph = -log 10 ( ) = 2.09 Answer: 2.09 What mass of NaF needs to be added to ml of the above solution to make a buffer with a ph of 3.00? Using the Henderson-Hasselbalch equation for the ph of the buffer: ph = pk a + log To make a buffer with ph = 3.00 and [acid] = [HF] = 0.10 M: 3.00 = log. or log = =0.17. Hence, [F - ] = = M The number of moles in ml is thus mol. As NaF will dissolve to give one F - per formula unit, this is also the number of moles of NaF required. ANSWER CONTINUES ON THE NEXT PAGE
10 CHEM N-7 November 2008 The formula mass of NaF is (22.99 (Na) (F)) g mol -1 = g mol -1. The mass of NaF required is thus: mass = number of moles formula mass = ( mol) (41.99 g mol -1 ) = 0.28 g Answer: 0.28 g Explain why HCl is a much stronger acid than HF. Cl is a much larger atom than F and is less electronegative. The H Cl bond is therefore much longer and weaker than the H F bond. The H Cl bond is therefore easier to break and it is the stronger acid. HF is actually a weak acid. F is smaller and more electronegative than O, so the H F bond is stronger than the O H bond. There is consequently little dissociation of HF when it is dissolved in water.
11 CHEM N-5 November 2009 A solution is prepared by dissolving mol of acetic acid, mol of sodium acetate and mol of HCl in water to give a final volume of 250 ml. The pk a of acetic acid is What is the ph of this solution? Marks 3 HCl will react with the acetate to produce acetic acid: HCl + CH 3 CO 2 - CH 3 COOH + Cl - As mol of CH 3 CO 2 - is initially present, the number of moles after this reaction is ( ) mol = mol. As mol of CH 3 COOH - is initially present, the number of moles after this reaction is ( ) mol = mol. The final volume is 250 ml so the concentrations are: [CH 3 CO - 2 (aq)] =.. = M [CH 3 COOH(aq)] =.. = M The ph of the solution containing both an acid (CH 3 COOH) and its conjugate base (CH 3 CO 2 - ) is given by the Henderson-Haseelbalch equation: ph = pk a + log = log.. = 4.33 ph = 4.33
12 CHEM N-7 November 2009 A 20.0 ml solution of nitrous acid (HNO 2, pk a = 3.15) was titrated to its equivalence point with 24.8 ml of M NaOH. What is the concentration of the HNO 2 solution? Marks 7 The number of moles of OH - required in the titration is: number of moles = concentration volume = (0.020 mol L -1 ) ( L) = mol This is equal to the number of moles of HNO 2 in 20.0 ml. Hence, the concentration of HNO 2 is equal to: concentration =.. = M What was the ph at the start of the titration? Answer: M HNO 2 is a weak acid so the equilibrium concentrations need to be calculated using a reaction table: HNO 2 H 2 O H 3 O + (aq) NO 2 - (aq) Initial large 0 0 Change -x +x +x Equilibrium x x x As pk a = -log 10 K a, at equilibrium, K a = =. =. = As K a is so small, x will be tiny and x ~ and so x 2 = or x = [H 3 O + (aq)] = M As ph = -log 10 [H 3 O + (aq)], ph = -log 10 ( ) = 2.38 ph = 2.38 ANSWER CONTINUES ON THE NEXT PAGE
13 CHEM N-7 November 2009 What was the ph after (a) 12.4 ml and (b) 24.8 ml of the NaOH had been added? (a) 12.4 ml represents the half equivalence point. At this point, [HNO 2 (aq)] = [NO 2 - (aq)] and ph = pk a. Hence ph = 3.15 (b) 24.8 ml represents the equivalence point. At this point, all of the HNO 2 has been converted into NO 2 - so: number of moles of NO 2 - = mol The total volume of the solution is ( ) ml = 44.8 ml. Hence: [NO -. 2 (aq)] =. = M The solution contains a weak base. The ph needs to be calculated using a reaction table. NO 2 - H 2 O HNO 2 (aq) OH - (aq) Initial large 0 0 Change -y +y +y Equilibrium y y y As pk a + pk b = 14.00, pk b = = At equilibrium, K b = =. = As K b is so small, y will be tiny and y ~ and so y 2 = or y = [OH - (aq)] = M As poh = -log 10 [OH - (aq)], poh = -log 10 ( ) = 6.40 Finally, as ph + poh = 14.00, ph = = 7.60 (a) 12.4 ml: ph = 3.15 (b) 24.8 ml: ph = = ANSWER CONTINUES ON THE NEXT PAGE
14 CHEM N-7 November 2009 Qualitatively, how would each of these three ph values be affected if M NH 3 had been used in place of the NaOH solution? The pk b of NH 3 is The initial ph is unchanged as no base is present. As pk b for NH 3 is 4.76, pk a for its conjugate acid NH 4 + is ( ) = The half equivalence point is in the acidic region of the titration (it is at ph = 3.15 for the weak acid / strong base titration above). This ph is considerably lower the pk a value of NH 4 + and so essentially all of the NH 3 will be present as NH 4 + and it will not contribute to [H 3 O + (aq). The ph at the half-equivalence point will be the same as it depends only on the pk a of HNO 2. The ph at the equivalence point will be lower. At equivalence, the solution will contain NO 2 - as in the HNO 2 / OH - titration. It will also contain NH 4 +, the conjugate acid of NH 3. As this is weakly acid, the ph will be lowered.
CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?
You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4
More informationChapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
More informationAcid-Base Chemistry. Brønsted-Lowry Acids & Bases
Acid-Base Chemistry ν There are a couple of ways to define acids and bases ν Brønsted-Lowry acids and bases ν Acid: H + ion donor ν Base: H + ion acceptor ν Lewis acids and bases ν Acid: electron pair
More informationName period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see
More informationWrite the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.
Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called
More informationChem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria
Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria Key Questions 1. A 0.0100 M solution of a weak acid HA has a ph of 2.60. What is the value of K a for the acid? [Hint: What
More informationReview for Solving ph Problems:
Review for Solving ph Problems: Acid Ionization: HA H 2 O A - H 3 O CH 3 COOH H 2 O CH 3 COO - H 3 O Base Ionization: B H 2 O BH OH - 1) Strong Acid complete dissociation [H ] is equal to original [HA]
More informationCHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +
More informationSince we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.
Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the
More informationAcids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
More informationChemical equilibria Buffer solutions
Chemical equilibria Buffer solutions Definition The buffer solutions have the ability to resist changes in ph when smaller amounts of acid or base is added. Importance They are applied in the chemical
More informationChapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water
Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF
More informationQUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -
QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions
More informationAcids and Bases. Chapter 16
Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following
More informationChapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More informationNote: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-
AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +
More informationCHAPTER 18 ACID-BASE EQUILIBRIA
CHAPTER 18 ACID-BASE EQUILIBRIA 18.1 The Arrhenius definition classified substances as being acids or bases by their behavior in the solvent water. 18. All Arrhenius acids contain hydrogen and produce
More informationChapter 14 - Acids and Bases
Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry
More informationCHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
More informationCopyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.
Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of
More information3 The Preparation of Buffers at Desired ph
3 The Preparation of Buffers at Desired ph Objectives: To become familiar with operating a ph meter, and to learn how to use the Henderson-Hasselbalch equation to make buffer solutions at a desired ph
More informationAcid-Base (Proton-Transfer) Reactions
Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius
More information6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must
More informationTitrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration
Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical
More informationph. Weak acids. A. Introduction
ph. Weak acids. A. Introduction... 1 B. Weak acids: overview... 1 C. Weak acids: an example; finding K a... 2 D. Given K a, calculate ph... 3 E. A variety of weak acids... 5 F. So where do strong acids
More informationChapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50
Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs
More informationp3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic
General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10
More informationCHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
More informationAn acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationAcid-Base Equilibrium
AcidBaseEquil 1 Acid-Base Equilibrium See AqueousIons in Chemistry 1110 online notes for review of acid-base fundamentals! Acid- Base Reaction in Aqueous Salt Solutions Recall that use [ ] to mean concentration
More informationChem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
More informationEquilibrium Constants The following equilibrium constants will be useful for some of the problems.
1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO
More informationChapter 15 Acids and Bases. Fu-Yin Hsu
Chapter 15 Acids and Bases Fu-Yin Hsu Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria To help break down food To activate enzymes that break
More informationACID-BASE REACTIONS/ THE PH CONCEPT.
Dr Mike Lyons School of Chemistry Trinity College Dublin. melyons@tcd.ie ACID-BASE REACTIONS/ THE PH CONCEPT. Chemistry Preliminary Course 2011 1 Lecture topics. 2 lectures dealing with some core chemistry
More informationph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
More informationAcid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases
Acids Identifying Acids and Bases Acid (anhydrides) contains H+ ions as the cation, with and other element as the anion Non-metal oxide H2SO4 HI P2O5 Bases Base (anhydrides) Contains OH- as the anion Combined
More informationChapter 14: Acids and Bases
Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid
More informationUnit Two: Acids and Bases
Section One: Theoretical Stuff Unit Two: Acids and Bases The concept of acids and bases has existed for centuries. We can discuss them two ways, operational definitions and theoretical definitions. 1.
More informationCHAPTER 16: ACIDS AND BASES
CHAPTER 16: ACIDS AND BASES Active Learning: 4, 6, 14; End-of-Chapter Problems: 2-25, 27-58, 66-68, 70, 75-77, 83, 90-91, 93-104 Chapter 15 End-of-Chapter Problems: 69-74, 125, 129, 133 16.1 ACIDS AND
More informationAcid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!!
Acid/Base Reactions some covalent compounds have weakly bound H atoms and can lose them to water (acids) some compounds produce OH in water solutions when they dissolve (bases) acid/base reaction are very
More informationUNIT (6) ACIDS AND BASES
UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that
More informationI N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
More informationAP FREE RESPONSE QUESTIONS ACIDS/BASES
AP FREE RESPONSE QUESTIONS ACIDS/BASES 199 D A chemical reaction occurs when 100. milliliters of 0.200molar HCl is added dropwise to 100. milliliters of 0.100molar Na 3 P0 solution. (a) Write the two net
More informationTopic 5. Acid and Bases
Topic 5 5-1 Acid and Bases Acid and Bases 5-2 There are a number definitions for aicd and bases, depending on what is convenient to use in a particular situation: Arrhenius and Ostwald: Theory of electrolyte
More informationTopic 8 Acids and bases 6 hours
Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates
More informationWe remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point.
Titrations Titration - a titration is defined as the determination of the amount of an unknown reagent (analyte) through the use of a known amount of another reagent (titrant) in an essentially irreversible
More informationstoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
More informationNH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid
Acid-Base Concepts -- Chapter 15 1. Arrhenius Acid-Base Concept (last semester) Acid: H+ supplier Base: OH- supplier 2. Brønsted-Lowry Acid-Base Concept (more general) (a) Definition (H+ transfer) Acid:
More informationAcids and Bases HW PSI Chemistry
Acids and Bases HW PSI Chemistry Name 1) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H + B) causes an increase in the concentration of H + in
More informationAcids and Bases. Problem Set: Chapter 17 questions 5-7, 9, 11, 13, 18, 43, 67a-d, 71 Chapter 18 questions 5-9, 26, 27a-e, 32
Acids and Bases Problem Set: Chapter 17 questions 5-7, 9, 11, 13, 18, 43, 67a-d, 71 Chapter 18 questions 5-9, 26, 27a-e, 32 Arrhenius Theory of Acids An acid base reaction involves the reaction of hydrogen
More informationChapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon
Chapter 16 Acid-Base Equilibria Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon dioxide dissolves in water, it forms carbonic acid, H 2 CO 3. Basic solutions
More informationSimilarities The ph of each of these solutions is the same; that is, the [H + ] is the same in both beakers (go ahead and count).
Compare 1 L of acetate buffer solution (0.50 mol of acetic acid and 0.50 mol sodium acetate) to 1 L of HCl solution AcO - AcO - H+ Cl - AcO - AcO - Cl - Cl - AcO - Cl - Cl - Cl - Cl - AcO - AcO - AcO -
More informationChapter 13 & 14 Practice Exam
Name: Class: Date: Chapter 13 & 14 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Acids generally release H 2 gas when they react with a.
More information3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation
Lecture Presentation Chapter 15 Acids and Bases Sherril Soman Grand Valley State University Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria
More information4. Acid Base Chemistry
4. Acid Base Chemistry 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B + HA
More informationChemistry 201. Practical aspects of buffers. NC State University. Lecture 15
Chemistry 201 Lecture 15 Practical aspects of buffers NC State University The everyday ph scale To review what ph means in practice, we consider the ph of everyday substances that we know from experience.
More informationCh 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent
1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled
More information5.111 Principles of Chemical Science
MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. Page 1 of 10 pages
More informationCHEM1909 2006-N-2 November 2006
CHEM1909 006-N- November 006 High-purity benzoic acid, C 6 H 5 COOH, (H comb = 37 kj mol 1 ) is used to calibrate a bomb calorimeter that has a 1.000 L capacity. A 1.000 g sample of C 6 H 5 COOH is placed
More informationChemistry 106 Fall 2007 Exam 3 1. Which one of the following salts will form a neutral solution on dissolving in water?
1. Which one of the following salts will form a neutral solution on dissolving in water? A. NaCN B. NH 4 NO 3 C. NaCl D. KNO 2 E. FeCl 3 2. Which one of the following is a buffer solution? A. 0.10 M KCN
More informationTOPIC 11: Acids and Bases
TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react
More informationVolumetric Analysis. Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115
Volumetric Analysis Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115 Experimental Aims To prepare and standardize (determine concentration) a NaOH solution Using your standardized NaOH calculate
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationWorksheet 23 Strong Acid/Strong Base Titrations
Worksheet 2 Strong Acid/Strong Base Titrations A. Initial ph This is always determined based solely on the initial concentration of the acid or base being titrated. Every mole of acid or base will produce
More informationAcid-Base Titrations. Setup for a Typical Titration. Titration 1
Titration 1 Acid-Base Titrations Molarities of acidic and basic solutions can be used to convert back and forth between moles of solutes and volumes of their solutions, but how are the molarities of these
More informationAnswer Key, Problem Set 5 (With explanations)--complete
Chemistry 122 Mines, Spring 2016 Answer Key, Problem Set 5 (With explanations)complete 1. NT1; 2. NT2; 3. MP; 4. MP (15.38); 5. MP (15.40); 6. MP (15.42); 7. NT3; 8. NT4; 9. MP; 10. NT5; 11. NT6; 12. MP;
More informationCommon Ion Effects. CH 3 CO 2 (aq) + Na + (aq)
Common Ion Effects If two reactions both involve the same ion, then one reaction can effect the equilibrium position of the other reaction. The ion that appears in both reactions is the common ion. Buffers
More informationTopic 18 Acids and Bases. 18.1 Exercises
Topic 18 Acids and Bases 18.1 Exercises 1. Define: (a) ph The negative log of the hydrogen ion concentration in a solution. i.e. ph = log[h 3 O + ] (b) poh The negative log of hydroxide ion concentration
More informationAP*Chemistry The Chemistry of Acids and Bases
AP*Chemistry The Chemistry of Acids and Bases "ACID"--Latin word acidus, meaning sour. (lemon) "ALKALI"--Arabic word for the ashes that come from burning certain plants; water solutions feel slippery and
More informationStoichiometry and Aqueous Reactions (Chapter 4)
Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.
More informationQ1: What is the ph Scale? Q6: As acids become more acidic, their ph values
Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values increase or decrease? Q2: The range of values of the ph scale is: Q7: As bases become more alkaline, their ph values increase
More informationACID-BASE TITRATIONS
ACID-BASE TITRATIONS 1 In this exercise you will use Excel to construct titration curves for a titration between a strong acid and strong base and between a weak acid and strong base. To set up a spreadsheet
More information10. Acids, Bases, and Salts. Acids and bases. 10.1 Arrhenius Acid-Base Theory. 10.2 Bronsted-Lowry Acid-Base Theory
10. Acids, Bases, and Salts Acids and bases For centuries people have known acids are in vinegar, lemon juice and many other foods taste sour. Only few hundred years ago that it was discovered that acids
More informationChemistry 3202. Unit 2 Acids and Bases
Chemistry 3202 Unit 2 Acids and Bases Definitions of Acids and Bases An operational definition is one that is based on the observable properties, behaviours or uses of an entity. The earliest definitions
More informationBalance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O
Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent
More informationINTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationGeneral Chemistry II Chapter 20
1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water
More informationSuggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99
Chemistry I Accelerated Study Guideline - Chapter 19 Acids, Bases and Salts ------------------------------------------------------------------------------ By the end of this unit, the skills you should
More informationClassification of Reagents in Chemistry I: Acids and Bases
University of Califnia, Davis F use with UC Davis Chem 8 and 118 Series Classification of Reagents in Chemistry I: Acids and Bases There are 3 definitions of acids and bases. All three are used in both
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationChapter 9 Lecture Notes: Acids, Bases and Equilibrium
Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether
More informationCh 15: Acids and Bases
Ch 15: Acids and Bases A c i d s a n d B a s e s C h 1 5 P a g e 1 Homework: Read Chapter 15 Work out sample/practice exercises in the sections, Bonus problems: 39, 41, 49, 63, 67, 83, 91, 95, 99, 107,
More informationAcids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA
Acids and Bases An Introduction David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Properties of Acids 1. Sour taste (examples: vinegar, citric acid, lemon juice) 2. Turns litmus
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationEquilibria Involving Acids & Bases
Week 9 Equilibria Involving Acids & Bases Acidic and basic solutions Self-ionisation of water Through reaction with itself: The concentration of water in aqueous solutions is virtually constant at about
More informationProperties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases
CAPTER Acids, Bases and Salts Properties of Aqueous Solutions of Acids and Bases Strong and Weak Acids Acids are substances that generate in aqueous solutions. Strong acids ionize 0% in water. That is,
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationElectrical Conductivity of Aqueous Solutions
Electrical Conductivity of Aqueous Solutions PRE-LAB ASSIGNMENT: Reading: Chapter 4.-4.3 in Brown, LeMay, Bursten & Murphy.. Using Table in this handout, determine which solution has a higher conductivity,.
More informationAP Chemistry Summary Acids, Bases and Buffers Definitions:
AP Chemistry Summary Acids, Bases and Buffers Definitions: Arrhenius: Acid - Produces H + ions in solution HCl H + (aq) + Cl - (aq) Base - Produces OH - ions in solution NaOH Na + (aq) + OH - (aq) Dissociation
More informationChemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
More informationBuffer solutions. Division of Radiooncology, Deutsches Krebsforschungszentrum, 69120 Heidelberg, Germany
Buffer solutions WOLF D. KUHLMANN, M.D. Division of Radiooncology, Deutsches Krebsforschungszentrum, 69120 Heidelberg, Germany Aqueous buffer solutions and acid-base reactions Buffer solutions have the
More informationAcids and Bases CHAPTER 12. Opening Essay
CHAPTER 12 Acids and Bases Opening Essay Formerly there were rather campy science-fiction television shows in which the hero was always being threatened with death by being plunged into a vat of boiling
More informationChemical Calculations
Moles and Molecules Moles and Chemical Reactions Moles, Chemical Reactions, and Molarity All done as UNIT CONVERSIONS!!! and practice, practice, practice CHM 1010 Sinex 1 Mass moles particles conversions
More informationChapter 2 Polar Covalent Bonds: Acids and Bases
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds: Acids and Bases Modified by Dr. Daniela R. Radu Why This Chapter? Description of basic ways chemists account for chemical
More information