Lecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
|
|
- Kelley Mathews
- 5 years ago
- Views:
Transcription
1 Lecture 10 Professor Hicks Inorganic Chemistry II (CHE152) ph Scale of [H 3 O + ] (or you could say [H + ]) concentration More convenient than scientific notation ph = log [H 3 O + ] still not sure? take the log of 10 it should be 1 [H 3 O + ] 1
2 poh Same idea as ph Scale of OH concentration poh = log [OH ] [H 3 O + ] K eq pk eq K eq values vary over a VERY wide range K eq and K eq As an alternative to using scientific notation often expressed a pk eq values For example K eq for acids K a pk a K eq for bases K b pk b K eq for autoionization of water K w pk w 2
3 ph, poh, and pk w ph + poh = 14 Why? [H 3 O + ][OH ] = ) take log both sides 2) log(a*b) = log(a) + log(b) ph is what most people think in terms of some problems we get a result [OH] or poh use this equation to express it as a ph ph + poh = log(10 14 ) = 14 ph = 14 poh ph fun facts! Bacteria that are not harmful tend to grow in acidic conditions (acidophilus strains) More harmful bacteria tend to grow in basic conditions Blood ph about 7.4 Stomach ph 1.5! Acid rain lowers ph of environment dissolving Al(OH) 3 solid 3
4 Why is ph (in other words [H + ]) important? H + and OH form from water Life on earth exists in water H + and OH promote numerous reactions as catalysts Their concentration must be carefully controlled a ph change of 0.50 causes irreversible damage change in [ H + ] of only 9.6x10 7!!! ph poh [OH ] [H + ] ph poh = 14 ph ph = 14 poh poh [H + ] = 10 ph ph = log [H + ] [OH ] = 10 poh poh = log [OH ] [H + ] [OH ] = [H + ] [H + ] = [OH ] [OH ] 4
5 5
6 6
7 7
8 8
9 bases NaOH Sr(OH) 2 9
10 Monoprotic Acids Monoprotic acids acids that provide only one H + (H 3 O + ) Common examples of monoprotic acids are here H 2 SO 4 is a diprotic acid H 3 PO 4 is a triprotic acid We will only cover calculations for monoprotic acids 10
11 Dissociation of weak acids Calculate [H 3 O + ] at equilibrium for a 0.55 M solution of HF in water. Write a hydrolysis reaction Acid + H 2 O H 3 O + + conj base initial (M) change (M) equilibrium (M) HF (aq) + H 2 O (l) H 3 O + (aq) + F (aq) x +x +x 0.55x +x +x K a = [H 3 O + ][F] [HF] to solve for x you could use the quadratic equation a quicker alternative is to look for an approximation look up K a for HF x x 10 4 = x =??? 0.55x if x is very small compared to x 10 4 = x x = sqrt{ 0.55* 7.1 x 10 4 } = M x = change in [HF] to reach equilibrium, and is also final equilibrium molarities for [H 3 O + ], [F ] Percent Dissociated (aka percent ionized) % Dissociated = x Initial molarity x 100% Initial molarity HF before dissociation dissolve Initial molarity x HF (aq) H + (aq) F (aq) x at equilibrium 11
12 initial (M) change (M) equilibrium (M) Dissociation of weak acids HF (aq) + H 2 O (l) H 3 O + (aq) + F (aq) x +x +x 0.55x +x +x K a = [H 3 O + ][F] [HF] to solve for x you could use the quadratic equation a quicker alternative is to look for an approximation x x 10 4 = x =??? 0.55x % dissociated is is small compared to 0.55 M? if x is very small compared to 0.55 x 100% = 3.6% 7.1 x 10 4 = x x = sqrt{ 0.55* 7.1 x 10 4 } = M 5% error is widely accepted in science Approximation is valid b/c % dissociated is less than 5% Le Chateliers Principle and % dissociated HF + H 2 O F + H 3 O + K a = 7.1 x 10 4 ~100% 90% 10% 40% 50% 60% 70% 80% 1% 30% at infinite dilution percent dissociated disturbance = increase H 2 O (dilute acid) 1.0 M 0.10 M M response = decrease [H 2 O] M etc 12
13 1) Break into groups of 23 each group will be assigned an acid 2) Use the approximation method to estimate the ph and % dissociated. If more than 5% is dissociated at equilibrium then the approximation is not good. Acid Acid Concentration K a [H 3 O + ] diss 1) HF 4.50E E E02 2) HNO E E E02 3) C 9 H 8 O E E E03 4) HCOOH 1.08E E E03 5) C 6 H 8 O E E E03 6) C 6 H 5 COOH 6.09E E E03 7) CH 3 COOH 1.26E E E04 8) HCN 3.48E E E08 9) C 6 H 5 OH 1.26E E E09 13
14 A M solution of a weak acid is found to have a ph of What is the K a of this weak acid? What is this acid s pk a value? 14
15 Calculate the ph of a M solution of acetic acid. Confirm that your calculation is valid by calculating the percent dissociated. Ionization of weak bases Calculate ph at equilibrium for a 0.10 M solution of Na 2 CO 3 in water. write hydrolysis reaction base + H 2 O conj acid + OH initial (M) change (M) equilibrium (M) K b = [OH ][HCO 3 ] [CO 3 2 ] look up K b for CO x 10 4 = x x CO 2 3 (aq) + H 2 O (l) HCO 3 (aq) + OH (aq) x +x +x 0.10 x x x 1.8 x 10 4 = x x = sqrt{ 0.10* 1.8 x 10 4 } = M % ionized= x100% = 4.2 % less than 5%! approximation is OK poh = log [OH ] = log ( )=2.37 ph=142.37=
16 Weak bases React with water to produce OH Base + H 2 O BaseH + + OH hydrolysis reaction NH 3 (aq) + H 2 O (l) NH 4 + (aq) + OH (aq) Do not react completely Equilibrium constant K b 16
17 Aniline is a weak base. If a 0.95 M solution of aniline is % ionized, what is the K b value for aniline? 17
18 Determine the ph of a 4.0 x 10 3 M solution of methylamine (CH 3 NH 2 ). 18
19 19
20 20
21 Weak acids and the salts of their conjugate bases Acids H + + anion H+ anion If an acid is uncharged its conjugate base is negatively charged Conjugate bases of acids exist as ionic compounds aka salts Often from group I since all group I salts are soluble Salts of acids replace H + any cation + anion Na + anion K + anion Strong acids HCl HNO 3 H 2 SO 4 H + Cl H + NO 3 2H + SO 2 4 hydrochloric acid nitric acid sulfuric acid Weak acids HC 2 H 3 O 2 HF H + C 2 H 3 O 2 H + F acetic acid hydrofluoric acid Salts of Strong acids LiCl NaNO 3 K 2 SO 4 Li + Cl Na + NO 3 2K + SO 2 4 lithium chloride sodium nitrate potassium sulfate Salts of Weak acids Mg(C 2 H 3 O 2 ) 2 CsF Mg 2+ 2C 2 H 3 O 2 Cs + F magnesium acetate cesium fluoride Weak base compound with lone pairs often a N containing compound H N H Weak bases and the salts of their conjugate acids ammonia H H N R H If a base is uncharged its conjugate acid is positively charged Conjugate acids of bases exist as ionic compounds aka salts amines H H H N H Salt of its conjugate acid + anion H H and H N R H + anion When they act as bases gaining H + they become positively charged examples NH 4 Cl CH 3 NH 3 (ClO 4 ) H 21
22 Salts of weak acids/bases If soluble fully dissociate into ions Initial molarity calculated from chemical formula 0.33 M NaC 2 H 3 O 2 a solution 0.33 M in C 2 H 3 O M Ca(C 2 H 3 O 2 ) 2 a solution 0.48 M in C 2 H 3 O 2 2 C 2 H 3 O 2 per 1 Ca(C 2 H 3 O 2 ) M NH 4 Br a solution 0.24 M in NH 4 + Ions of group I Li +, Na +, K + = etc. have no effect on ph Ions of group II Mg 2+, Ca 2+, Ba 2+ = etc. have a very small acidic effect on ph Both are often treated as being spectator ions that do not affect ph if any other acid or base is present at a significant concentration. K a K b = K w For acetic acid the hydrolysis reaction is HC 2 H 3 O 2 (aq) + H 2 O(l) C 2 H 3 O 2 (aq) + H 3 O + (aq) K a =1.76 x10 5 for acetate ion the hydrolysis reaction is C 2 H 3 O 2 (aq) + H 2 O HC 2 H 3 O 2 (aq) + OH (aq) K b =5.68 x10 10 notice if you add them the conjugate acid and base cancel overall reaction becomes 2H 2 O(l) H 3 O + (aq) + OH (aq) K w =? Remember when reactions are added the overall K eq is the product of the K eq s K a K b = 1.76 x10 5 x 5.68 x10 10 = 10 14!!!!!!!!! 22
23 You will not have this half of the table for the exam You will not have this half of the table for the exam 23
24 ICE tables for salts of weak acids What is the ph of a 0.66 M solution of sodium acetate? C 2 H 3 O 2 (aq) + H 2 O HC 2 H 3 O 2 (aq) + OH (aq) Initial Change Equililibrium x +x +x 0.66x +x +x By the usual approximation x = square root (0.66*5.68 x ) = x 10 5 [OH ] = x 10 5 poh = 4.71 ph = = 9.29 acetate ion K b = K a (acetic acid) A basic solution b/c we added the conjugate base of acetic acid = x10 5 = 5.68 x10 10 This problem is setup like other weak base problems, but you must recognize it as the conjugate base of a weak acid ICE tables for salts of weak bases What is the ph of a 0.66 M solution of ammonium chloride? NH 4 + (aq) + H 2 O NH 3 (aq) + H 3 O + (aq) initial change equil x +x +x 0.33x +x +x By the usual approximation x = square root (0.33*5.56 x ) = 1.35 x 10 5 [H 3 O + ] = 1.35 x 10 5 ph = 4.87 An acidic solution b/c we added the conjugate acid of ammonia Ammonium ion K a = K b (ammonia) = x10 5 = 5.56 x
25 (so weak they do not affect ph) alcohols C 2 H 5 OH H 2 O weaker weak acids HCN Weak acids stronger weak acids HClO 2 Strong Acids HCl, HBr, HI, HNO 3, HClO 4, H 2 SO 4 Increasing Acid Strength Strong bases C 2 H 5 O OH Conjugate bases of weak acids stronger weak bases CN weaker weak bases ClO 2 Conjugate bases of Strong Acids (so weak they do not affect ph) Cl, Br, I, NO 3, ClO 4, HSO 4 Increasing Base Strength Determine the ph of a M solution of methyl amine bromide (CH 3 NH 3 Br) 25
26 Determine the ph of a M solution of sodium benzoate (NaC 7 H 5 O 2 ) Buffers Buffers = solutions that resist ph changes Act by neutralizing added acid or base Made by preparing a solution of a weak acid/base and the salt of its conjugate acid/base Most of the weak acid does not dissociate into H 3 O + but it can react with OH Most of the weak base does not react to form OHbut it can react with any H 3 O + that is added HC 2 H 3 O 2 HC 2 H 3 O 2 C 2 H 3 O 2 H + H + HC 2 H 3 O C 2 2 H 3 O 2 HC 2H 3 O 2 H + H + H + HC 2 H 3 O 2 C 2 H 3 O 2 Free H + determines the ph but all the H can react with added OH The overall effect is that the ph will not change as much as water would if a strong acid or base was added 26
27 Making a Buffer How buffers work against strong acid new HA H 2 O HA + H 3 O + HA (an acid) A (conjugate base) Added H 3 O + 27
28 new A How buffers work against strong base H 2 O HA A HA A + H 3O + Added HO pk a and pk b K a and K b values vary over a wide range Smaller than Larger than Often shown in tables as pk a or pk b to avoid need for scientific notation pk a = log(k a ) pk b = log(k b ) Stronger acids have lower pk a values 28
29 HendersonHasselbach Equation Used to calculate ph of buffer solution Equation derived from the K a expression Input = initial concentrations of the weak acid and conjugate base Where: pk a = log(k a ) ph p K a B log A B = molarity or # of moles of the base A = molarity or # of moles of the acid 29
30 Example: What is the ph of a buffer that is M HC 7 H 5 O 2 and M NaC 7 H 5 O 2? HC 7 H 5 O 2 + H 2 O C 7 H 5 O 2 + H 3 O + [A ] ph pk a log [HA] ph log ph 4.66 log K a for HC 7 H 5 O 2 = 6.5 x 10 5 pk a log K a Recognize chemical formula has 2 oxygen atoms it is a carboxylic acid weak acid The other substance is its conjugate base It is a buffer so use the HHA equation Effectiveness of Buffers A buffer will be most effective against acids and bases when B/A = 1 equal amounts of acid and base Reasonably effective when 0.1 < B/A < 10 Buffers always have a larger capacity when B and A amounts are both higher 30
31 Example: Calculate the ph of a solution prepared so that it was M in nitrous acid (HNO 2 ) and 0.10 M in sodium nitrite (NaNO 2 ). This solution is a buffer b/c we have a weak acid and its conjugate bases use the HH eqn 1) look up K a 2) calculate pk a 3) calculate [B]/[A] ph = pk a + log([b]/[a]) B = NO 2 A =HNO 2 K a = 4.6 x 10 4 ph = log (1.17) ph = [B]/[A] = 0.10/0.085 = 1.17 pk a = log (4.6 x10 4 ) = Example: Calculate the ph of a solution prepared so that it was 0.85 M in nitrous acid (HNO 2 ) and 1.0 M in sodium nitrite (NaNO 2 ). This solution is a buffer bc we have a weak acid and its conjugate bases use the HH eqn 1) look up K a 2) calculate pk a 3) calculate [B]/[A] ph = pk a + log([b]/[a]) B = NO 2 A =HNO 2 K a = 4.6 x 10 4 ph = log (1.17) [B]/[A] = 1.0/0.85 = 1.17 pk a = log (4.6 x10 4 ) = this buffer has same B/A ratio and therefore same ph as previous example 31
32 Selecting a conjugate acid/base pair for a buffer Buffers are most effective against acids and bases when B=A or B/A=1 This occurs when ph = pk a This is achieved by selecting an acid with a pk a close to desired ph This will make the B/A ratio close or equal to to 1.0 more effective buffer against acids and bases Example: Which of the following acids would be the best choice to combine with its sodium salt to make a buffer with ph 4.25? Chlorous Acid, HClO 2 pk a = 1.95 Nitrous Acid, HNO 2 pk a = 3.34 Formic Acid, HCHO 2 pk a = 3.74 Hypochlorous Acid, HClO pk a = 7.54 pk a of 3.74 is closest to the desired ph of
33 Example a) Which acid and its conjugate base would be the best choice to make a ph 4.0 buffer? b) Calculate the B/A ratio for this buffer ph = pk a + log (B/A) 4.0 = log (B/A).01 = log (B/A) = (B/A) (B/A) = 0.97 By adding a little less base than acid the ph will be lower than the pk a 33
34 Example. Calculate the B/A ratio for a buffer based on chloroacetic acid and its conjugate base with a ph=3.0 34
35 Example: Calculate how many grams of sodium trichloroacetate must be combined with 1.0 gram of trichloroacetic acid in order to make a buffer with a ph of
36 36
Lecture 7. Acids. non-metals form anions. metals form cations H+ - Professor Hicks Inorganic Chemistry (CHE152) + anion. molecular compounds
Lecture 7 Professor icks Inorganic Chemistry (CE152) Acids + + anion + - anion substances that release + ions when dissolved Strong acids Cl NO 3 2 SO 4 + Cl - + NO - 3 2 + SO 2-4 hydrochloric acid nitric
More informationLecture 8. Polyprotic Acids often acid molecules have more than one ionizable H these are called polyprotic acids. sulfuric acid is a diprotic acid
Lecture 8 Professor icks Inorganic Chemistry (CE152) Polyprotic Acids often acid molecules have more than one ionizable these are called polyprotic acids 1 = monoprotic, 2 = diprotic, 3 = triprotic Cl
More informationLecture 8. Making a Buffer. Buffers. Professor Hicks Inorganic Chemistry (CHE152)
Lecture 8 Professor Hicks Inorganic Chemistry (CHE152) Making a Buffer Buffers buffers = solutions that resist ph changes act by neutralizing added acid or base made by preparing a solution of a weak acid/base
More informationQuiz #5. Lecture 14. Professor Hicks General Chemistry (CHE132) Spring Copyright 2009 Charles Hicks. Copyright 2009 Charles Hicks
Quiz #5 Lecture 14 Professor Hicks General Chemistry (CHE132) Spring 2009 1 Making a Buffer Buffers buffers = solutions that resist ph changes act by neutralizing added acid or base made by preparing a
More informationA) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species
3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates
More informationThe 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
More informationAP Study Questions
Name: Class: Date: AP 17.1-17.2 Study Questions True/False Indicate whether the statement is true or false. 1. The extent of ionization of a weak electrolyte is increased by adding to the solution a strong
More informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
More informationCH 15 Summary. Equilibrium is a balance between products and reactants
CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium
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 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation
Chem 106 3--011 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation 3//011 1 The net ionic equation for the reaction of KOH(aq) and
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More informationCHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).
CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).
More informationAcid/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
More informationUnit 6: ACIDS AND BASES
Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric
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 informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
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 informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More informationCHEM Dr. Babb s Sections Exam #3 Review Sheet
CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
More informationChapter 16. Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationAP Study Questions
ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025
More informationCHEMISTRY 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
More informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
More informationAP Chemistry CHAPTER 16 STUDY GUIDE Acid-Base Equilibrium
AP Chemistry CHAPTER 16 STUDY GUIDE AcidBase Equilibrium 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept
More informationHA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 16.1-27 The ph of a 0.10 M solution of a weak base is 9.82. What is the K b for this base? A. 8.8 10-8 B. 2.1
More informationProton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College
16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases
More informationMarch 21, 2005 (Print Clearly)
Chemistry 202 Exam 4 KEY March 21, 2005 (Print Clearly) 1. (16 pts) Fill in the blanks with the best answer. 2 points each. (a) Consider the reaction 3A(g) + B(g) 3 C(s) + 3 D(g).!H reaction = -150.0 kj/mol.
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
More informationChapter 10. Acids and Bases
Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.
More informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationAcids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY
Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationAcids & 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
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 informationAdvanced Chemistry Practice Problems
Finding ph 1. Question: Determine the ph for each of the given solutions. a. 0.150 M HNO3 b. 0.150 M CH3COOH, a = 1.8 10-5 c. 0.150 M CHOOH, a = 3.5 10-4 Answer: The method to determine the ph of a solution
More informationChapter 6 Acids and Bases
Chapter 6 Acids and Bases Introduction Brønsted acid-base reactions are proton transfer reactions. Acids donate protons to bases. In the process, the acid is converted into its conjugate base and the base
More informationChemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationChap 16 Chemical Equilibrium HSU FUYIN
Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen
More informationg. Looking at the equation, one can conclude that H 2 O has accepted a proton from HONH 3 HONH 3
Chapter 14 Acids and Bases I. Bronsted Lowry Acids and Bases a. According to Brønsted- Lowry, an acid is a proton donor and a base is a proton acceptor. Therefore, in an acid- base reaction, a proton (H
More informationChapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
More informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
More informationCalorimetry, Heat and ΔH Problems
Calorimetry, Heat and ΔH Problems 1. Calculate the quantity of heat involved when a 70.0g sample of calcium is heated from 22.98 C to 86.72 C. c Ca= 0.653 J/g C q = 2.91 kj 2. Determine the temperature
More informationFormation 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
More informationUnit 4: ACIDS, BASES AND SALTS
ABS - 1 Unit 4: ACIDS, BASES AND SALTS 4.1 Arrhenius Acids and Bases Acids release H + in water Bases release OH - in water Salts are products of an acid-base neutralization reaction. The salt is an ionic
More informationAcid / 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,
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
More informationUnit 9: Acids and Bases Chapter 19
Unit 9: Acids and Bases Chapter 19 I. Introduction In aqueous solutions, the solvent is. Aqueous solutions contain. In the self-ionization of water, the hydrogen ion (H+) exists in solution as the ion.
More informationAP 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
More informationAqueous Equilibria Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry The Common-Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) If
More informationUnit Nine Notes N C U9
Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release
More informationChapter 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
More informationReally useful information = H + = K w. K b. 1. Calculate the ph of a solution made by pouring 5.0 ml of 0.20 M HCl into 100. ml of water.
Acid Base Equilibrium Putting it all together HA H + + A H + A incomingsa HA +incomingsa Strong Acids HCl HNO3 HBr H2SO4 HI HClO4 HClO3 Really useful information K w H + OH K w M V M V B + H2O OH + HB
More informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY
ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationAcids 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
More informationExample 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates
Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate
More informationChapter 16 Acid Base Equilibria
Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar
More informationCHEM 200/202. Professor Gregory P. Holland Office: GMCS-213C. All s are to be sent to:
CHEM 200/202 Professor Gregory P. Holland Office: GMCS-213C All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 12:00 pm to 2:00 pm or by appointment.
More informationName: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.
Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following
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 14: Acids and Bases
Chapter 14: Acids and Bases 14.1 The Nature of Acids and Bases Bronsted-Lowry Acid-Base Systems Bronsted acid: proton donor Bronsted base: proton acceptor Bronsted acid base reaction: proton transfer from
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationChem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
More informationAP Chemistry: Acids & Bases Notes
AP Chemistry: Acids & Bases Notes Objectives Definition of Acids-Bases Acid Strength Base Strength ph-poh Scale Calculating ph of Strong Acids-Bases Calculating ph of Weak Acids-Bases Calculating Ka from
More informationChapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
More informationACID-BASE EQUILIBRIA. Chapter 16
P a g e 1 Chapter 16 ACID-BASE EQUILIBRIA Nature of Acids and Bases Before we formally define acids and bases, let s examine their properties. Properties of Acids Sour taste Ability to dissolve many metals
More informationCHE 107 Fall 2016 Exam 3
CHE 107 Fall 2016 Exam 3 Your Name: Your ID: Question #: 1 [H3O + ] in a typical solution of hand soap is 3.2 10 10 M. The ph of this solution is 1. Report your answer with two decimal places. Do NOT include
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 informationLecture 20 Chapter 17, Sections 4-5 More weak acids and bases. Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases
Lecture 20 Chapter 17, Sections 4-5 More weak acids and bases Identifying acids and bases Conjugate acids and bases Salts of weak acids and bases Acids and Bases Strong vs. Weak K a vs. K b ph = -log([h])
More informationChem 105 Tuesday March 8, Chapter 17. Acids and Bases
Chem 105 Tuesday March 8, 2011 Chapter 17. Acids and Bases 1) Define Brønsted Acid and Brønsted Base 2) Proton (H + ) transfer reactions: conjugate acid-base pairs 3) Water and other amphiprotic substances
More informationExam Practice. Chapters
Exam Practice Chapters 16.6 17 1 Chapter 16 Chemical Equilibrium Concepts of: Weak bases Percent ionization Relationship between K a and K b Using structure to approximate strength of acids Strength of
More informationEXAM 2 PRACTICE KEY. Leaders: Deborah Course: CHEM 178
Leaders: Deborah Course: CHEM 178 EXAM 2 PRACTICE KEY Instructor: Bonaccorsi/Vela Date: 3/6/18 Make sure you (also) know: Acid-base definitions Arrhenius Bronsted-Lowry Lewis Autoionization process of
More informationChapter 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
More information1. 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
More informationSection 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You
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 informationAcids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh
Honors Chemistry Name Acids and Bases Review Worksheet II Date / / Period Solute Name of Solute Molar Mass grams mole Molarity moles L Normality [H 3 O +1 ] [OH ] ph poh Acidic or Basic 1. HCl Hydrochloric
More informationUnit 7, Lesson 08: The ph of Salt Solutions, Answers
1. Complete the following chart: Unit 7, Lesson 08: The ph of Salt Solutions, Answers on NH 4 PO 3 3- Parent Acid or Base s the parent strong or weak? Will this ion hydrolyze? f the ion will hydrolyze
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationUnit 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
More informationBrønsted-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)
More informationCh 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,
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 informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More informationCHAPTER 14 THE CHEMISTRY OF ACIDS AND BASES
CHAPTER 14 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 informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationCHEMISTRY - BURDGE-ATOMS FIRST 3E CH.17 - ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
!! www.clutchprep.com CONCEPT: CLASSIFICATION AND IDENTIFICATION OF BUFFERS Solutions which contain a acid and its base are called buffer solutions because they resist drastic changes in ph. They resist
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More information