Formation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic
|
|
- Alexandrina Carr
- 5 years ago
- Views:
Transcription
1 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 A solution where NaF(aq) is added to pure water is basic Cations of Weak Bases Consider the weak base CH3NH2 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 1 of 13
2 Determine [HF], [H3O + ], [F ] and ph of a 1.0 M solution of HF. KA of HF is Determine [HF], [H3O + ], [F ] and ph of a 1.0 M solution of NaF. KA of HF is [HF] = 1.0 M [H3O + ] = M [F ] = M ph = 1.57 [HF] = M [H3O + ] = M [F ] = 1.0 M ph = 8.57 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 2 of 13
3 KA and KB for a Conjugate Acid-Base Pair Describe the chemistry of an aqueous ammonium chloride solution Describe the chemistry of an aqueous sodium acetate (CH3COONa) solution Describe the chemistry of an aqueous sodium chloride solution Review Concept Check Benzoic acid, HC7H5O2, has an ionization constant with the value: KA = at 25 o C. Calculate the value of pkb for the conjugate base of benzoic acid. a b c d e We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 3 of 13
4 Sodium acetate (CH3COONa) has applications in photographic development and textile dyeing. What is the ph of 0.25 M sodium acetate? KA of CH3COOH is ph = 9.07 Summary/ Review Cations from strong bases: Group 1A alkali metal cations (Li +, Na +, K +, etc) heavier alkaline earth cations of group 2A (Ca 2+, Sr 2+, Ba 2+, etc) These ions have no acid strength Cations from weak bases: NH3 and its derivatives NH4 +, CH3NH3 +, (CH3)2NH2 +, (CH3)3NH +, etc Hydrated cations of small, highly charged metal cations: Al 3+, Fe 2+, Fe 3+, Cr 3+, Zn 2+ Anions from strong monoprotic acids Cl, Br, I, NO3, ClO3, and ClO4 These ions have no base strength Anions from a weak acid: CN, NO2, F, CH3COO, CO3 2 etc.. These ions have some base strength These ions have some acid strength We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 4 of 13
5 Salts that Yield Neutral Solutions the anion of a strong acid and the cation of a strong base yields a neutral solution Neither ion has any appreciable acid or base strength Salts that Yield Acidic Solutions The cation is the conjugate acid of a weak base and therefore has some acidic strength It will to react with water to yield H3O + ions The anion is the conjugate base of a strong acid and has no strength as a base It has no tendency to react with water Net result is an acidic solution Salts that Yield Basic Solutions The cation is the conjugate acid of a strong base and therefore has no acidic strength It has no tendency to react with water The anion is the conjugate base of a weak acid and has some strength as a base It will to react with water to yield OH ions Predict whether aqueous solutions of the following are acidic, basic, or neutral, and write an equation for the reaction of any ion that reacts with water. Potassium perchlorate, KClO4 Sodium benzoate, C6H5COONa neutral Salts of Weakly Acidic Cations and Weakly Basic Anions If a salt solution consists of the anion of a weak acid and the cation of a weak base, the ph of the solution will depend on the relative acid strength or base strength of the ions Compare the relative values of KA and KB of the ions If KA > KB, the solution will be acidic (phsoln < 7) If KA < KB, the solution will be basic (phsoln > 7) If KA for the cation and KB for the anion are comparable, the solution will contain approximately equal concentrations of H3O + and OH ions (phsoln 7) basic We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 5 of 13
6 Concept Check If aqueous solutions of the following soluble ionic compounds are formed, the ph of each solution is LiCl CH3NH3Br Na3PO4 a. acidic basic neutral b. basic neutral acidic c. Neutral basic acidic d. Neutral acidic basic AlCl3 is an acidic salt since Al 3+ (aq) froms a complex that acts as an acid in solution. Calculate the ph of a 0.10 M AlCl3; solution. Hint: KA of Al(H2O)6 3+ = The Leveling Effect HClO4 is a stronger than HClO3, but there is no difference between them when dissolved in water due to water s leveling effect All strong acids and bases are equally strong in water Practice Problems ph=2.93 Predict whether the following salt solutions are neutral, acidic, or basic, and calculate the ph of each. Hint: Write the equation for dissociation of the salt and any equilibrium established M NH4Br; KB of NH3 = ph=4.93 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 6 of 13
7 0.10 M NaCN; KA of HCN = M NaNO2; KA of HNO2 = ph=11.16 ph= 8.32 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 7 of 13
8 Buffers: Acid-Base Equilibria An acid-base buffer is a solution that lessens the impact of ph from the addition of acid or base A 100-mL sample of dilute HCl is adjusted to ph A 100-mL sample of an acetate buffer is adjusted to ph 5.00 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 8 of 13
9 How a Buffer Works A buffer works acts to absorb small amounts of added acid or base Concept Check NaOH is added to buffer solution which is 0.50 M NH3 and 0.50 M NH4Cl. The added NaOH (OH ) reacts with in the buffer and [NH3]. a. NH4 + ; increases b. NH4 + ; decreases c. NH3; increases d. NH3 decreases Relative Concentrations of Buffer Components & The Henderson-Hasselbalch Equation Consider a solution of acetic acid at equilibrium We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 9 of 13
10 Calculate the ph of a solution consisting of 0.50 M CH3COOH and 0.50 M CH3COONa Note: KA of CH3COOH = ph= 4.74 Calculate the ph of the solution resulting when mole of NaOH(s) is added to 1.0 L of a buffer consisting of 0.50M CH3COOH and 0.50M CH3COONa. (Assume the addition caused a negligible change in volume.) ph = 4.78 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 10 of 13
11 Calculate the ph of the solution resulting when mole of HCl(g) is added to 1.0 L of a buffer consisting of 0.50M CH3COOH and 0.50M CH3COONa. (Assume the addition caused a negligible change in volume.) ph = 4.71 Concept Check Which of the following gives a buffer solution when equal volumes of the two solutions are mixed? a M HNO3 and 0.65 M NaNO3 b M HNO2 and 0.65 M NaNO2 c M HCl and 0.65 M NaCl d M HNO2 and 0.65 M HNO3 e M HNO2 and 0.65 M NaF Buffer Capacity measure the ability of a buffer to maintain the ph with addition of an acid or base The greater the concentrations of the buffer components, the more acid or base it can absorb w/ little ph change We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 11 of 13
12 Buffer Range [ HA ] The closer the ratio - [ A ] is to 1, the more effective the buffer If one component is more than 10 times the other, buffering action is poor Choose buffer system so that pka w/in one unit of desired ph Concept Check A buffer consists of 1.2 M N2H4 (Kb = ) and 0.80 M N2H5Cl. What is the ph of this buffer solution? a b c d e Concept Check A buffer solution with a ph of 6.00 is needed in an experiment. Which of the following buffer systems would work best? a. H2PO4 / HPO4 2 KA of H2PO4 is b. NH3 / NH4 + KB of NH3 is c. N2H4 / N2H5 + KB of N2H4 is d. H2CO3 / HCO3 KA of H2CO3 is e. HNO2 / NO2 KA of is HNO2 is A buffer consists of 3.0 M NH3 (KB = ) and 2.0 M NH4Cl. What is the ph of this buffer after the addition of 1.5 moles of HNO3 to 1.0 L of this buffer? (Assume the volume does not change on addition of the HNO3) ph=8.89 We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 12 of 13
13 Which of the following mixture WILL produce a buffer solution if 1.0 liters of each solution is added together? What s in the beaker? Consider the reaction(s) that occur upon mixing a. 1.5 M HNO3 and 0.8 M NaNO3 b. 1.4 M NH3 and 1.8 M HCl c M HF and 0.80 M NaOH d. 1.6 M HC2H3O2 and 1.4 M NaOH e. None of the above D We are what we repeatedly do. Excellence, then, is not an act, but a habit. Aristotle Page 13 of 13
Diprotic Acids Diprotic acids have two ionizable protons that undergo successive ionization.
Diprotic Acids Diprotic acids have two ionizable protons that undergo successive ionization. + H2A + H2O º H3O + + HA [H3O [HA Ka [H2A + 2 HA + H2O º H3O + + A 2 [H3O [A Ka 2 [HA In general, Ka >> Ka 2.
More informationANALYTICAL CHEMISTRY - CLUTCH 1E CH.8 - MONOPROTIC ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ARRHENIUS ACIDS AND BASES The most general definition for acids and bases was developed by Svante Arrhenius near the end of the 19 th century. According to him, the cation
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 informationExam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]=
Chem 101B Study Questions Name: Chapters 14,15,16 Review Tuesday 3/21/2017 Due on Exam Thursday 3/23/2017 (Exam 3 Date) This is a homework assignment. Please show your work for full credit. If you do work
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 information1032_2nd Exam_ (A)
1032_2nd Exam_1040422 (A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Give the equation for a saturated solution in comparing Q with Ksp. A)
More informationLecture #11-Buffers and Titrations The Common Ion Effect
Lecture #11-Buffers and Titrations The Common Ion Effect The Common Ion Effect Shift in position of an equilibrium caused by the addition of an ion taking part in the reaction HA(aq) + H2O(l) A - (aq)
More informationChapter 16 Aqueous Ionic Equilibrium Buffer Solutions
Chapter 16 Aqueous Ionic Equilibrium 16.1-16.2 Buffer Solutions Why? While a weak acid will partially ionize to produce its conjugate base, it will not produce enough conjugate base to be considered a
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 informationAP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS
AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS THE COMMON ION EFFECT The common ion effect occurs when the addition of an ion already present in the system causes the equilibrium to shift away
More informationCHEMISTRY - BROWN 13E CH.16 - ACID-BASE EQUILIBRIA - PART 2.
!! www.clutchprep.com CONCEPT: ph and poh To deal with incredibly small concentration values of [H + ] and [OH - ] we can use the ph scale. Under normal conditions, the ph scale operates within the range
More informationUNIT 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
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 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 informationCHEMISTRY - CLUTCH CH.15 - ACID AND BASE EQUILIBRIUM.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
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 informationACIDS, BASES, AND SALTS
ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none
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 informationK A K B = K W pk A + pk B = 14
Relationship between the ionization constants of an acid and its conjugate base HCN (aq) H 2 O(l) CN (aq) H O (aq) Conjugate couple The product between of an acid and of its conjugate base is : p p 14
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 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 informationAcid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33
Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with
More informationCHEMISTRY - MCQUARRIE 4E CH.21 - BUFFERS & THE TITRATION OF ACIDS & BASES
!! 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 informationChapter 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
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 informationAP Chemistry. CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect Buffered Solutions. Composition and Action of Buffered Solutions
AP Chemistry CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak electrolyte.
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. Essential Practice for success on the exam!
Acids and Bases AP Chemistry Review 1. If 50 ml of 0.025 M NaOH is mixed with 50 ml of 0.05 M HCl, what is the resulting ph of the mixture closest to? A) 1 B) 2 C) 3 D) 4 E) 5 2. What is the ph of a 0.1
More informationPreparation of different buffer solutions
Preparation of different buffer solutions 1 - Buffers: - All biochemical reactions occur under strict conditions of the concentration of hydrogen ion. - Biological life cannot withstand large changes in
More informationProblem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x
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 )? Write out acid dissociation reaction: C 6 H 5 COOH C 6 H 5 COO H Make an ICE chart since this is a weak
More informationPart One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute)
CHAPTER 16: ACID-BASE EQUILIBRIA Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) A. Weak Monoprotic Acids. (Section 16.1) 1. Solution of Acetic Acid: 2. See Table
More informationChemistry 102 Chapter 17 COMMON ION EFFECT
COMMON ION EFFECT Common ion effect is the shift in equilibrium caused by the addition of an ion that takes part in the equilibrium. For example, consider the effect of adding HCl to a solution of acetic
More informationReactions with water do NOT go to completion, so to find ion concentrations, need to know K eq and solve an equilibrium problem!
Strong Acid and Base Solutions Easy to find ion concentrations! 0.1 M HCl = [H 3 O + ] = 0.1 M [OH ] = 1 x 10 13 M 0.1 M NaOH = [OH ] = 0.1 M [H 3 O + ] = 1 x 10 13 M Weak Acid and Base Solutions Reactions
More informationCH3NH2(aq) + H3O + (aq) 3. The reaction of carbon monoxide and diiodine pentoxide is endothermic. The yield could be increased by
1. What is the ph of a 0.020 M HClO4 solution? a. 0.040 b. 1.70 c. 12.30 d. 0.020 Chemistry 116: Exam 2 2. Given that KB of CH3NH2 is 4.2 10 4 at 25 o C, what is the equilibrium constant for the reaction
More informationHonors Chemistry Study Guide for Acids and Bases. NH4 + (aq) + H2O(l) H3O + (aq) + NH3(aq) water. a)hno3. b) NH3
Honors Chemistry Study Guide for Acids and Bases 1. Calculate the ph, poh, and [H3O + ] for a solution that has a [OH - ] = 4.5 x 10-5? 2. An aqueous solution has a ph of 8.85. What are the [H + ], [OH
More informationChapter 15 - Acids and Bases Behavior of Weak Acids and Bases
Chapter 15 - Acids and Bases Behavior of Weak Acids and Bases 6) Calculate [H+] and ph for 1.0 10 8 M HCl. HCl H + + Cl - For a strong acid, [H+] = 1.0 10 8 M, ph = 8.0, BUT THIS DOES NOT MAKE SENSE!!!
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 informationAcid Base Equilibria
Acid Base Equilibria Acid Ionization, also known as acid dissociation, is the process in where an acid reacts with water to produce a hydrogen ion and the conjugate base ion. HC 2 H 3 O 2(aq) H + (aq)
More informationHomework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)
More informationCHEMISTRY - 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 informationChapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
More informationWeak Acids, Weak Bases, and Salts
Weak Acids, Weak Bases, and Salts Introduction: Weak acids and weak bases only dissociate to a small degree (typically less than 5%). Weak acids vary in their tendency to ionize in water. A weak acid that
More informationChem1120pretest2Summeri2015
Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward
More information2017:2 (a) Ammonia, NH3, is a weak base. pka (NH4 + ) = 9.24 Ka (NH4 + ) = (i) Calculate the ph of a mol L 1 NH3 solution.
AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Collated Buffer Questions 2017:2 (a) Ammonia, NH3, is a weak base. pka (NH4 + ) = 9.24 Ka (NH4 + ) = 5.75 10 10 (i) Calculate
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 informationConsider a 1.0 L solution of 0.10 M acetic acid. Acetic acid is a weak acid only a small percent of the weak acid is ionized
Chemistry 12 Acid- Base Equilibrium V Name: Date: Block: 1. Buffers 2. Hydrolysis Buffers An acid- base buffer is a solution that resists changes in ph following the addition of relatively small amounts
More informationChem 112, Fall 05 Exam 3A
Before you begin, make sure that your exam has all 10 pages. There are 32 required problems (3 points each, unless noted otherwise) and two extra credit problems (3 points each). Stay focused on your exam.
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationWeak Acids, Weak Bases, and Salts
Weak Acids, Weak Bases, and Salts Introduction: Weak acids and weak bases only dissociate to a small degree (typically less than 5%). Weak acids vary in their tendency to ionize in water. A weak acid that
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 information*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base.
16.2 Bronsted-Lowry Acids and Bases An acid is a substance that can transfer a proton to another substance. A base is a substance that can accept a proton. A proton is a hydrogen ion, H +. Proton transfer
More informationChapter 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
More informationPart 01 - Assignment: Introduction to Acids &Bases
Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4
More informationApplications of Aqueous Equilibrium Chapter 15. Common Ion Effect & Buffers Sections 1-3
Applications of Aqueous Equilibrium Chapter 15 Common Ion Effect & Buffers Sections 1-3 Solutions of Acids or Bases Containing a Common Ion NaF Na + + F - HF H + + F - What effect does the NaF have on
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 informationLecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
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
More informationExam 2 Practice (Chapter 15-17)
Exam 2 Practice (Chapter 15-17) 28. The equilibrium constant Kp for reaction (1) has a value of 0.112. What is the value of the equilibrium constant for reaction (2)? (1) SO2 (g) + 1/2 O2(g) SO3 (g) Kp
More informationLast week, we discussed the Brønsted Lowry concept of acids and bases. According to this model:
Last week, we discussed the Brønsted Lowry concept of acids and bases This model is not limited to aqueous solutions; it can be extended to reactions in the gas phase! According to this model: Acids are
More informationMultiple Choice Neatly write your choice in the blank provided. (3 pts each)
Name CH302H EXAM 2 Spring 2013 Multiple Choice Neatly write your choice in the blank provided. (3 pts each) 1. What is the effect of a volume decrease on the reaction: C(s) H2O(g) CO(g) H2(g)? (a) K increases
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 informationCHEMISTRY - BROWN 14E CH.16 - ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
More informationBuffer Effectiveness, Titrations & ph curves. Section
Buffer Effectiveness, Titrations & ph curves Section 16.3-16.4 Buffer effectiveness Buffer effectiveness refers to the ability of a buffer to resist ph change Effective buffers only neutralize small to
More informationChapter 16 Acid-Base Equilibria
Page 1 of 20 Chapter 16 Acid-Base Equilibria 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 o acids
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 informationAS Demonstrate understanding of equilibrium principles in aqueous systems. Collated Buffer Questions
2016: AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems No separate buffer question asked. 2015: 3 Collated Buffer Questions 20.0 ml of 0.258 mol L 1 hydrofluoric acid, HF,
More informationProblems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.
Problems -- Chapter 1 1. Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. (a) NaNO and HNO answers: see end of problem set (b)
More informationChem. 1A Final. Name. Student Number
Chem. 1A Final Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units. Calculators are allowed. Cell phones may not be used for calculators.
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 informationChapter 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
More informationKotz 7 th ed. Section 18.3, pp
Lecture 15 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added
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 14 Acid- Base Equilibria Study Guide
Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and
More informationPractice test Chapters 15 and 16: Acids and Bases
Name: Class: Date: Practice test Chapters 15 and 16: Acids and Bases 1. Which of the following pairs of species is not a conjugate acid base pair? A) HOCl, OCl B) HNO 2, NO + 2 C) O 2, OH D) HSO 4, SO
More informationLe Chatlier's principle can be used to decide whether the above equilibrium will be shifted left or right
Problems, Chapter 17 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) In which of these solutions will HNO2 ionize less than it does in pure water? a) 0.10 M NaCl b)
More informationPreparation Of Different Buffer Solutions. BCH 312 [Practical]
Preparation Of Different Buffer Solutions BCH 312 [Practical] Introduction: All biochemical reactions occur under strict conditions of the concentration of hydrogen ion. Biological life cannot withstand
More informationChapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Often, there are many equilibria going on in an aqueous solution. So, we must determine the dominant equilibrium (i.e. the equilibrium reaction
More informationCHEMISTRY 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
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 informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
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 informationLe Chatlier's principle can be used to decide whether the above equilibrium will be shifted left or right
Problems, Chapter 17 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) In which of these solutions will HNO2 ionize less than it does in pure water? a) 0.10 M NaCl b)
More informationGuide to Chapter 15. Aqueous Equilibria: Acids and Bases. Review Chapter 4, Section 2 on how ionic substances dissociate in water.
Guide to Chapter 15. Aqueous Equilibria: Acids and Bases We will spend five lecture days on this chapter. During the first two class meetings we will introduce acids and bases and some of the theories
More informationStrong and Weak. Acids and Bases
Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF
More informationChapter 15. Acid-Base Equilibria
Chapter 15 Acid-Base Equilibria The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion already involved in the equilibrium
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 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 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 informationLecture 12. Acid/base reactions. Equilibria in aqueous solutions.
Lecture 12 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added
More informationAnalytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS
Analytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS Buffer solutions Definition Solutions which resist changes in ph when small quantities of acid or alkali are added. a solution that
More informationChem 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
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria
Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:
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 informationCHEMISTRY. Chapter 16 Acid-Base Equilibria
CHEMISTRY The Central Science 8 th Edition Chapter 16 Acid-Base Equilibria Kozet YAPSAKLI Why study acids bases? bases are common in the everyday world as well as in the lab. Some common acidic products
More informationBuffers. How can a solution neutralize both acids and bases? Beaker B: 100 ml of 1.00 M HCl. HCl (aq) + H 2 O H 3 O 1+ (aq) + Cl 1 (aq)
Buffers How can a solution neutralize both acids and bases? Why? Buffer solutions are a mixture of substances that have a fairly constant ph regardless of addition of acid or base. They are used in medicine,
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 informationCHM 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
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
More informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
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 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 information