Chapter 19: Acids And Bases Homework Packet (50 Pts)
Chapter 19: Acids and BasesHomework Packet (50 pts)TopicpgSection 19.1Section 19.2Section 19.3Section 19.4Naming AcidsProperties of Acids/BasesConjugate Acid/Base PairsIon Product ConstantCalculating pH and pOHAcid and Base DissociationStrong and Weak ets are due the day of the test, but i will check throughout the unit to see if you are keepingup with the work. I will grade the packets based on effort, completeness and correctness(weighing more towards the 1st two criteria). You must show your work to receive full credit.Name:Score:/ 50
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 209Name19DateClassACIDS, BASES, AND SALTSSECTION 19.1 ACID–BASE THEORIES (pages 587–593)This section compares and contrasts acids and bases as defined by the theoriesof Arrhenius, Brønsted-Lowry, and Lewis. It also identifies conjugate acid–basepairs in acid–base reactions.Properties of Acids and Bases (pages 587–588)1. Circle the letters of all the terms that complete the sentence correctly.The properties of acids include .a. reacting with metals to produce oxygenb. giving foods a sour tastec. forming solutions that conduct electricityd. causing indicators to change colorwater2. Bases are compounds that react with acids to formsaltand a(n). Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.3. Circle the letters of all the terms that complete the sentence correctly.The properties of bases include .a. tasting bitterb. feeling slipperyc. changing the color of an indicatord. always acting as a strong electrolyteArrhenius Acids and Bases (pages 588–590)4. Match the number of ionizable hydrogens with the type of acid.conea. diproticatwob. triproticbthreec. monoprotic5. Is the following sentence true or false? Only the hydrogens in weak polarfalsebonds are ionizable.electronegative6. Hydrogen is joined to a veryelement in a very polarbond.basic7. Alkali metals react with water to producesolutions.Chapter 19 Acids, Bases, and Salts 209
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 210NameDateClassCHAPTER 19, Acids, Bases, and Salts (continued)8. How do concentrated basic solutions differ from other basic solutions?They are extremely caustic.Brønsted-Lowry Acids and Bases (pages 590–592)9. How does the Brønsted-Lowry theory define acids and bases?The Brønsted-Lowry theory defines an acid as a hydrogen-ion donor and a baseas a hydrogen-ion acceptor.10. Is the following sentence true or false? Some of the acids and bases included inthe Arrhenius theory are not acids and bases according to the Brønsted-Lowryfalsetheory.11. Is the following sentence true or false? A conjugate acid is the particle formedtruewhen a base gains a hydrogen ion.base12. A conjugateis the particle that remains when an acidhas donated a hydrogen ion.A conjugate acid–base pair consists of two13. What is a conjugate acid–base pair?substances related by the loss or gain of a single hydrogen ion.14. A substance that can act as both an acid and a base is said to beamphoteric.Water is a base because it accepts a proton.Lewis Acids and Bases (pages 592–593)A Lewis acid is a substance that can accept a pair of16. What is a Lewis acid?electrons to form a covalent bond.donate17. A Lewis base is a substance that cana pair ofelectrons to form a covalent bond.210 Guided Reading and Study Workbook Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.15. In a reaction with HCl, is water an acid or a base?
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 211NameDateClass18. Is the following sentence true or false? All the acids and bases included in theBrønsted-Lowry theory are also acids and bases according to the Lewis theory.true19. Complete this table of acid-base definitions.Acid–Base DefinitionsTypeAcidBaseBrønsted-LowryH donorH acceptorLewiselectron-pair acceptorelectron-pair donorArrheniusH producerOH– producerSECTION 19.2 HYDROGEN IONS AND ACIDITY (pages 594–604)This section classifies solutions as neutral, acidic, or basic, given the hydrogenion or hydroxide-ion concentration. It explains how to convert hydrogen-ionconcentrations into pH values and hydroxide-ion concentrations into pOHvalues.Hydrogen Ions from Water (pages 594-595) Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.1. What does a water molecule that loses a hydrogen ion become?It becomes a negatively charged hydroxide ion (OH–).2. What does a water molecule that gains a hydrogen ion become?It becomes a positively charged hydronium ion (H3O ).3. The reaction in which water molecules produce ions is called theself-ionizationof water.hydrogen ions (H )4. In water or aqueous solution,are always joined towater moleculesas hydronium ions (H O ). 35. Is the following sentence true or false? Any aqueous solution in which [H ] andtrue[OH–] are equal is described as a neutral solution.Ion Product Constant for Water (pages 595–596)6. What is the ion-product constant for water (Kw)? Give the definition, theThe ion-product constant for water is the product of theexpression, and the value.concentrations of the hydrogen ions and hydroxide ions in water.K w [H ] [OH– ] 1.0 10 –14Chapter 19 Acids, Bases, and Salts 211
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 212NameDateClassCHAPTER 19, Acids, Bases, and Salts (continued)acidic7. A(n)solution is one in which [H ] is greater than [OH–].basicA(n)solution is one in which [H ] is less than [OH–].8. Match the type of solution with its hydrogen-ion concentration.bacidica. less than 1.0 10–7 Mcneutralb. greater than 1.0 10–7 Mabasicc. 1.0 10–7 MThe pH Concept (pages 596–600)pH of a solution is the negative logarithm of the hydrogen-ion9. Theconcentration.10. Match the type of solution with its pH.cacidica. pH 7.0bneutralb. pH 7.0abasicc. pH 7.011. Look at Table 19.5 on page 598. What is the approximate [H ], the [OH–], and the1 10–12 mol/L, 1 10–2 mol/L, and 12.0pH of washing soda?12. The pOH of a solution is the negative logarithm of thehydroxide-ionconcentration.14. For pH calculations, in what form should you express the hydrogen-ionYou should express the hydrogen-ion concentration in scientific notation.concentration?15. Look at the pH scale below. Label where you would find acids, bases, andneutral 0 0 10 1 10 2 10 3 10 4 10 5 10 6 10 7 10 8 10 9 10 10 10 11 10 12 10 13 10 14212 Guided Reading and Study Workbook Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.713. What is the pOH of a neutral solution?
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 213NameDateClass16. Is the following sentence true or false? Most pH values are whole numbers.false17. If [H ] is written in scientific notation but its coefficient is not 1, what do you need toneed either a table of common logarithms or a calculatorcalculate pH? Youwith a log function key.18. Is the following sentence true or false? You can calculate the hydrogen-iontrueconcentration of a solution if you know the pH.Measuring pH (pages 600–603)19. When do you use indicators and when do you use a pH meter to measure pH?You use indicators for preliminary measurements and for small-volume samples. Youuse a pH meter for precise and continuous measurements.20. Why is an indicator a valuable tool for measuring pH?It is a valuable tool for measuring pH because its acid form and base form havedifferent colors in solution.21. Why do you need many different indicators to span the entire pH spectrum?For each indicator, the change from dominating acid form to dominating base form Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.occurs in a narrow range of approximately two pH units.22. Look at the figure below. Fill in the missing pH color change ranges for theindicators.Bromphenol blueBromcresol greenPhenol redPhenolphthalein01234567891011121314pH23. List three characteristics that limit the usefulness of indicators.a. At temperatures other than 25 C, an indicator may change color at a different pH.b. Indicator color can be distorted if a solution is not colorless.c. Dissolved salts in a solution can affect the dissociation of the indicator.Chapter 19 Acids, Bases, and Salts 213
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 214NameDateClassCHAPTER 19, Acids, Bases, and Salts (continued)24. How accurate are measurements of pH obtained with a pH meter?to within 0.01 pH unit of the true pH25. What is the pH of each of the following solutions?7a. water3b. vinegar10.5c. milk of magnesia26. Is the following sentence true or false? Measurements of pH obtained with apH meter are typically accurate to within 0.001 pH unit of the true pH.falseSECTION 19.3 STRENGTHS OF ACIDS AND BASES (pages 605–611)This section defines strong acids and weak acids, and then explains how tocalculate an acid dissociation constant. It describes how acids and bases arearranged by strength according to their dissociation constants (Ka) and (Kb).Strong and Weak Acids and Bases (pages 605–609)1. What factor is used to classify acids as strong or weak?Acids are classified by the degree to which they ionize in water.only slightlyacids ionizein aqueous solution.3. Look at Table 19.6 on page 605. Which acid is the weakest acid in the table?Which base is the weakest base?Hypochlorous acid is the weakest acid. Ammonia is the weakest base.4. What do you use to write the equilibrium-constant expression?You use a balanced chemical equation.5. An acid dissociation constant (Ka) is the ratio of the concentration of thedissociatedform of an acid to the concentration of theundissociatedform.6. What is another name for dissociation constants?Another name is ionization constants.7. Is the following sentence true or false? The stronger an acid is, the smaller itsfalseKa value.two8. A diprotic acid hasdissociation constants.214 Guided Reading and Study Workbook Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.completely2. Strong acids areionized in aqueous solution; weak
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 215NameDateClass9. Look at Table 19.7 on page 607. What is the second dissociation constant for theKa 6.2 10–8triprotic phosphoric acid?10. Weak bases react with water to form the hydroxide ion and theconjugate acidof the base.11. A base dissociation constant (Kb) is the ratio of the concentration of theconjugate acidtimes the concentration of the hydroxideconjugate baseion to the concentration of the.12. What does the magnitude of the base dissociation constant (Kb) indicate?It indicates the ability of a weak base to compete with the very strong base OH – forhydrogen ions.13. The words concentrated and dilute indicate how much acid or base isdissolvedin solution.14. Is the following sentence true or false? The words strong or weak refer to thetrueextent of ionization or dissociation of an acid or base.Calculating Dissociation Constants (pages 609–610)15. Is the following sentence true or false? You can calculate the acid dissociationtrueconstant (Ka) of a weak acid from experimental data.16. To measure the equilibrium concentrations of all substances present atequilibrium for a weak acid, what two conditions must you know?You must know the initial molar concentration of the acid and the pH (or [H3O ]) ofthe solution at equilibrium.
05 Chem GRSW Ch19.SE/TE 6/11/04 3:50 PM Page 216NameDateClassCHAPTER 19, Acids, Bases, and Salts (continued)SECTION 19.4 NEUTRALIZATION REACTIONS (pages 612–616)This section explains how acid–base titration is used to calculate theconcentration of an acid or a base. It also explains the concept ofequivalence in neutralization reactions.Acid–Base Reactions (pages 612–613)1. Is the following sentence true or false? Acids react with compounds containingtruehydroxide ions to form water and a salt.2. What does the reaction of an acid with a base produce?It produces water and a salt.3. In general, reactions in which an acid and a base react in an aqueous solutionneutralizationto produce a salt and water are calledreactions.4. Look at Table 19.9 on page 613. Circle the letter of the salt that is used forphotographic emulsions.a. calcium chloridec. silver bromideb. potassium chlorided. sodium chlorideanion5. Salts are compounds consisting of a(n)from an acidcationand a(n)from a base.6. How can you determine the concentration of an acid or base in a solution?You can perform a neutralization reaction.7. Complete the flow chart below showing the steps of a neutralization reaction.unknownA measured volume of an acid solution ofconcentration is added to a flask.indicatorSeveral drops of theare added to the solutionwhile the flask is gently swirled.knownMeasured volumes of a base ofconcentration arecolormixed into the acid until the indicator changes.216 Guided Reading and Study Workbook Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.Titration (pages 613–616)
Naming AcidsNameChem Worksheet 19-0Acids are compounds that can donate the hydrogen ion, H . When the formula for an acid is writtenthe symbol for this hydrogen generally appears at the beginning of the formula. For example the formulafor hydrochloric acid is written HCl and the formula for phosphoric acid is H3PO4. Notice that bothformulas begin with the letter H. In both cases the acid is made of a hydrogen ion (or hydrogen ions) and anegative ion, known as the anion.The name for an acid is based on the name of the anion. If the anion ends with the letters –ide, theacid is named one way while acids containing anions that end with –ate use a different rule. Rememberthat monatomic anions typically end with –ide. The rules for naming acids are summarized below.Naming AcidsAnion called (root)Example: sulfide, S2-ideAcid called hydro (root) ic acidExample: hydrosulfuric acid, H2SAnion called (root) ateExample: chlorate , ClO3–Anion called (root) iteExample: chlorite , ClO2–Acid called (root) ic acidExample: chloric acid, HClO3Acid called (root) ous acidExample: chlorous acid, HClO2Examples#1.#2.Write the chemical formula for: sulfurous acid.- this acid contains the hydrogen ion and the sulfite ion:H - create a neutral compound from these ions:H1 SO32SO32-H2SO3Name the following acid: H2CO3.- this acid contains the hydrogen ion and the carbonate ion:H CO32-- the name of the negative ion is carbonate, therefore the acid is called carbonic acid.Fill in the following table with the missing .FormulaHClHNO3H2SO4H2SO3CationH H H H H H2C2O4HFormula for anionCl–F–SO42ClO3–I–HClO John Erickson, 2005AsO43–Name of teName of Acidhydrofluoric acidchloric acidhydrocyanic acidacetic acidsulfidearsenatenitrous acidWS19-0NamingAcids
Name Date PeriodAcid/Base Homework #11. An aqueous solution tastes bitter and turns litmus blue. Is the solution acidic or basic?2. An acidic solution reacts with magnesium carbonate to produce a gas. What is the formulaof the gas?3. How did Arrhenius describe acids and bases? Why was his description important?4. Classify each of the following compounds as an Arrhenius acid or an Arrhenius base.a. H2Sb. RbOHc. Mg(OH)2d. H3PO45. Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Givean example of each.6. Ammonia contains three hydrogen atoms per molecule. However, an aqueous ammoniasolution is basic. Explain using the Bronsted-Lowry model of acids and bases.7. Identify the conjugate acid-base pairs in the equilibrium equation.HC2H3O2 H2O H3O C2H3O2-
8. Gaseous HCl molecules interact with gaseous NH3 moleucles to form a white smoke made upof solid NH4Cl particles. Explain whether or not this is an acid-base reaction according toboth the Arrhenius model and the Bronsted-Lowry model.9. Write a balanced formula equation for the reaction between sulfuric acid and calcium metal.10. Write a balanced formula equation for the reaction between potassium hydrogen carbonateand chlorous acid (HClO2).11. Write the balanced chemical equation for the ionization of perchloric acid (HClO 4) in water.12. Write the balanced chemical equation for the dissociation of solid magnesium hydroxide inwater.
Conjugate Acid Base PairsNameChem Worksheet 19-2An acid is defined as a proton (H ) donor while a base is a protonacceptor. The substance that is produced after an acid has donated itsproton is called the conjugate base while the substance formed when abase accepts a proton is called the conjugate acid. The conjugate acidcan donate a proton to the conjugate base, to reform the originalreactants in the reverse reaction.HF H2OacidbaseAcids donate protonsBases accept protonsA proton is a hydrogen ionH3O F–c. acidc. baseIn the reaction above HF is the acid and H2O is the base. The HF has given a proton to the H2O,forming H3O and F–. Since the product H3O can donate a proton back to F– it is labeled the conjugateacid, while the F– is the conjugate base.ExampleWrite an equation that shows NH3 reacting with HCl. Label the acid, base, and conjugate acid and conjugate base.H - Write reactants and transfer a proton from the acid to the base:NH4 Cl–NH3 HClbaseacidc. acidc. baseRewrite each equation. Identify the acid, the base, the conjugate acid, and the conjugatebase in each of the equations.1. HCl NH32. OH– HCN3. PO43– HNO34. HCO3– HClNH4 Cl–5. HCO3– OH–H2O CN–6. NH4 H2ONO3– HPO42–NH3 H3O 7. C2O42– HC2H3O28. HPO42– H2OH2CO3 Cl–H2O CO32–HC2O4– C2H3O2–OH– H2PO4–Fill in the following table.AcidBase9HNO2H2O10H2OF–Conjugate AcidHFConjugate Base13H2OHSO4–NO2– H3O NH3 HCNNH4 CN–ClO3–PO43–S2– H2O1415HNO2 H2OOH–1112EquationHCO2HOH-OH– HS–
Ion Product Constant Practice Questions1. What is the hydroxide ion concentration with a hydroniumconcentration of 6.80 x 10-10 mol/L?2. What is the [H3O ] in a solution with [OH-] of 5.67 x 10-3mol/L?3. If the [H3O ] in a nitric acid solution is 0.0020 mol/L, what isthe [OH-]?4. If the [OH-] in a sodium hydroxide solution is 0.050 mol/L,what is [H3O ]?
Name: Date: Period:Calculating pH, [H ], [OH-]Show work when needed.1. What is the pH of a solution that has a H concentration of 1.00 x 10-2 M? Is this solutionacidic or basic?2. What is the concentration of hydrogen ions in a solution having a pH of 7.50? Is thissolution acidic or basic?3. What is the concentration of H ions in a solution having a pH of 9.609?4. What is the concentration of H ion in a solution having a pH of 3.857? Is the solutionacidic or basic?5. Find the pH of a solution in which [H ] 1.39 x 10-4 M.6. A solution has a pH reading of 0.61. What is the hydrogen ion concentration of thesolution?
7. The pH of rainwater is 6.2 and the pH of tomato juice is 4.2. Compare the relativenumber of hydronium ions in rainwater and tomato juice.89Find the pH of a solution in which [OH-] 2.6 x 10-7 MWhat is the concentration of OH- ions in a solution with a pH of 4.38? Is the solutionacidic or basic?10. The pOH of a solution is 5.67. What is the [OH-] of the solution?11. The pOH of a solution is 11.28. What is the [H ] of the solution?
Name Date PeriodAcid & Base Ionization Constants1. The Ka of benzoic acid (HC7H5O2) is 6.6 x 10-5.a. Write the equation for the ionization of benzoic acid in water.b. Write the equilibrium constant expression for the reaction.c. Calculate the concentration of H3O in 0.10 M benzoic acid solution.2. A 0.10 M HC6H5O2 solution has a pH of 2.59. What’s the Ka?3. Find the concentration of hydroxide ion in a 0.15 M ammonia solution. Forammonia, Kb 1.8 x 10-5.
Strong & Weak Aci
Chapter 19 Acids, Bases, and Salts209 SECTION 19.1 ACID–BASE THEORIES(pages 587–593) This section compares and contrasts acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis. It also identifies conjugate acid–base pairs in acid–base reactions. Properties of Acids and Bases (pages 587–588) 1.
2. Describe the common properties of acids and bases 3. Identify acids and bases using indicators, pH papers 4. Name some common lab acids and bases, acids at and bases at home 5. Describe reactions of acids with metals, bases and carbonates 6. Describe the application of acids, bases and p
_7. Which statement describes an alternate theory of acids and bases? (1) Acids and bases are both H acceptors. (2) Acids and bases are both H donors. (3) Acids are H acceptors, and bases are H donors. (4) Acids are H donors, and bases are H acceptors. _8. Which substance is the
Properties of Acids and Bases Return to the Table of contents Slide 5 / 208 What is an Acid? Acids release hydrogen ions into solutions Acids neutralize bases in a neutralization reaction. Acids corrode active metals. Acids turn blue litmus to red. Acids taste sour. Properties of Acids Slide 6 / 208 Properties
Lecture Notes for Chapter 16: Acids and Bases I. Acids and Bases a. There are several ways to define acids and bases. Perhaps the easiest way to start is to list some of the properties of acids and bases. b. The table below summarizes some properties that will be helpful
Acids, Bases, and pH The hydrohalic acids (HX (aq)), where X represents a halogen) include HF, HCl, HBr, and HI. Only HF is a weak acid. The rest are strong acids. What factors account for this difference? 8.1 Explaining the Properties of Acids and Bases 8.2 The Equilibrium of Weak Acids and Bases 8.3
properties of acids and bases. 5. Describe the colors that form in acidic and basic solutions with litmus paper and phenolphthalein. 6. Explain the difference between strong acids or bases and weak acids or bases. 7. Memorize the strong acids and bases. 8. Define the terms polyprotic and amphiprotic. 9. Perform calculations using the following .
Unit 12 Acids and Bases- Funsheets Part A: Name and write the formula for the following acids and bases. 1) Carbonic acid _ . Part E: Using your knowledge of acids and bases, answer the following questions. 1) Fill in the following Venn diagram about properties of acids and bases. You must fill in at least 4 facts in each.
Unit 11 Objectives: Acids & Bases Acid-Base Nomenclature Content Objectives: I can name ionic compounds containing acids, and bases, using (IUPAC) nomenclature rules. I can write the chemical formulas of acids and bases. Criteria for Success: I can identify an acid as a binary acid or an oxyacid. I can name common binary acids, oxyacids, and bases given their chemical formula.
