SeCtION 1 Properties Of Acids And Bases
Section 1Properties of Acidsand BasesMain IdeasAcids are identified by theirproperties.Some acids are useful inindustry.Key Termsbinary acidoxyacidArrhenius acidArrhenius baseThe properties of bases differfrom those of acids.strong acidweak acidHow many foods can you think of that are sour? Chances are that almost all thefoods you thought of, like those in Figure 1.1a, owe their sour taste to an acid.Sour milk contains lactic acid. Vinegar, which can be produced by fermentingjuices, contains acetic acid. Phosphoric acid gives a tart flavor to many carbonatedbeverages. Most fruits contain some kind of acid. Lemons, oranges, grapefruits,and other citrus fruits contain citric acid. Apples contain malic acid, and grape juice contains tartaric acid.Many substances known as bases are commonly found in household products,such as those in Figure 1.1b. Household ammonia is an ammonia-water solutionthat is useful for all types of general cleaning. Sodium hydroxide, Na OH, known bythe common name lye, is present in some commercial cleaners. Milk of magnesiais a suspension in water of magnesium hydroxide, Mg(OH)2, which is not verywater-soluble. It is used as an antacid to relieve discomfort caused by excesshydrochloric acid in the stomach. Aluminum hydroxide, Al (OH)3, and sodiumhydrogen carbonate, NaHCO3, are also bases commonly found in antacids.Arrhenius acids and basesproduce ions in solution. Figure 1.1Common Acids and BasesBenzoic acid, HC7H5O2Sorbic acid, HC6H7O2Phosphoric acid, H3PO4Carbonic acid, H2CO3NH3(aq)Citric acid,H3C6H5O7Ascorbic acid,H2C6H6O6NaOHNaHCO3Al(OH)3(a) Fruits and fruit juices contain acids suchas citric acid and ascorbic acid.Carbonated beverages contain benzoicacid, phosphoric acid, and carbonic acid.(b) Many household cleaners containbases such as ammonia and sodiumhydroxide. Antacids contain basessuch as aluminum hydroxide.Acids and Bases441
Figure 1.2Acid Indicator A strip of pHpaper dipped into vinegar turns red,showing that vinegar is an acid.Main IdeaAcids are identified by their properties.Acids were first recognized as a distinct class of compounds because ofthe common properties of their aqueous solutions. These properties arelisted below.1. A queous solutions of acids have a sour taste. Taste, however, shouldNEVER be used as a test to evaluate any chemical substance. Manyacids, especially in concentrated solutions, are corrosive; that is, theydestroy body tissue and clothing. Many are also poisons.2. A cids change the color of acid-base indicators. When pH paperis used as an indicator, the paper turns certain colors in acidic solution. This reaction is demonstrated in Figure 1.2.3. S ome acids react with active metals and release hydrogen gas, H2.Recall that metals can be ordered in terms of an activity series. Metalsabove hydrogen in the series undergo single-displacement reactionswith certain acids. Hydrogen gas is formed as a product, as shown bythe reaction of barium with sulfuric acid.Ba(s) H2SO4(aq) BaSO4(s) H2(g)4. A cids react with bases to produce salts and water. When chemicallyequivalent amounts of acids and bases react, the three properties justdescribed disappear because the acid is “neutralized.” The reactionproducts are water and an ionic compound called a salt.5. A cids conduct electric current. Some acids completely separate intoions in water and are strong electrolytes. Other acids are weakelectrolytes.Acid NomenclatureA binary acid is an acid that contains only two different elements: hydrogen andone of the more electronegative elements. Many common inorganic acidsare binary acids. The hydrogen halides—HF, HCl, HBr, and HI—are allbinary acids. Names for some binary acids are given in Figure 1.3.Figure 1.3Names of Binary Acids442Chapter 14FormulaAcid nameMolecule nameHFhydrofluoric acidhydrogen fluorideHClhydrochloric acidhydrogen chlorideHBrhydrobromic acidhydrogen bromideHIhydriodic acidhydrogen iodideH2Shydrosulfuric acidhydrogen sulfide
In pure form, each compound listed in the table is a gas. Aqueous solutions of these compounds are known by the acid names. Specific rules fornaming binary compounds are listed below.Binary Acid Nomenclature1. The name of a binary acid begins with the prefix hydro-.2. The root of the name of the second element follows this prefix.3. The name then ends with the suffix -ic.An oxyacid is an acid that is a compound of hydrogen, oxygen, and a thirdelement, usually a nonmetal. Nitric acid, HNO3, is an oxyacid. The structuresof two other oxyacids are shown in Figure 1.4. Oxyacids are one class ofternary acids, which are acids that contain three different elements.Usually, the elements in an oxyacid formula are written as one or morehydrogen atoms followed by a polyatomic anion. But as you can see fromthe structures, the H atoms are bonded to O atoms. The names of oxyacidsfollow a pattern, and the names of their anions are based on the names ofthe acids. Some common oxyacids and their anions are given inFigure 1.5. Many of these names should be familiar to you.Figure 1.4Oxyacid Structure Althoughthe chemical formula shows hydrogenatoms and a polyatomic ion, noticethat the hydrogens are bonded to theoxygen in an oxyacid.H. O : . . . : . . H : OP. . : O. . : . . : H: O : .(a) Structure of H3PO4.: O. . : . . . . . : HH : O. . : .S. :O: O :.Figure 1.5Names of Common Oxyacids and OxyanionsFormulaAcid nameAnionCH3COOHacetic acidCH3COO-, acetateH2CO3carbonic acid C O 23 , carbonateHClOhypochlorous acidClO -, hypochloriteHClO2chlorous acid ClO 2 , chloriteHClO3chloric acid ClO 3 , chlorateHClO4perchloric acid ClO 4 , perchlorateHIO3iodic acid IO 3 , iodateHNO2nitrous acid NO 2 , nitriteHNO3nitric acid NO 3 , nitrateH3PO3phosphorous acid PO 33 , phosphiteH3PO4phosphoric acid PO 34 , phosphateH2SO3sulfurous acid SO 23 , sulfiteH2SO4sulfuric acid SO 24 , sulfate(b) Structure of H2SO4---Acids and Bases443
Main IdeaSome acids are useful in industry.The properties of acids make them important chemicals both in thelaboratory and in industry. Sulfuric acid, nitric acid, phosphoric acid,hydrochloric acid, and acetic acid are all common industrial acids.Sulfuric AcidSulfuric acid is the most commonly produced industrial chemical in theworld. More than 37 million metric tons of it are made each year in theUnited States alone. Sulfuric acid is used in large quantities in petroleumrefining and metallurgy as well as in the manufacture of fertilizer. It is alsoessential to a vast number of industrial processes, including the production of metals, paper, paint, dyes, detergents, and many chemical rawmaterials. Sulfuric acid is the acid used in automobile batteries.Because it attracts water, concentrated sulfuric acid is an effectivedehydrating (water-removing) agent. It can be used to remove water fromgases with which it does not react. Sugar and certain other organiccompounds are also dehydrated by sulfuric acid. Skin contains organiccompounds that are attacked by concentrated sulfuric acid, which cancause serious burns.Nitric AcidPure nitric acid is a volatile, unstable liquid. Dissolving the acid in watermakes the acid more stable. Solutions of nitric acid are widely used inindustry. Nitric acid also stains proteins yellow. The feather in Figure 1.6was stained by nitric acid. The acid has a suffocating odor, stains skin,and can cause serious burns. It is used in making explosives, many ofwhich are nitrogen- containing compounds. It is also used to makerubber, plastics, dyes, and pharmaceuticals. Initially, nitric acid solutionsare colorless; however, upon standing, they gradually become yellowbecause of slight decomposition to brown nitrogen dioxide gas.Figure 1.6Nitric Acid and ProteinsConcentrated nitric acid stains afeather yellow.444Chapter 14
Phosphoric AcidPhosphorus, along with nitrogen and potassium, is an essential elementfor plants and animals. The bulk of phosphoric acid produced each yearis used directly for manufacturing fertilizers and animal feed. Dilutephosphoric acid has a pleasant but sour taste and is not toxic. It is used asa flavoring agent in beverages and as a cleaning agent for dairy equipment. Phosphoric acid is also important in the manufacture of detergentsand ceramics.Hydrochloric AcidThe stomach produces HCl to aid in digestion. Industrially, hydro chloricacid is important for “pickling” iron and steel. Pickling is the immersionof metals in acid solutions to remove surface impurities. This acid is alsoused in industry as a general cleaning agent, in food processing, in theactivation of oil wells, in the recovery of magnesium from sea water, andin the production of other chemicals.Concentrated solutions of hydrochloric acid, commonly referred to asmuriatic acid, can be found in hardware stores. It is used to maintain thecorrect acidity in swimming pools and to clean masonry.Acetic AcidPure acetic acid is a clear, colorless, and pungent-smelling liquid knownas glacial acetic acid. This name is derived from the fact that pure aceticacid has a freezing point of 17 C. It can form crystals in a cold room. Thefermentation of certain plants produces vinegars containing acetic acid.White vinegar contains 4% to 8% acetic acid.Acetic acid is important industrially in synthesizing chemicals used inthe manufacture of plastics. It is a raw material in the production of foodsupplements—for example, lysine, an essential amino acid. Acetic acid isalso used as a fungicide.Main IdeaThe properties of bases differ from those of acids.Figure 1.7Base Indicator pH paper turnsblue in the presence of this solutionof sodium hydroxide.How do bases differ from acids? You can answer this question by comparing the following properties of bases with those of acids.1. Aqueous solutions of bases taste bitter. You may have noticed this factif you have ever gotten soap, a basic substance, in your mouth. As withacids, taste should NEVER be used to test a substance to see if it is abase. Many bases are caustic; they attack the skin and tissues, causingsevere burns.2. Bases change the color of acid-base indicators. As Figure 1.7 shows, anindicator will be a different color in a basic solution than it would bein an acidic solution.Acids and Bases445
3. Dilute aqueous solutions of bases feel slippery. You encounter thisproperty of aqueous bases whenever you wash with soap.4. Bases react with acids to produce salts and water. The properties of abase disappear with the addition of an equivalent amount of an acid.It could also be said that “neutralization” of the base occurs whenthese two substances react to produce a salt and water.5. Bases conduct electric current. Like acids, bases form ions in aqueoussolutions and are thus electrolytes.Household Acids and BasesQuestionWhich of the household substancesare acids, and which are bases?ProcedureRecord all your results in a datatable.1. To make an acid-base indicator,extract juice from red cabbage.First, cut up some red cabbageand place it in a large beaker.Add enough water so that thebeaker is half full. Then, bringthe mixture to a boil. Let it cool,and then pour off and save thecabbage juice. This solution isan acid-base indicator.4. Add a drop or two of the redcabbage juice to the solutionbeing tested, and note thecolor. The solution will turn redif it is acidic and green if it isbasic.Discussion1. Are the cleaning productsacids, bases, or neither?2. What are acid/base characteristics of foods and beverages?3. Did you find consumer warninglabels on basic or acidic products?Safety2. Assemble foods, beverages,and cleaning products to betested. ear safetyWgoggles, glovesand an apron.3. If the substance being tested isa liquid, pour about 5 mL into asmall beaker. If it is a solid,place a small amount into abeaker, and moisten it withabout 5 mL of water.Red cabbage, which contains ananthocyanin pigment, can be madeinto an acid-base indicator.446Chapter 14Materials dishwashing liquid, dishwasherdetergent, laundry detergent,laundry stain remover, fabricsoftener, and bleach mayonnaise, baking powder,baking soda, white vinegar, cidervinegar, lemon juice, soft drinks,mineral water, and milk fresh red cabbage hot plate beaker, 500 mL or larger beakers, 50 mL spatula tap water tongs
Main IdeaArrhenius acids and bases produce ions in solution.Svante Arrhenius, a Swedish chemist who lived from 1859 to 1927,understood that aqueous solutions of acids and bases conducted electriccurrent. Arrhenius therefore theorized that acids and bases must produceions in solution. An Arrhenius acid is a chemical compound that increasesthe concentration of hydrogen ions, H , in aqueous solution. In other words,an acid will ionize in solution, increasing the number of hydrogen ionspresent. An Arrhenius base is a substance that increases the concentration ofhydroxide ions, OH-, in aqueous solution. Some bases are ionic hydroxides.These bases dissociate in solution to release hydroxide ions into thesolution. Other bases are substances that react with water to remove ahydrogen ion, leaving hydroxide ions in the solution.Aqueous Solutions of AcidsThe acids described by Arrhenius are molecular compounds with ionizable hydrogen atoms. Their water solutions are known as aqueous acids.All aqueous acids are electrolytes.Because acid molecules are sufficiently polar, water molecules attractone or more of their hydrogen ions. Negatively charged anions are leftbehind. As explained in a previous chapter, the hydrogen ion in aqueoussolution is best represented as H3O , the hydronium ion. The ionizationof an HNO3 molecule is shown by the following equation. Figure 1.8 alsoshows how the hydronium ion forms when nitric acid reacts with water.HNO3(l) H2O(l) H3O (aq) NO 3 (aq)Similarly, ionization of a hydrogen chloride molecule in hydrochloricacid can be represented in the following way.HCl(g) H2O(l) H3O (aq) Cl-(aq)Figure 1.8Arrhenius Acids Arrhenius’s observations form the basis of a definition of acids. Arrheniusacids, such as the nitric acid shown here, produce hydronium ions in aqueous solution. HNO3HNO3Nitric acidNitric acid H 2OH2OWaterWater–H 3O H3O HydroniumNO 3 –ionHydronium ion NO Nitrate3Nitrate ionAcids and Bases447
Figure 1.9Common Aqueous AcidsStrong acidsWeak acidsHI H2O H3O I- H O SO 2 HSO 4 H2O 4 3-HClO4 H2O H3O ClO 4 H O H PO H3PO4 H2O 32 4 HBr H2O H3O Br- H O FHF H2O 3HCl H2O H3O Cl- H O CH COOCH3COOH H2O 33 H O HCO - H2SO4 H2O H3O HSO 4 H2CO3 H2O 33-HClO3 H2O H3O ClO 3 H O HSH2S H2O 3 H O CNHCN H2O 3 H O CO 2 HCO 3 H2O 3 3Strength of AcidsA strong acid is one that ionizes completely in aqueous solution. A strong acidis a strong electrolyte. Perchloric acid, HClO4, hydrochloric acid, HCl, andnitric acid, HNO3, are examples of strong acids. In water, 100% of the acidmolecules are ionized. The strength of an acid depends on the polarity ofthe bond between hydrogen and the element to which it is bonded andthe ease with which that bond can be broken. Acid strength increaseswith increasing polarity and decreasing bond energy.An acid that releases few hydrogen ions in aqueous solution is a weak acid.The aqueous solution of a weak acid contains hydronium ions, anions,and dissolved acid molecules. Hydrocyanic acid is an example of a weakacid. In aqueous solution, both the ionization of HCN and the reversereaction occur simultaneously. In a 1 M solution of HCN there will beonly two H ions and two CN- ions out of 100,000 molecules. The other99,998 molecules remain as HCN. H O (aq) CN-(aq)HCN(aq) H O(l) 23Common aqueous acids are listed in Figure 1.9. Each strong acidionizes completely in aqueous solution to give up one hydrogen ion permol ecule. Notice that the number of hydrogen atoms in the formula doesnot indicate acid strength. Molecules with multiple hydrogen atoms maynot readily give them up. The fact that phosphoric acid has three hydrogen atoms per molecule does not mean that it is a strong acid. None ofthese ionize completely in solution, so phosphoric acid is weak.Organic acids, which contain the acidic carboxyl group—COOH, aregenerally weak acids. For example, acetic acid, CH3COOH, ionizesslightly in water to give hydronium ions and acetate ions, CH3COO-. H O (aq) CH COO-(aq)CH COOH(aq) H O(l) 3448Chapter 14233
A molecule of acetic acid contains four hydrogen atoms. However, only oneof the hydrogen atoms is ionizable. The hydrogen atom in the carboxylgroup in acetic acid is the one that is “acidic” and forms the hydronium ion.This acidic hydrogen can be seen in the structural diagram in Figure 1.10.Aqueous Solutions of BasesMost bases are ionic compounds containing metal cations and thehydroxide anion, OH-. Because these bases are ionic, they dissociate whendissolved in water. When a base completely dissociates in water to yieldaqueous OH‑ ions, the solution is referred to as strongly basic. Sodiumhydroxide, NaOH, is a common laboratory base. It is water-soluble anddissociates as shown by the equation below.Figure 1.10Acetic Acid Acetic acid contains fourhydrogen atoms, but only one of them is“acidic” and forms the hydronium ion insolution. H O H – C – C – O – H Hacidic hydrogenHO2 Na (aq) OH-(aq)NaOH(s) ― As you will remember from learning about the periodic table, Group 1elements are the alkali metals. This group gets its name from the fact thatthe hydroxides of Li, Na, K, Rb, and Cs all form alkaline (basic) solutions.Not all bases are ionic compounds. A base commonly used in household cleaners is ammonia, NH3, which is molecular. Ammonia is a basebecause it produces hydroxide ions when it reacts with water molecules,as shown in the equation below. NH (aq) OH-(aq)NH (aq) H O(l) 342Strength of BasesAs with acids, the strength of a base also depends on the extent to whichthe base dissociates, or adds hydroxide ions to the solution. For example,potassium hydroxide, KOH, is a strong base because it completelydissociates into its ions in dilute aqueous solutions.check for understandingDifferentiate What is the differencebetween the strength and the concentration of an acid or base?HO2 K (aq) OH-(aq)KOH(s) ― Strong bases are strong electrolytes, just as strong acids are strong electrolytes. Figure 1.11 lists some strong bases.Figure 1.11Common Aqueous AcidsStrong basesWeak basesCa(OH)2 Ca2 2OH- NH OHNH3 H2O 4Sr(OH)2 Sr2 2OH- C H NH C6H5NH2 H2O 3 OH6 5Ba(OH)2 Ba2 2OHNaOH Na OHKOH K OHRbOH Rb OHCsOH Cs OHAcids and Bases449
Figure 1.12Insoluble Hydroxides Thehydroxides of most d-block metals arenearly insoluble in water, as is shown by thegelatinous precipitate, copper(II) hydroxide,Cu(OH)2, in the beaker on the right.Chloride ion,ClNa (aq) OH-(aq)Chloride ion, Cl-Sodium ion,Na Cu(OH)2(s)Copper(II) ion,Cu2 Water molecule,H2OCu2 (aq) 2OH-(aq) Cu(OH)2(s)Bases that are not very soluble do not produce a large number ofhydroxide ions when added to water. Some metal hydroxides, such asCu(OH)2, are not very soluble in water, as seen in Figure 1.12. They cannotproduce strongly alkaline solutions. The alkalinity of aqueous solutionsdepends on the concentration of OH- ions in solution. It is unrelated tothe number of hydroxide ions in the undissolved compound.Now consider ammonia, which is highly soluble but is a weak electrolyte. The concentration of OH- ions in an ammonia solution is relativelylow. Ammonia is therefore a weak base. Many organic compounds thatcontain nitrogen atoms are also weak bases. For example, codeine,C18H21NO3, a pain reliever and common cough suppressant found inprescription cough medicine, is a weak base.Section 1 Formative ASSESSMENTReviewing Main Ideas1. a. What are five general properties of aqueousacids?b. Name some common substances that haveone or more of these properties.2. Name the following acids: a. HBrO b. HBrO3.3. a. W hat are five general properties of aqueousbases?b. Name some common substances that haveone or more of these properties.450Chapter 144. a. Why are strong acids also strong electrolytes?b. Is every strong electrolyte also a strong acid?Critical Thinking5. relating ideas A classmate states, “Allcompounds containing H atoms are acids, andall compounds containing OH groups are bases.”Do you agree? Give examples.
Acids react with bases to produce salts and water. When chemically equivalent amounts of acids and bases react, the three properties just described disappear because the acid is “neutralized.” The reaction products are water and an ionic compound called a salt. 5. Acids conduct electric curr
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
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
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
vii SCOPE AND SEQUENCE Section Title Syllabus objectives UNIT 6 Acids and Alkalis 6.1 Acids, bases and alkalis State that compounds can be classified as acids and alkalis Identify common acids, alkalis and salts Create a safety booklet dealing with the handling of acids and alkalis Investigate selected reactions of acids and alkalis Cite practical examples of neutralisation .
Therefore, acids and bases are electrolytes. Strong acids and bases will be strong electrolytes. Weak acids and bases will be weak electrolytes. This affects the amount of conductivity. However, acids will react with metal, so testing conductivity may not be plausible. Physical 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
_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. 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 .
