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BYUI CHEM 105 - Acids and bases, salts and solutions

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Acids and bases, salts and solutionsKey conceptsVarious properties of acids and basesArrhenius theory of acids/basesProtons are not alone….Brønsted-Lowry theory (1923)Ionization of weak acids/basesConjugate acid-base pairsAcid/base strengthAmphoterismAcid strengthLeveling solventsSlide 13Ternary acids and basesTernary acid strengthimportant!Neutralization of Brønsted-Lowry acids/basesWeak acid + strong baseAcid saltsLewis theorySlide 21When is Lewis theory used?Acid-Base calculationsMolaritySimilarities between acid-base and other reaction calculationsSome examplesTITRATIONSTitrations (con’t)Primary and secondary standardsEQUIVALENT WEIGHTS AND NORMALITYnormalityEQUIVALENTS in acid/base reactionsAcids and bases, salts and solutionsChapter 10-1 – 10-9, 11-1 – 11-4Key concepts•Compare and contrast the Arrhenius and Brønsted-Lowry theories of acids and bases•Describe hydrated protons•Properties of acid and base solutions•Arrange acids according to acid strength•Balance acid-base equations•Amphoterism•Lewis acid-base theory•Molarity calculations in titrations•EquivalentsVarious properties of acids and basesAcids BasesTaste Sour (e.g., vinegar, citrus) Bitter (e.g., baking soda)Indicators Litmus paper: redPhenophthalein: clearLitmus paper: bluePhenophthalein: pink/purpleReactivity w/ metalsReacts w/ metals above H in activity series to produce H2 (g)Normally non-reactiveReactivity w/MO, MOHReact to form salt + H2O Metal hydroxides are basesOther rxns Strong acid + weak acid salt → weak acid + strong acid saltReacts with lipids (soap + grease)Acid + base → salt + waterconductivity Electrolytic solution Electrolytic solutionArrhenius theory of acids/bases•Developed in 1884.•An acid is a substance containing hydrogen that produces _______ in aqueous solution.•A base is a substance containing the OH group that produces _______ in aqueous solution.Protons are not alone….•Protons combine with water molecules to form __________ ___________.•We commonly represent this as the hydronium ion, H3O+(aq), but writing H+(aq) means the same thing.Brønsted-Lowry theory (1923)•An acid is a _______ _________.•A base is a ________ __________.•Bases are no longer restricted to compounds that release OH- in solution. For instance, NH3 is a base. What does it look like after reacting with a proton?Ionization of weak acids/bases•While strong acids dissociate completely, not all reactions are complete and irreversible (in fact, most are not).•Rxns with weak acids/bases are reversible. Example: HF + H2O•What is the acid? What is the base? (depends on which side of rxn you look at)Conjugate acid-base pairs•Conjugate acid-base pairs differ in structure by ___ _________.•Some examples of conjugate pairs:Acid/base strength•The strength of an acid is _______ proportional to the strength of its base.•Strong acids have ________________.•Weaker acids have ________________. As the acid gets weaker and weaker, what happens to the conjugate base? What does this tell you about the amount of ionization taking place?Amphoterism•Some substances can both give and accept protons. This process is called amphoterism. •Water is the prime example of amphiprotic behavior.2H2O → H3O+ + OH-Acid strength•The hydrohalic acids: HF, HCl, HBr, HI•What are the sizes of the halogens? How will this affect the H-X bond?•HF bond is very strong vs. the other halogens.•F- causes ordering of the H2O molecules (how does that happen?)Leveling solvents•In aqueous solution, no acid is stronger than H3O+(aq). All other acids completely dissolve in water to form H3O+.•Because of this, all strong acids are of equal strength in water.•A similar effect is observed for strong bases, which completely dissolve to form OH-.Ternary acids and bases•What is a ternary acid?•Ternary acids are hydroxyl compounds of a ______________.•Ionize to produce H+.•Compare to other hydroxyl compounds…•Metal hydroxides—ionize to produce ________________ and are ________ in aqueous solution.Ternary acid strength•H2SO4 vs H2SO3. What’s the difference in acid strength?–Compare oxidation number of sulfur in each.•Acid strength increases with _______ oxidation number of the central atom.•Order the following acids from weakest to strongest:– HBrO3, HBrO, HBrO4, HBrO2important!•When comparing ternary acid strength, make sure the compounds have similar structure.•Where are the hydrogens located?•(H3PO3 vs H3PO4)Neutralization of Brønsted-Lowry acids/basesHA + MB → HB + MA•In many cases, HB ends up being ______.•Classic example: strong acid + strong base.•What happens in the reaction of hydrochloric acid and sodium hydroxide?•What is the net ionic equation?Weak acid + strong base•General reaction:HxA (aq) + x OH- (aq) → A- (aq) + x H2O (l)–When does x vary?–Examples:Acid salts•Acid salts are salts of ______ acids that still contain __________ ___________.Lewis theory•The most general of all acid-base theories–Discards the proton acceptor/donator all together.•A Lewis acid _______ a share in an electron pair.•A Lewis base _________ a share in an electron pair.•Lewis acids and bases are neutralized when a ________ _______ forms.Bronsted-LowryWhen is Lewis theory used?ArrheniusLEWIS THEORYArrhenius or B-L theorya better description for most aqueous sol’nsLewis theory a gooddescriptor for nonaqueoussolvents or transition metalsAcid-Base calculations•Molarity calculations play an important part in acid-base reaction stoichiometry•Much of what we will learned in Chapter 3 will be used here.Molarity•M = mol/L or•M = mmol/mL•we can use moles and liters, or millimoles and milliliters, and the molarity is still the same.Similarities between acid-base and other reaction calculations•We still compare moles to moles, not volumes to volumes or molarities to molarities.•Additionally, knowing the limiting reactant is very important (i.e, what will run out first—acid or base?)Some examples1. what volume of 0.800 M NH3 is required to neutralize 22.0 mL of 12.0 M HCl?2. 25.0 mL of 0.0500 M Ca(OH)2 added to 10.0 mL of HNO3. –Is the solution now acidic or basic?–how many moles excess acid or base are in the solution?–how much additional Ca(OH)2 or HNO3 sol’n required to neutralize solution?TITRATIONS•Combining a known concentration with an unknown concentration solution.•Titrant: The solution of one


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BYUI CHEM 105 - Acids and bases, salts and solutions

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