chapter 15 acids and bases. sect. 15-1: properties of acids and bases acids have a sour taste ...
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Chapter 15
Acids and Bases
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Sect. 15-1: Properties of Acids and Bases
AcidsHave a sour tasteChange the color of acid-base indicatorsSome react with metals to produce hydrogen
gas (if above hydrogen on activity series)React with bases to produce a salt and waterSome conduct electric current
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Acid nomenclature Binary acid – contains hydrogen and one other
element (hydro- root –ic acid) Oxyacid – contains hydrogen, oxygen, and one other
element (-ate polyatomic ions become –ic acids and –ite polyatomic ions become –ous acids)
Common industrial acids Sulfuric acid – petroleum refining, metallurgy, fertilizer Nitric acid – explosives, plastics, pharmaceuticals, etc Phosphoric acid – fertilizer, animal feed, soft drinks Hydrochloric acid – metal work, cleaning masonry Acetic acid – used in chemical synthesis
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BasesTaste bitterChange the color of acid-base indicatorsFeel slipperyReact with acids to produce a salt and waterConduct electric current
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Arrhenius acid – a chemical compound that increases the concentration of hydrogen ions in aqueous solution
Arrhenius base – a substance that increases the concentration of hydroxide ions in aqueous solution
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Aqueous solutions of acidsAcid molecules attract water molecules which
take the hydrogen (forming hydronium, H3O+) and leave behind an anion
HNO3 + H2O H3O+ + NO3-
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Aqueous solutions of bases Ionic compound will dissociate to produce
cations and hydroxide ions NaOH Na+ + OH-
Alkaline – a solution that is created when a base completely dissociates in water to yield aqueous hydroxide ions
Other bases produce hydroxide ions by reacting with water molecules
NH3 + H2O NH4+ + OH-
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Strength of acids and bases
Strong acid – ionizes completely in aqueous solutions; strong electrolyte
Weak acid – acids that are weak electrolytes
Strong bases – strong electrolytes Weak bases – produces a relatively low
concentration of hydroxide ions in solution
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Strong acids Chloric acid Hydrobromic acid Hydrochloric acid Hydroiodic acid Nitric acid Perchloric acid Sulfuric acid
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Sect. 15-2: Acid-Base Theories
Arrhenius definition of acid/base requires aqueous solutions, but substances act as acid/base at other times as well, so other definitions had to be created (Brønsted-Lowry and Lewis)
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Brønsted-Lowry acid – a molecule or ion that is a proton donor (remember, H+ is a proton)
Brønsted-Lowry base – a molecule or ion that is a proton acceptor
HCl + NH3 NH4+ + Cl-
HCl is acting as an acid and NH3 as a base by B-L definition
Brønsted-Lowry acid-base reaction – protons are transferred from one reactant (the acid) to another (the base)
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Monoprotic acid – an acid that can donate only one proton per molecule (ex. HCl)
Polyprotic acid – an acid that can donate more than one proton per molecule (ex. H2SO4)Hydrogen atoms are lost one at a timeDiprotic acid – can donate 2 protons per
moleculeTriprotic acid – can donate 3 protons per
molecule
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Lewis acid – an atom, ion, or molecule that accepts an electron pair to form a covalent bond
Lewis base – an atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis acid-base reaction – the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor
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Sect. 15-3: Acid-Base Reactions
Conjugate base – the species that remains after a Brønsted-Lowry acid has given up a protonHF + H2O F- + H3O+
Since HF is the acid, F- is the conjugate base
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Conjugate acid – the species that is formed when a Brønsted-Lowry base gains a protonHF + H2O F- + H3O+
Since water is acting as a base, the H3O+ is the conjugate acid
The base and its conjugate acid are referred to as a conjugate acid-base pair
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Strength of conjugate acid/base
Strong acids produce weak conjugate bases The stronger a base, the weaker its conjugate
acid will be Pg. 471 Proton transfer reactions favor the production of
the weaker acid and weaker base
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Amphoteric – any species that can react as either an acid or a baseWater acts as base with HCl, but was acid
with NH3
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Molecular compounds containing the hydroxyl group (-OH) can either be amphoteric or acidic
The more oxygen atoms attached to the atom to which the –OH group is attached, the more acidic it will be due to polarity of the bonds
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Neutralization reactions
Neutralization – reaction of hydronium ions and hydroxide ions to form water molecules
Salt – an ionic compound composed of a cation from a base and an anion from an acid
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Acid rain is caused by gases (NO, NO2, SO2, SO3) from industrial processes reacting with water vapor in the air to form acids such as sulfuric and nitric acid
Acid rain reacts with marble in statues and buildings, eroding it away