Acid and Base Chemistry
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Transcript of Acid and Base Chemistry
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Acid and Base Chemistry
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Review• Acids• pH less than 7• Turns litmus from blue to red• Sour taste
• Bases• pH greater than 7• Turns litmus from red to blue• “slippery” feeling
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Definitions• Arrhenius• Acids produce H+ ions, bases produce OH- ions in
aqueous solutions• Limits the number of reactions considered Acid-Base
• Bronsted-Lowry• Acid is an H+ donor• Base is an H+ acceptor
• Lewis• Acid Accepts an electron pair• Base donates an electron pair
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Properties of acids1. Sour taste
citric, malic, tartaric are well known food additives
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Properties of Acids
2. Contain the hydrogen ion (H+ ), react with active metals to give off H2 gas
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Properties of Acids3. Change the color of indicators
Low pH
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Properties of acids
4. React with bases to produce salts and water
Base + Acid → Water + Salt2NaOH + H2SO4 → 2H2O + Na2SO4
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Properties of Acids5. Acids are electrolytes
Break apart and form ionscan conduct electricity
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Common acids• HCl – hydrochloric acid• H2SO4 – sulfuric acid• HC2H3O2 – acetic acid - vinegar• HNO3 – nitric acid• H3PO4 – phosphoric acid• H2CO3 – carbonic acid
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Hydrochloric Acid (Muriatic Acid)• Produced in the stomach and aids in digestion• Industrial Cleaning Agent
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Sulfuric Acid• #1 industrial chemical• Fertilizers, petroleum refining, metallurgy• Production of metal, paper, paint, detergents• Used as a measure of a country’s economy
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Acetic Acid• Dilute acetic acid is vinegar• Used in making plastics• Raw material necessary in the production of food
supplements
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Nitric Acid• Explosive making uses nitric acid, due to its
instability• Used in the rubber and plastics industry• Dyes and drug production also utilize nitric acid
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Phosphoric Acid• Manufacture of fertilizers and animal feed• Detergents and ceramics also utilize phosphoric
acid• Carbonated beverage production
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Carbonic Acid• Made from dissolving carbon dioxide (CO2) in
water• Sodas, or any carbonated beverage.
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Monoprotic Acid vs Diprotic acid• Monoprotic Acids donate 1 proton (H+) • Ie HCl
• Diprotic Acids donate (2) protons (H+) per molecule• Ie: H2SO4
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Triprotic acids• Donates (3) protons• Example: H3PO4
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Strong vs Weak Acids and Bases• Does not mean dangerous vs safe• Strong Acids ionize completely• Every available H+ ion is separated from anion in aqueous
solution• If 0.1 mol of HCl is added to water, then 0.1 mol of H+,
and 0.1 mol of Cl- are fromed• Table 4.1
• Weak Acids do not ionize completely• We use a reversible reaction (double) arrow to represent
not complete ionization
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Bases
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Properties of bases1. Bitter taste
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Properties of Bases
2. Feel slippery to the skin
3. Change color of indicatorsHigh pH
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Properties of Bases
4. React with acids to produce water and salts
2NaOH + H2SO4 → 2H2O + Na2SO4
5. Bases are electrolytes
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Common bases
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Sodium hydroxide
• (NaOH), also known as lye or caustic soda, is a caustic metallic base. It is widely used in many industries, mostly as a strong chemical base in the manufacture of pulp and paper, textiles, drinking water, soaps and detergents. Worldwide production in 1998 was around 45 million tons.
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Ammonium hydroxide• (NH4)(OH)• Common household cleaner
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pH scale
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pH Equation• - log [H+]• If [H+] = 1 x 10-8 M• Then –log[1 x 10-8] = pH pH = 8
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pH Equation• Notice pH can be estimated by the exponent • -log(1.0 x 10-5) = pH of 5• -log(1.0 x 10-9) = pH of 9• -log(1.0 x 10-13) = pH of 13
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If [H+] = 3.4 x 10-5 find pH = -[(log 3.4 x 10-5)]
= -[(log 3.4 + log 10-5)] = -[(0.53) + (-5)] = -(0.53 – 5) = 4.47
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Reactions• Neutralization of Acids / Base• When acid and base react to an equivalence point• Where all H+ ions have reacted with all OH- ions to
produce _________?
“Spectator Ions” – Ions that do not actually take part in the reaction.
Often times, the other ion in the acid or base, that gets separated from the H+ or OH- doesn’t really take part in the reaction.
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If [H+] = 3.4 x 10-5 find pH = -[(log 3.4 x 10-5)]
= -[(log 3.4 + log 10-5)] = -[(0.53) + (-5)] = -(0.53 – 5) = 4.47
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Neutralization reactions• React an Acid and a Base together to form water,
bring pH to neutral• Reaction of hydronium ions (H3O+) and hydroxide
(OH-) ions to form water• Hydronium is sometimes simplified to H+
H3O+ + OH- 2H2OorH+ + OH- H2O or H+OH-
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Titration
• Controlled addition & measurement of an amount of solution of a known concentration, that is required to react completely with a measured amount of solution of unknown concentration.
• Example: HCl + NaOH NaCl + H2OA 100.0 mL sample of HCl is titrated to a stoichiometric endpoint with 76.8 mL of a 1.17 M NaOH. What is the molarity of the HCl?
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Acid-Base Titrations• Reaction to an equivalence point (pH 7)
• Used to determine the concentration of an unknown solution.
• If you find how much volume of a known concentration (standard) you need to add to a known volume of an unknown concentration……
• If I have 25.0 mL of a .316 M solution of H2SO4, What volume of NaOH do I need to neutralize it?
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Graph of titration typical titration curve