acids and bases. naming acids binary acids (contains h & 1 other element) hydro- and –ic if...
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Acids and Bases
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Naming AcidsBinary Acids (contains H & 1 other element)
• Hydro- and –ic if anion does not contain oxygen
HCl-hydrochloric acid
Oxyacids (contain H, O, & other elements)
• -ic anion ends in –ate
H2SO4 - SO4 is sulfate = sulfuric acid
• -ous anion ends in -ite
H2SO3-SO3 is sulfite = sulfurous acid
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Common Acids
• Sour milk (lactic acid)
• Vinegar (acetic acid)
• Carbonated beverages (phosphoric acid)
• Lemons, oranges (citric acid)
• Apples (malic acid)
• Grape Juice (tartaric acid)
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Sulfuric Acid
• Most commonly used product in the world
• Petroleum
• Automobile batteries
• Dehydration agent• Metallurgy• Refining
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Nitric Acid
• Stains proteins yellow• Suffocating odor• Stains skin• Causes burns
• Explosives
• Rubber
• Plastics
• Dyes
• Pharmaceuticals
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Phosphoric Acid
• Manufacturing fertilizers for plants and animal feed
• Flavoring agent in beverages• Cleaning agent for dairy equipment
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Hydrochloric acid
• Produced in the stomach• Cleaning agent
• Maintain acidity in pools
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Common Properties of Acids
• Sour taste
• Produce hydronium H3O+ ions
• Change the color of acid-base indicators
• React with active metals to release hydrogen gas
• React with bases to produce salts and water
• Conduct electric current
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Bases
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Common Bases
• Lye (sodium hydroxide)
• Milk of magnesia (magnesium hydroxide)
• Antacids (aluminum hydroxide)
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Common Properties of Bases
• Taste bitter
• Produce hydroxide OH- ions
• Change the color of acid-base indicators
• Feel slippery
• React with acids to produce salts and water
• Conduct electric current
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Specific Definitions of Acids/Bases
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Arrhenius Acids and Bases
• Arrhenius acid-increases H+ ions (H3O+)
H2SO4 + H2O H3O+ +HSO4-
• Arrhenius base-increases OH- ions
Ca(OH)2Ca+2 + 2OH-
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Weak/Strong
• Weak acid-weak electrolyte (end in -COOH)• Strong acid-ionizes completely, strong electrolyte
(HCl)• Alkaline-base completely dissociates in water to
yield OH- ions
NaOH Na+ + OH-
• Strong bases-completely dissociates, strong
electrolyte (end in OH)
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Bronsted-Lowry
• Bronsted-Lowry Acid-proton donor
• Bronsted-Lowry Base-proton acceptor
HCl + NH3NH4+ + Cl-
• Monoprotic acid-donates one proton HCl
• Diprotic acid-donates two protons H2SO4
• Triprotic acid-donates three protons H3PO4
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Conjugate Acids and Bases
• Conjugate base-the species that remains after a Bronsted-Lowry acid has given up a proton
HF + H2O F- + H3O+
Acid Conj. Base• Conjugate acid-the species that is formed when a
Bronsted-Lowry base gains a proton
HF + H2O F- + H3O+
Base Conj. Acid
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Strength of Acid/Conj. Base
Strong acidweak conjugate base
Weak acidstrong conjugate base
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Other Terms
• Amphoteric compound-any species that can react as either and acid or a base
• Neutralization-the reaction of hydronium ions and hydroxide ions to form water molecules and salt
Self-ionization of water H3O+ + OH- 2H2O or
H20 + H2OH3O+ + OH-
• Salt-an ionic compound composed of a cation from a base and an anion from an acid
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Buffers
• A solution that resists a change in its pH even when a strong acid or base is added to it.
• A solution is buffered by the presence of a weak acid and its conjugate base.
• Added H+ reacts with base
• Added OH- reacts with weak acid
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Titration Practice Problems
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Ex 1A 30.mL volume of HCl is
titrated with 23mL of 0.20M NaOH. What is the molarity of HCl in this solution?
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Answer
0.15M
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Ex 2 A 26mL volume of NaOH is
titrated with 23mL of 0.20MHCl. What is the molarity of NaOH in this solution?
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Answer
0.18M
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Ex 3A 40.mL volume of H2SO4 is
titrated with 38mL of 0.24M NaOH. What is the molarity of H2SO4 in this solution?
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Answer
0.11M
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Acid/Base Rhapsody
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Is this the real life? Is this just fantasy? No protons around here. Hydronium reality. Open your book and take a look and seeeeeeeeeeeee…. I’m just a poor student – prof. give me your sympathy. Marks are easy come, they’re easy go. Sometimes they’re high, sometimes they’re low. As long as you understand it, it doesn’t really matter to me - to me.
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Mama, just had my class, Learned about Arrhenius, Bronsted Lowry, Lewis acids. Conjugate acid/base pairs. Amphoteric and hydrides pull my hair. Mama, oo-ooo-ooo-ooh, Some salts with hydrolize. If I don’t call again this time tomorrow. Carry on, carry on, I’m studying for this test.
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Mama lots to learn acids strong and weak.
Leveling affect- an A is what I seek.
Acid-ionization constants-O, my brain is sore.
Oxyacids, indicators change color!
Mama oooooooooo.
Water auto-ionizes forms hydroxide and hydronium all the time. What??
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I see a little acid and its conjugate base - Got a buffer! Got a buffer! Will you do the calculation?! Want a certain pH, find the pka that’s near. Bronsted-Lowry, Bronsted-Lowry,Bronsted-Lowry, Bronsted-Lowry rules the day. O-o-o-o-ow… I’m just a poor student spent my money at dance clubs. He’s just a poor student studies titrations at home. Spare him this question of a polyprotic acid.
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Easy come easy go-indicator tells youNow is the endpoint near
I overshot again (and over)I overshot again (and over)I think I got it now…. I got it nowOhOhOhOhOhOhIndicator, indicator, indicator lets me knowThe lab TA has a buret to decide for me.for me, for me, For MEEEEEEEEEEEEEEEEEEEEE!!!!!!
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So you think you can do an acid/base titration!!! But when you overshoot the endpoint, it just leads to frustration.Oh, maybe, just a little more base maybe.
I’ll think I’ll get it right. I got to get it right this time.
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Doesn’t really matter-acid or base the same.
Doesn’t really matter
Doesn’t really matter to meeeeeeeeeee.
Doesn’t really matter to me.