chapter 8 acids and bases 산과 염기. acids what is an acid? –hydrogen ion, proton (h + ) donor...
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Chapter 8
Acids and Bases
산과 염기
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Acids• What is an Acid?
– Hydrogen ion, proton (H+) donor
• Properties– Taste sour, reacts with metals, donates protons
• Classes of Acids
• Common Acids
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Acid Reaction• 물과의 반응
HA H+ + A-
H+ + H2O H3O+
HA(aq) + H2O(l) H3O+(aq) + A-
(aq)
• Acids increase the hydronium ion concentration in water
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Hydronium Ion
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Types of Acids• Strong
– Acids that dissociate completely in water– Inorganic Acids– HCl, H2SO4, HNO3, HClO4
• Weak– Acids that partially dissociate in water– Organic Acids– 강산을 제외한 대부분의 산
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Bases• What is a base?
– Hydrogen ion acceptor
– Hydroxide ion (OH-) and Ammonia (NH3)
• Properties– Taste bitter, forms insoluble hydroxide with
metals, accepts hydrogen ions
• Common Bases
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Base Reaction• Generic Reaction in Water
BOH B+ + OH-
OH- + H2O H2O + OH-
BOH(aq) B+(aq)
+ OH-(aq)
• Bases increase the hydroxide ion concentration
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Chemical Equilibrium• What determines strong vs weak?
• 화학 평형 Chemical Equilibrium– The state in a reaction when there in no change
in the concentration of the reactants or products– Reactions that proceed in both directions at the
same time (rate)
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Carbon Dioxide• Carbon Dioxide, CO2
CO2 + H2O H2CO3
H2CO3 + H2O H3O+ + HCO3-
HCO3- + H2O H3O+ + CO3
-2
H2CO3- + 2 H2O 2 H3O+ + CO3-2
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Acid-Base Pairs• Acid that loses a H+ becomes a base
– Called conjugate base
H2CO3 + H2O H3O+ + HCO3-
• 짝산 - 짝염기
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Water• Auto protolysis
H2O + H2O H3O+ + OH-
• Amphiprotic (Amphoteric)– substance that can behave as an acid or a base
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Water
• [H+] = 1 x 10-7 mol/L
• [OH-] = 1 x 10-7 mol/L
Kw = [H+] x [OH-] = 1 x 10-14
-
322OH OH OH OH
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pH Scale• Concentration [H+] or [OH-]
pH = - log [H+]
pOH = - log [OH+]
• What is the pH of neutral water?
pH + pOH = 14
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Conversions
• acidic/neutral /basic
• pH of common substances
OH H
pOH pH
-
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Measuring pH• Meters
– meter uses a standard electrode to measure the hydrogen ion concentration, [H+]
• Indicators– Molecules that change color depending on the
hydrogen ion concentration, [H+]
• Common Indicators
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Natural Indicators• Anthocyanins
– found in flower, fruits and vegetables
+O
OH
OH
OH
H O+O
OH
OH
OH
H O
OH
+O
OH
OH
OH
H O
OH
OH
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Neutralization
• 중화– process of adding acid or base to a solution to
achieve a neutral solution, pH = 7– equal amounts of acid and base
• 적정 , Titration– determination of the concentration of a
solution by reaction with a solution of known concentration
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Neutralization• 당량점 Equivalence Point
– the point in a titration when equal portions of the reactants have been added (stoichiometry)
• Mole Acid = Moles of Base
MAVA = MBVB
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Buffers• 완충용액 , Buffers
– chemical systems composed of acid-base pairs that resist changes in pH
– buffers contain an acid-base pair which maintain the pH
• Example – Acetic Acid and Sodium Acetate
H3C C
O
O- Na+H3C C
O
OH
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Buffers
• pH = pKa + log{[base form]/[acid form]}
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Homework• 교과서 281 쪽 연습문제
– 1, 5, 7, 23– 마감 1/10 목요일 수업시작 전까지