#Chem 162-2008 6th week recitation truncated

#Chem 162-2008 6th week recitation truncated - TAVSS'...

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CHEMISTRY 162-2008 6 th WEEK RECITATION ANNOUNCEMENTS E-MAIL ATTENDANCE Sign in EXAMS    See results QUIZ Recitation quiz this week; sections 14.1 – 15.3 Pick up old quizzes after class. Chem 162-2008 6 th week recitation 1 Rutgers/Pharmacy CHEM 162-2007 EXAM I SCORES ALL SECTIONS RUTGERS SECTIONS AVERAGE TAVSS’ SECTIONS AVERAGE
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PLAN FOR TODAY : CHAPTER 14 ACIDS AND BASES EQUILIBRIUM Nature of acids and bases Autoionization of water and the pH scale Solutions of acids and bases Acid-base properties of salts Relationships between structure and strengths of acids and bases Lewis acids and Bases Chem 162-2008 6 th week recitation 2
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CHEMICAL, ACID AND BASE EQUILIBRIA pH [H + ] 14 Basic 1x10 -14 H 2 O + H 2 O H 3 O + + OH - K w = 1x10 -14 7 Neutral (e.g. H 2 O) 1x10 -7 K w = [H + ][OH - ] = 1 x 10 -14 pH + pOH = 14 K w = K a x K cb = K ca x K b = 1 x 10 -14 * *a & b = acid and base; ca & cb = conjugate acid and conjugate base pK a + pK b = 14 0 Acidic 1x10 o pH = -log[H + ] pH [H + ] [H + ] = 10 -pH pOH = -log[OH - ] [OH - ] = 10 -pOH pOH [OH - ] Chem 162-2008 6 th week recitation 3 H + pOH = 14 pH + pOH = 14 [H + ][OH - ] = 1 x 10 -14 H pOH = -log[OH - ] [OH - ] = 10 -pOH pH = -log[H + ] [H + ] = 10 -pH
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REACTIONS OF ACIDS AND BASES WITH WATER ET: Discuss Bronsted-Lowry acids and bases (an acid is a proton donor, and a base is a proton acceptor); acid base reaction; amphoteric substances; ACID + WATER H H — A + :A - + H H H R—N—H + R—N: H H H .. R - N - H + R - N - H + H H H A:─ H─A + H Chem 162-2008 6 th week recitation 4 H ·· : O H H : O + H : O H ·· : O : + H : O + H H ·· : O H + : O H ·· : O :
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NATURE OF ACIDS AND BASES ET: Discuss three types of acids and bases. ET: Discuss recommendation to have weak acids react with H 2 O. ET: Discuss Lowry-Bronsted conjugate acid and conjugate base. 14.31 For the following aqueous reaction, identify the acid, the base, the conjugate base, and the conjugate acid. a. HF + H 2 O F - + H 3 O + HF is an acid; F - is its conjugate base. H 2 O is a base; H 3 O + is its conjugate acid. or H 3 O + is an acid; H 2 O is its conjugate base. F - is a base; HF is its conjugate acid. Chem 162-2008 6 th week recitation 5
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SIX STRONG ACIDS ET: Discuss strong acids and strong bases and the strengths of their conjugate bases and acids; practice both. Very weak base (i.e., not a base; K a Acid spectator ion) ~10 6 HCl + H 2 O H 3 O + + Cl - ~10 8 HBr + H 2 O H 3 O + + Br - ~10 9 HI + H 2 O H 3 O + + I - H 2 SO 4 + H 2 O H 3 O + + HSO 4 - HNO 3 + H 2 O H 3 O + + NO 3 - HClO 4 + H 2 O H 3 O + + ClO 4 - (HClO 3 + H 2 O H 3 O + + ClO 3 - )* *Strong, but not common, acid. Generally not considered as a strong acid. All other acids are weak acids, e.g., HA (acetic acid), H 2 SO 3 , RNH 3 + , BF 3 Arrhenius acid: Anything that provides a proton, e.g., HA, H 2 SO 3 , RNH 3 + LB Acid: Anything tending to give up a proton, e.g., HA, H 2 SO 3 , RNH 3 + Lewis Acid: Anything tending to react with an electron pair, e.g., BF 3 NINE STRONG BASES (Most Group 1A and 2A hydroxides [not HOH]) e.g. Very weak acid (i.e., not an acid; Base spectator ion) LiOH OH - + Li + NaOH OH - + Na + Mg(OH) 2 2OH - + Mg 2+ Ba(OH) 2 2OH - + Ba 2+ All other bases are weak bases, e.g., RNH 2 , CO 3 2- Arrhenius Base: Anything that provides an OH- group, e.g., NaOH LB Base: Anything that tends to react with a proton, e.g., NaOH, RNH 2
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This note was uploaded on 09/23/2009 for the course CHEM 162 taught by Professor Siegal during the Spring '08 term at Rutgers.

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#Chem 162-2008 6th week recitation truncated - TAVSS'...

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