C142A Ch 7 2011 lecture notes rev

C142A Ch 7 2011 lecture notes rev - Test 2 Mon. Nov. 21:...

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Test 2 Mon. Nov. 21 : Same rules as on Test 1. Covers all material through section 7.6 of Ch. 7 (slight change from syllabus, which had only through section 7.4) NOTE: this change also made in ALEKS Obj. #6: due Fri. (11/18): covers Chapter 7.1 7.6 Check new seat assignments posted on web by Wednesday. CLUE will be holding review sessions for Exam 2 and Final: see next page for times / locations (which is posted in lecture notes)
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CLUE will be holding review sessions for Exam 2 and Final. Times / locations: Midterm II Thursday Nov. 17 6:30 - 8:30pm Mary Gates Hall 287 Poplar Hall Room 104 (main lounge), Monday November 14, 7-10 pm McCarty Hall Room C, Sunday, November 13, 7:00-10:00pm Final Thursday Dec. 8 6:30-8:30pm Mary Gates Hall 287 Poplar Hall Room 106 Sunday December 11 7:00-10:00pm McCarty Hall Room 334 Sunday December 11 7:00-10:00pm
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Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The pH Scale 7.4 Calculating the pH of Strong Acid Solutions 7.5 Calculating the pH of weak Acid Solutions 7.6 Bases 7.7 Polyprotic Acids 7.8 Acid-Base Properties of Salts 7.9 Acid Solutions in Which Water Contributes to the H + Concentration 7.10 Strong Acid Solutions in Which Water Contributes to the H + Concentration 7.11 Strategy for solving Acid-Base Problems: A Summary
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From Chapter 4: Acids and Bases An Acid is a substance that produces H + (H 3 O + ) ions when dissolved in water, and is a proton donor A Base is a substance that produces OH - ions when dissolved in water: Example: NaOH(aq) ! Na + (aq) + OH - (aq) The OH - ions react with the H + ions (if an acid is present) to produce water, H 2 O, and are therefore proton acceptors . Acids and Bases are electrolytes. Their strength is categorized in terms of their degree of dissociation in water to make hydronium or hydroxide ions. Strong acids and bases dissociate completely , and are strong electrolytes. Weak acids dissociate partially (some small % of the molecules dissociate) and are weak electrolytes.
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Selected Acids and Bases Acids Bases Strong: H + (aq) + A - (aq) Strong: M + (aq) + OH - (aq) Hydrochloric, HCl Sodium hydroxide, NaOH Hydrobromic, HBr Potassium hydroxide, KOH Hydroiodoic, HI Calcium hydroxide, Ca(OH) 2 Nitric acid, HNO 3 Strontium hydroxide, Sr(OH) 2 Sulfuric acid, H 2 SO 4 Barium hydroxide, Ba(OH) 2 Perchloric acid, HClO 4 Weak Weak Hydrofluoric, HF Ammonia, NH 3 Phosphoric acid, H 3 PO 4 accepts proton from water to make Acetic acid, CH 3 COOH NH 4 + (aq) and OH - (aq) (or HC 2 H 3 O 2 )
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Strong Acids and the Molarity of H + Ions in Aqueous Solutions of Acids Problem: In aqueous solutions, each molecule of sulfuric acid will loose one proton to yield one H + ion and one HSO 4 - ion. (Approx.) What is the molarity of the HSO 4 - and Hydronium ions in a solution prepared by dissolving 155 g of concentrated sulfuric acid into sufficient water to produce 2.30 Liters of acid solution?
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This note was uploaded on 01/18/2012 for the course CHEM 142A taught by Professor Campbell during the Fall '11 term at University of Washington.

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C142A Ch 7 2011 lecture notes rev - Test 2 Mon. Nov. 21:...

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