C142A Exam 2 Review Ch 5-7.6

C142A Exam 2 Review Ch 5-7.6 - Same rules as Test 1: Bring...

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Test 2 on Monday! Same rules as Test 1: Bring Scantron, #2 pencil, proper calculator. 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 Test 2 seat assignments posted on web. Test 2: emphasis will be on material covered since Test 1 (Ch. 5 – Ch. 7.6), BUT I may throw in some Redox Reaction stuff from the end of Ch. 4 since we were just finishing that before Test 1.
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Today’s Lecture: Review for Test 2, then Finish Ch. 7 thru section 7.6. Before Today’s Lecture: Read Ch. 7 thru 7.6. Nearly finish ALEKS Obj. 6 over Ch. 7.1- 7.6 (revised!), due tonight 9 PM. Test Monday! Before next Weds. lecture: Read rest of Ch. 7. Start ALEKS Obj. 7 due 9 PM Friday week after Thanksgiving, covers Ch 7.5 8.3.
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What is the pH of a 1.00 M solution of an acid which has K a = 1 x10 -6 ? 6 . 5 4. 3. 2. None of the ab. .. 0% 1. 6.0 2. 5.0 3. 4.0 4. 3.0 5. 2.0 6. None of the above
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Using K a , the Acid Dissociation Constant For the generalized reaction between a weak acid, HA(aq), and water: HA (aq) + H 2 O (l) H 3 O + (aq) + A - (aq) Eqbm. constant: K a = = 1x10 -6 = x 2 / (1.0-x) x = 1x10 -3 = [H + ] pH = 3.0 [H + ] [A - ] [HA] K =
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He Ne Ar Kr Xe Rn The Periodic Table of the Elements CrMn Fe Co Ni Mo W Tc Re Ru Os Rh Ir Pd Pt Most Probable Oxidation State +1 +2 +3 +4 +3 +_4 - 3 - 2 - 1 0 H Li Na K Rb Cs Fr Sc Y Be Mg Ca Sr Ba Ra La Ac B Al Ga In Tl Ti Rf Hf Zr C Si Ge Sn Pb F Cl Br I At O S Se Te Po N P As Sb Bi Zn Cd Hg + 2 +1 Cu Ag Au +5 V Nb Ta Ce Th Pr Nd PmSmEu Gd Tb Dy Ho Er TmYb Lu Pa U Np Pu AmCmBk Cf Es FmMd No Lr +3 +3 Db Sg Bh Hs Mt Ds
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Recognizing Oxidizing and Reducing Agents - I Problem: Identify the oxidizing and reducing agent in each of the Rx: a) Zn (s) + 2 HCl (aq) ZnCl 2 (aq) + H 2 (g) b) S 8 (s) + 12 O 2 (g) 8 SO 3 (g) c) NiO (s) + CO (g) Ni (s) + CO 2 (g) Plan: First we assign an oxidation number (O.N.) to each atom (or ion) based on the rules in Table 4.3. The reactant is the reducing agent if it contains an atom that is oxidized (O.N. increased in the reaction). The reactant is the oxidizing agent if it contains an atom that is reduced ( O.N. decreased). Solution: a) Assigning oxidation numbers: Zn (s) + 2 HCl (aq) ZnCl 2 (aq) + H 2 (g) 0 +1 -1 +2 -1 0 HCl is the oxidizing agent, and Zn is the reducing agent!
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Balancing REDOX Equations: The oxidation number method Step 1) Assign oxidation numbers to all elements in the equation. Step 2) From the changes in oxidation numbers, identify the oxidized and reduced species. Step 3) Compute the number of electrons lost in the oxidation and gained in the reduction from the oxidation number changes. Draw tie-lines between these atoms to show electron changes. Step 4) Choose coefficients for these species to make the electrons lost equal the electrons gained (or total increase in ON = total decrease in ON), remembering to first balance the numbers of atoms of those elements which change ON (red = my addition).
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C142A Exam 2 Review Ch 5-7.6 - Same rules as Test 1: Bring...

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