acids_and_bases_L2_Spring2008

Acids_and_bases_L2_S - Room Assignments for Exam 2 Thursday March 27 8:30 10:00 PM Solar ID 000000000 105893402 105893403 106067703 106067704

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1 Engineering 145 106323691 106474392 Javits 109 106474393 999999999 Harriman Hall 137 106241820 106287741 Engineering 143 106287742 106323690 Javits 102 106176862 106209479 Javits 110 106209480 106241819 Old Chemistry 116 106143846 106176861 Earth & Space Science 001 106067704 106143845 Javits 100 Balcony 105893403 106067703 Javits 100 Main Floor 000000000 – 105893402 Room Solar ID Room Assignments for Exam 2 Thursday, March 27, 8:30 – 10:00 PM On material covered from Monday, Feb. 18 through Friday, Mar. 14 On material covered from Monday, Feb. 18 through Friday, Mar. 14 . 2 Room Assignments are posted on Blackboard. Be sure to bring the following: • Stony Brook ID card • 2 or more #2 pencils and a good eraser • Calculator with extra batteries Do NOT bring any of the following: • Cell phones, beepers, iPods, or other communication devices. • Textbook, notes, or any aids to taking the exam. • All personal belongings must be placed under your seat not on the seat next to you. Note there is an error on the cover page •pH = pK a + log ([base]/[acid]) not ln No one will be permitted to leave the exam before 9:15 PM No one will be permitted to leave the exam before 9:15 PM . Exam 2, Thursday, March 27, 8:30 – 10:00 PM
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3 What is the pH of a buffer solution prepared from .24 M NH 3 and 0.2 M NH 4 Cl ? What is its pH if 0.005 mol NaOH is added to 0.5 L of this buffer ? K b for NH 3 is 1.8 x 10 -5 . 42 3 Init 0.2 M .24 M : 0.01 M Change: -0.01 M -0.01 M +0.01 M NH OH H O NH Add +− ++ ZZX YZZ () 5 0.19 0.00 M 0.25 M [ A c i d ] 0 . 1 9 pOH p log log 1.8 10 log 4.62 [Weak Base] 0.25 14.00 pOH = 14.00 - 4.62 = 9.38 b After M conj K pH =+ = × + = =− 5 4 3 [] 0.2 p log log 1.8 10 log 4.66 [NH ] 0.24 14.00 pOH = 14.00 - 4.66 = 9.34 b NH K pH + = × + = 0.005 0.01 0.5 mol M V == = Add base 4 Acid Acid -Base Titrations Base Titrations Titration is a commonly used technique for Titration is a commonly used technique for conducting a neutralization. conducting a neutralization. Objective Determination of the Equivalence Point (The point at which acid and base are in stoichiometric proportions) Color change of indicators typically used to locate the equivalence point.
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5 Auto Auto -Titrator Titrator 7 pH 6 Indicators Indicators pH Indicators are chemicals which change color when they are put into acids or alkalis.
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This note was uploaded on 04/28/2008 for the course CHEM 132 taught by Professor Laceyandhanson during the Spring '08 term at SUNY Stony Brook.

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Acids_and_bases_L2_S - Room Assignments for Exam 2 Thursday March 27 8:30 10:00 PM Solar ID 000000000 105893402 105893403 106067703 106067704

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