Lecture_38_120811 - Lecture 38: Buffers Goals: Describe the...

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Lecture 38: Buffers Goals: Describe the role of buffers in maintaining the pH of a solution. Outline (Timberlake 10.6-10.7): ± Acid-Base Properties of Salt Solutions (10.6) ± Buffers (10.7) Problems for Extra Practice: 10.63, 10.65, 10.67, 10.69, 10.75, 10.77, 10.81, 10.83, 10.85, 10.87, 10.89, 10.91, 10.93, 10.95, 10.97, 10.99, 10.101, 10.103, 10.105, 10.107, 10.109, 10.111
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Acid–Base Titration Titration • is a laboratory procedure used to determine the molarity of an acid • uses a base such as NaOH to neutralize a measured volume of an acid Base (NaOH) Acid solution
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Indicator An indicator • is added to the acid in the flask • causes the solution to change color when the acid is neutralized
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End Point of Titration At the end point , • the indicator has a permanent color • the volume of the base used to reach the end point is measured • the molarity of the acid is calculated using the neutralization equation for the reaction
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Guide to Calculating Molarity
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Calculating Molarity from a Titration with a Base What is the molarity of an HCl solution if 18.5 mL of a 0.225 M NaOH are required to neutralize 10.0 mL HCl? HCl( aq ) + NaOH( aq ) NaCl( aq ) + H 2 O( l ) – Step 1: Given: 18.5 mL (0.0185 L) of 0.225 M NaOH 10.0 mL of NaOH Need: M of HCl – Step 2: Plan: L NaOH b moles NaOH b moles HCl b M HCl – Step 3: State equalities and conversion factors: 1 L of NaOH = 0.225 mole of NaOH 1 mole of NaOH = 1 mole of HCl – Step 4: Set up the problem to calculate moles of HCl:
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Calculate the mL of 2.00 M H
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This note was uploaded on 01/18/2012 for the course CHEM 120A taught by Professor Leahmiller during the Fall '11 term at University of Washington.

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Lecture_38_120811 - Lecture 38: Buffers Goals: Describe the...

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