CH302_022211 - Neutralization Buffers Titration Principles...

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Principles of Chemistry II © Vanden Bout Neutralization Buffers Titration
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Principles of Chemistry II © Vanden Bout HA(aq) H + (aq) + A - (aq) How are we going to control this equilibrium? Add H + shift to the "reactants" Remove H + (Add OH - ) shift to the "products"
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Principles of Chemistry II © Vanden Bout Strong Acid/Strong Base (only H + and OH - ) What volume of a 0.5 M NaOH will you need to add to 200 mL of a 0.5 M solution of HCl to neutralize it? A. 100 mL B. 200 mL C. 300 mL D. 400 mL E. 500 mL
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Principles of Chemistry II © Vanden Bout What is the pH of a solution that is made of equal moles of a HF and NaOH? A. neutral (pH 7) B. acidic (pH < 7) C. basic (pH > 7)
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Principles of Chemistry II © Vanden Bout I can’t have OH - and acid I can’t have H + and base They will react Neutralization reactions H + (aq) + OH - (aq) OH - (aq) + HA(aq) OH - (aq) + BH + (aq) H + (aq) + A - (aq) H + (aq) + B(aq)
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Principles of Chemistry II © Vanden Bout What can I have at the same time in a solution? A weak acid and conjugate base HA and A - A weak base and its conjugate acid B and BH +
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Principles of Chemistry II © Vanden Bout What will have in solution if initially I have 1 mole of acetic acid and I add 0.5 mole of NaOH? A. 1 mole acetic acid and 0.5 mole OH - B. 1 mole H + and 0.5 moles OH - C. 0.5 moles H + D. 0.5 mole HA and 0.5 moles of A - E. 1 mole of Ha and 0.5 moles of A- OH - (aq) + HA(aq) A - (aq) 0.5 moles + 1 mole 0 moles neutralize
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This note was uploaded on 03/27/2011 for the course CHEM 302 taught by Professor Mccord during the Spring '10 term at University of Texas at Austin.

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CH302_022211 - Neutralization Buffers Titration Principles...

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