Chpt%2019-2

Chpt%2019-2 - Example • In a titration curve you begin...

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Titrations 19.2

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19.2 Acid-Base titrations Indicators: weak acids or bases that change color as they switch to the conjugate: HIndic  Indic- Most people use pH meters now
Titration curve Strong Acid w/ Strong Base

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Titration curves In a strong acid-strong base Equivalence point is where there is: Equal moles of the acid and base no H3O+ or OH- present (from the strong acid or base) pH = 7 End point is the end of the steep curve You can solve for the pH at any point on this curve
Titration curve Weak Acid w/ Strong Base Weak Acid Ka = 1.3 * 10- 5

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Titration curves Weak acid-strong base The equivalence point has: Equal moles of weak acid and strong base Leads to all weak acid converted to conjugate base a pH above 7 (owing to the conjugate base)

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Unformatted text preview: Example • In a titration curve you begin with 40.00 mL of 0.1000 M HF where Ka = 6.8 * 10-4 • Add 65.0 mL of 0.0500 M KOH • Solve for pH Note: Since volume keeps changing in this problem, focus on the number of moles of HF and KOH first. Convert to Molarity before using Ka Titration curves • Weak base and strong acid is similar • Equivalence point pH < 7 – Why? • Be able to: – Identify and define equivalence point – Identify whether curve represents strong or weak acids or bases (at least one of them will be strong) Polyprotic acid Polyprotics • Multiple equivalence points H2SO3 + OH- HSO3- + H2O HSO3- + OH- SO32- + H2O • But no math involved – we’re not covering polyprotics...
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This note was uploaded on 11/30/2011 for the course CHEM 1212 taught by Professor Dockery during the Fall '08 term at Kennesaw.

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Chpt%2019-2 - Example • In a titration curve you begin...

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