Chpt%2019-2

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

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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
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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
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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 were not covering polyprotics...
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Chpt%2019-2 - Example In a titration curve you begin with...

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