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Applications of aqueous equilibria

Applications of aqueous equilibria. Common ion effect Henderson-Hasselbalch Equation Buffer capacity Indicators Solubility Product Carol Brown Saint Mary’s Hall. Buffers/Common Ion Effect.

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Applications of aqueous equilibria

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  1. Applications of aqueous equilibria Common ion effect Henderson-Hasselbalch Equation Buffer capacity Indicators Solubility Product Carol Brown Saint Mary’s Hall

  2. Buffers/Common Ion Effect • A buffered solution contains 0.25 M NH3 (Kb= 1.8 x 10-5) and 0.40 M NH4Cl. Calculate the pH of the solution. • pH=9.05

  3. Henderson-Hasselbalch Equation

  4. Using Henderson-Hasselbalch • A buffered solution contains 0.25 M NH3 (Kb= 1.8 x 10-5) and 0.40 M NH4Cl. Calculate the pH of the solution.

  5. Buffer Capacity • 1. Calculate the pH of a solution which contains 0.50 M HOAc and 0.50 M OAc-. • 2. Calculate the pH of a solution which contains 0.10 M HOAc and 0.10 M OAc-. • Which has the greater buffer capacity?

  6. Indicators • Weak acids or bases that exhibit one color when the proton is attached to the molecule and another color when the proton is absent. • HIn <==> H+ + In- • Oxford University Indicatorshttp://www.chem.ox.ac.uk/vrchemistry/chapter16/Pag30.htm

  7. Indicator Color Change • For most indicators, about a tenth of the initial form must be converted for the human eye to detect a color change.

  8. Solubility Product • Copper(I) Bromide has a measured solubility of 2.0 x 10-4 mol/L. Calculate the Ksp.

  9. Calculating the molar solubility from the Ksp • The Ksp value for copper(II) iodate is 1.4 x 10-7. Calculate its solubility.

  10. Common Ion Effect • Calculate the solubility of solid CaF2 (Ksp= 4.0 x 10-11) in a 0.025 M NaF solution.

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