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1) Add 1 ml of 1 M HCl to 1 liter of pure H 2 O:

Clamping of [H 3 O + ] by a buffer solution. 1) Add 1 ml of 1 M HCl to 1 liter of pure H 2 O:. 2) Now add 1 ml of 1M HCl to one liter of solution containing 0.7 moles of HOAc and 0.6 moles of NaOAc. Remember, this is a buffer, so [HOAc]  0.7M and [OAc - ]  0.6M.

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1) Add 1 ml of 1 M HCl to 1 liter of pure H 2 O:

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  1. Clamping of [H3O+] by a buffer solution 1) Add 1 ml of 1 M HCl to 1 liter of pure H2O: 2) Now add 1 ml of 1M HCl to one liter of solution containing 0.7 moles of HOAc and 0.6 moles of NaOAc. Remember, this is a buffer, so [HOAc]  0.7M and [OAc-]  0.6M Max change in HOAc occurs if all H+ added reacts with OAc- HOAc: Reaction stoichiometry is as follows:

  2. [HOAc] = 0.701 and [OAc-] = 0.599 New [H3O+] = 2.17  10-5 “No” change in [H3O+] when buffered! If not buffered, get 104 change in H3O+ concentration!! “Physically” the H+ is being “stored” as undissociated HOAc: If add OH- also find pH does not change because the OH- reacts with HOAc to give H2O and OAc-!

  3. H2O(100mL) Add strong base to: 1) Pure water 2) 0.1 M/0.1 M Acetate buffer 3) 1.0 M/1.0M Acetate buffer 13 12 11 10 9 8 7 6 5 Unbuffered pH 0.10 M CH3COOH/0.10 M NaCH3COO (100mL) Buffered 0 10 20 30 40 Volume 0.10 M NaOH (mL) 1.0 M CH3COOH/1.0 M NaCH3COO (100mL) Buffered: small change in pH compared to unbuffered. Higher buffer concentration resists pH changes more effectively.

  4. 12 11 10 9 8 7 6 5 4 3 2 1 0 100.0 mL of 0.1000M HCl titrated with 0.1000 M NaOH. Equivalence point pH 0 50 100 At start [H3O+]=10-1 M Volume 0.1000 M NaOH (mL) Titration of a strong acid by a strong base.

  5. Titration Curve for aWeak Acid HA (red curve/points) HA + OH- H2O + A- Mix of HA and A- in buffer region Mostly HA at start

  6. Indicators Dye molecules whose color changes with pH or [H+]. Useful way to follow pH changes. HIn + H2O  H3O+ + In- (Indicators are themselves weak acids or bases.) In- yellow, HIn red In = Indicator Ratio of yellow, In- form, to red, HIn form, controlled only by [H3O+] for a given KI

  7. Bonus * Bonus * Bonus * Bonus * Bonus * Bonus

  8. Sensitivity range brackets: [In-]/[HIn] = 1 Center of pH range where indicator works best is pH = pKI Some Important Acid-Base Indicators (Skoog and West p 189, table 9-1) Indicator Sensitive pH Range Acid Color Base Color Thymolphthalein 9.3 - 10.5 colorless blue Phenolphthalein 8.0 - 9.8 colorless red-violet Methyl Yellow 2.9 - 4.4 red orange-yellow

  9. Thermodynamics (1st part) Introduction Thermodynamics is the study of energy flow for bulk matter. It is not a subject which concerns itself with the behavior of individual molecules. Thermodynamics is only valid under certain relatively restricted conditions. Most simply Thermodynamics describes equilibrium situations and change between equilibrium situations. All of Thermodynamic principles are based completely on experimental findings in the laboratory. As such it is a totally empirical science. Example: Sun rises every morning. Statement based on experience or measurement. Thermodynamics is a discipline with only 3 laws: (can only pay Paul by robbing Peter)

  10. Some Definitions : 1) System : Object or box or part of the physical universe which we want to study. 2) Surroundings: Every thing that isn't the system (i.e. the remainder of the universe) 3) Equilibrium states or more simply and sloppily just states: A situation in which a system does not change with time i.e. The bulk properties don't change. To describe the state of a system we usually need to know several things such as

  11. 4) State Functions: These are the most important quantities in Thermodynamics and also the most difficult to define. A state function is a property of a system which may have different values for different equilibrium states of the system ; Changes in values of state functions are easy to determine because the change depends only on the initial and final equilibrium states of the system.

  12. Example :Temperature is a state function Distance traveled between 2 points is not a state function. d1 Ti x Tf x d2 d1 ≠ d2 ∆T=Tf-Ti (Either path)

  13. Ideal Gas State functions: Consider 1 mole of an ideal gas PV = RT Suppose begin with: P1 = 5 atm V2 = 4.92 liters T1 = 300o K And end with: P2 = 4 atm V2 = 12.3 liters T2 = 600o K

  14. If we got to the condition 4 atm, 12.3 liters, and 600K by going as follows: 5 atm, 4.92 liters, 3004 atm, 6.15 liters, 300 4 atm, 12.3 liters, 600or by the path: 5 atm, 4.92 liters, 3005 atm, 9.84 liters, 600 4 atm, 12.3 liters, 600 Changes in state functions are independent of path. Important State Functions: Important Non State Functions: Work, Heat.

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