1. Acids & Bases pH Balance?

2. Video: Elements of Chemistry - Acids, Bases & Salts

3. Household Acids & Bases Lab Solution Blue litmus Red litmus Universal Indicator pH Vinegar Ammonia Put drop onto plate. Unplug pH probe Lemon juice Add drop of indicator. When done. Soft drink Record. Drain cleaner Rinse out plate at end Detergent of period please Baking soda Antacid (MoM)

4. Mentos & Pop http://www.stevespanglerscience.com/exp eriment/00000109 http://www.stevespanglerscience.com/exp eriment/00000109

5. Properties of Acids vs Bases Acids: Taste Sour – vinegar! Feel like water but sting cuts. Turn litmus red. React with active metals to form explosive H 2 gas. Act as electrolytes to conduct electricity. Neutralize bases! Bases: Taste bitter – soap! Feel slippery. Turn litmus blue. Don’t react with most metals. Act as electrolytes to conduct electricity. Neutralize acids!

6. Arrhenius Acids & Bases Acids: Release H + ions by dissociation. Release H + ions by dissociation. Example: HCl Example: HCl Combine H + with any negative ion on your ion chart to form an acid. Combine H + with any negative ion on your ion chart to form an acid. Examples: ??? Examples: ??? Bases: Release OH - ions by dissociation. Example: NaOH Combine OH - with any metal on the periodic table to form a base. Examples: ???

7. Arrhenius Explanations H+ provides the sour taste & stings. H+ provides the sour taste & stings. OH- the bitter taste & is slippery. OH- the bitter taste & is slippery. Dissociation of both acids & bases produces dissolved ions which act as electrolytes. Dissociation of both acids & bases produces dissolved ions which act as electrolytes. Neutralization occurs when H+ & OH- combine to form H2O. The left overs produce a salt like NaCl. Neutralization occurs when H+ & OH- combine to form H2O. The left overs produce a salt like NaCl.

8. Bronsted-Lowry Acids & Bases Acids: Donate H+ ions. Donate H+ ions. Example: Acetic acid & amino acids. Example: Acetic acid & amino acids. H+ ions are protons. H+ ions are protons. Acids may be monoprotic, diprotic or triprotic. Acids may be monoprotic, diprotic or triprotic. Examples: Examples: Bases: Accept H+ ions. Example: Ammonia, NH 3 All inclusive including bases ignored by Arrhenius.

9. Conjugate Acids & Bases Acids release H+ & bases accept H+. Once an acid releases its H+ it becomes a base that can accept H+ & vice versa. Examples: H 2 CO 3 vs HCO 3 -1 NH 3 vs NH 4 +1 H 2 O vs H 3 O +1

10. Hydronium Ion Water is amphoteric – it can act as both an acid & a base. Water is amphoteric – it can act as both an acid & a base. When water acts as a base, it forms the hydronium ion. When water acts as a base, it forms the hydronium ion. H 2 O + H +  H 3 O + H 2 O + H +  H 3 O + H+ ions always bind to something. H+ ions always bind to something. When water acts as an acid it forms OH-. When water acts as an acid it forms OH-. H 2 0  OH - + H + H 2 0  OH - + H + The fraction of water that normally dissociates is 10 -7 M. A very small fraction! 1/10million! The fraction of water that normally dissociates is 10 -7 M. A very small fraction! 1/10million!

11. pH Measures the H+ Concentration pH uses logs which are just powers of 10. pH uses logs which are just powers of 10. pH measures the electric “potential” of H+ ions in a solution. pH measures the electric “potential” of H+ ions in a solution. pH is calculated as the negative “power” of 10 of the H+ ion concentration. pH is calculated as the negative “power” of 10 of the H+ ion concentration. The equation for pH is pH = -log[H+] The equation for pH is pH = -log[H+] [brackets] mean concentration in Molarity. [brackets] mean concentration in Molarity. pH 7 is neutral, above 7 is basic & below 7 is acidic. pH 7 is neutral, above 7 is basic & below 7 is acidic.

12. Simple pH Calculations Acid3.3 10 -3.3.00047 Base12 10 -12.000000000001 Base9 10 -9.000000001 neutral7 10 -7.0000001 Acid5 10 -5.00001 Acid3 10 -3.001 Acid or Base? pH Power of 10 H + Molarity

13. pH Quiz – Determine the pH of: 1. A 4.63 x 10 -8 M solution of HNO3. 2. A 250L solution containing 4.3mol of HCl. 3. A 750.0ml solution containing 0.0046g of HBr. 4. A 8.9L solution of 0.65mol of H2SO4.

14. Titrations 5/13/08 Simulations Simulations http://www.sciencegeek.net/Shockwave/Titratio n.htm http://www.sciencegeek.net/Shockwave/Titratio n.htm http://www.sciencegeek.net/Shockwave/Titratio n.htm http://www.sciencegeek.net/Shockwave/Titratio n.htm Lesson: Lesson: Simulation Demo Simulation Demo Notes Notes Practice Problems Practice Problems Work Problems Work Problems Asmt: Simulation Problems A-E find [H+] in M Asmt: Simulation Problems A-E find [H+] in M

15. Titrations Titrations measure the concentration of solutions by finding out the amount of a known solution needed to neutralize an unknown solution. Titrations measure the concentration of solutions by finding out the amount of a known solution needed to neutralize an unknown solution. Neutralization occurs when Mol H+ = Mol of OH- Neutralization occurs when Mol H+ = Mol of OH- M = mol/L M = mol/L mol = L x M mol = L x M mol = M x V mol = M x V M a V a = M b V b (a is for acid, b is for base) M a V a = M b V b (a is for acid, b is for base) Some acids are diprotic or triprotic, some bases are multi-hydroxy. Some acids are diprotic or triprotic, some bases are multi-hydroxy. AM a V a = BM b V b AM a V a = BM b V b (A is for # of H+, B is for # of OH-) (A is for # of H+, B is for # of OH-)

16. Friday 6-11-04 Prep: 1. Litmus papers, droppers fill up bottles. 2. Graduation Rehearsal Class 1. End of Year Schedule 2. Vocabulary Assignment 3. Lab – pH of Household Substances Predictions Predictions Handling the pH probe & storage bottle Handling the pH probe & storage bottle Litmus tests & universal indicator Litmus tests & universal indicator

17. Acid – Base Vocabulary AcidBaseIndicatorNeutralization Hydronium ion Amphoteric Conjugate acid Conjugate base Dissociation pH Buffer Titration Equivalence point

18. pH of Household Substances Sample Predict pH Red Litmus Blue Litmus Univ. Indic- ator pHActual

19. pH of Household Substances 1. Make the following data table in your notebook. 2. Rank & predict pH of samples to be used: soda pop, drain cleaner, vinegar, ammonia, lemon juice, detergent, baking soda 3. ½ fill a well in the plate for each sample. 4. Test with red litmus, blue litmus & then add 1 drop of universal indicator to observe the color. Dispose down sink. 5. pH Probe: Cap stays on probe. Place storage bottle by faucet. Cap stays on probe. Place storage bottle by faucet. Rinse probe with distilled water before each test. Rinse probe with distilled water before each test. Place probe in each sample bottle. Place probe in each sample bottle. Swirl sample around probe for 30 seconds. Swirl sample around probe for 30 seconds. Record pH from top right corner of calculator. Record pH from top right corner of calculator. Recap all bottles when not in use. Recap all bottles when not in use.

20. Monday 6/14/04 Prep: 1. Get copies of tracking hurricanes for 14 juniors. 2. Update Chemistry Aces 3. Prepare for Rainbow Titrations Lab Class: Recollect Final Answers from 5 th Period 1. Schedule of Week 2. Due: Acids & Bases Vocabulary 3. Review Household Acids & Bases 4. Notes: Acids & Bases (10 points) 1. Properties 2. Definitions 3. pH

21. Tuesday 6/15/04 Prep: 1. Print 40 copies of the Final Keys 2. Distribute supplies for Rainbow Titration Lab (test burets & stopcocks) Class: 1. Pass out Final Exams – check keys & addition of scores. RECOLLECT! 2. Rainbow Titration Lab

22. Rainbow Titration Lab Goal: Determine all the distinct colors and their corresponding pH ranges for Universal Indicator. Procedures for Each Trial: 1. Add 25 ml of 0.1M HCl to a 100ml beaker. Add 6 drops of Universal. (Person A) 2. Close the stopcock on the buret. Add 50 ml of 0.1M NaOH to the buret. (Person B) 3. Place the magnetic stir bar in the beaker of liquid & turn it on a medium spin. (Person C) 4. Set up the pH probe to monitor the liquid in the beaker. (Person D) 5. Open the stopcock to SLOWLY drip base from the buret to the acid in the beaker. (Person B) 6. Record your observations of colors & pH. (Everyone) 7. Check your results with the instructor. (Everyone)

23. Monday 6/20/05 DMA: Copy 3 titration problems 1. Finish pH notes 2. Titration Notes 3. Demo: Titrate ?M H2SO4 w/ 2M NaOH Asmt: 3 titration problems

24. Titration Problems 1. If 20.00ml of acidic drain cleaner is titrated completely by 18.02ml of 0.100M NaOH, what is the acid’s concentration? 2. A 25.1ml volume of KOH is titrated with 43.2ml of 0.150M H 2 SO 4. What is the molarity of the KOH? 3. A volume of 34.0ml of 0.100M H 3 PO 4 neutralizes 25.0ml of Ba(OH) 2. What is the concentration of the barium hydroxide?

25. Tuesday 6/21/05 Prep: 1. Get copies of Acid-Base Mini-Exam 2. Make fine cards! Class: 1. Pass out AP Bio stuff. 2. Review a titration problem. 3. Acid-Base Mini-Exam 4. Pass back finals / fine cards / check basmati/ sign annuals. Plan: 1. Fill out fine cards! 2. Call Mary Anne about visiting Bob. After School: 1. Help students. 2. Clean up lab.

26. Vinegar Titration Lab Add 10.0 ml of vinegar to the beaker. Add 4 drops of indicator B, phenolpthalein. Add 10.0 ml of vinegar to the beaker. Add 4 drops of indicator B, phenolpthalein. Fill the buret with 1.00M NaOH. Record the starting volume. Fill the buret with 1.00M NaOH. Record the starting volume. Titrate until the mixture turns pink & stays pink. Use the minimum of drops. Titrate until the mixture turns pink & stays pink. Use the minimum of drops. Measure the final volume and determine the change in volume of the base. Measure the final volume and determine the change in volume of the base. Use AMaVa = BMbVb to determine the molarity of the vinegar, HC2H3O2. Use AMaVa = BMbVb to determine the molarity of the vinegar, HC2H3O2.

27. Antacid Titration Lab Goal: Determine which Antacid will neutralize the greatest amount of stomach acid – Rolaids, Tums, or Maalox 1. Pulverize a sample tablet with the mortar & pestle. 2. Dissolve sample with 25ml of distilled water & transfer the solution to a 100ml beaker. 3. Add 4 drops of bromothymol blue? and the stir bar. 4. Add 0.1M HCl to the buret. Record precisely the starting volume in the buret. 5. Use the minimum amount of 1.0M HCl needed to turn the solution yellow? and stay clear. 6. Record the final volume of the buret. Find the change in volume. 7. Repeat for each sample.

28. Friday 6/18/04 Prep: 1. Set up titration demo. 2. Get extra fine cards. Class: 1. Return book or receive fine card tied to grade report. 2. Check Basmati – bring personal issues to me after mini-exam. 3. Begin titration demo (5ml vs 50ml) 4. Review for mini-exam, no 3x5 card 5. Acids & Bases Mini-Exam – Check notes??? XC Asmt: 5 points if you bring treats for everyone for Monday’s Annual Signing Party

29. Conjugate Acids & Bases Any acid that can release H+ can re-accept and bind it to varying degrees. Any acid that can release H+ can re-accept and bind it to varying degrees. Strong acids like HCl release essentially all H+ ions. HCl  H + + Cl - Strong acids like HCl release essentially all H+ ions. HCl  H + + Cl - Weak acids like in vinegar release a small percentage of H+ ions. Most remain bound. Weak acids like in vinegar release a small percentage of H+ ions. Most remain bound. HC 2 H 3 O 2  H + + C 2 H 3 O 2 - HC 2 H 3 O 2  H + + C 2 H 3 O 2 - Salts contain positive & negative ions. Salts contain positive & negative ions. Any negative ion has some capacity to bind with H+ ions to act like a base. Examples: ??? Any negative ion has some capacity to bind with H+ ions to act like a base. Examples: ??? Conjugates represent examples with or without H+ attached. Examples: ??? Conjugates represent examples with or without H+ attached. Examples: ???

30. Equilibrium of Reversible Reactions Carbonated Water: CO 2(g) + H 2 O (l)  H 2 CO 3(aq) H 2 CO 3(aq)  H + (aq) + HCO 3 - (aq) Le Chatelier’s Principal – When disturbed a reaction will adjust to minimize the disturbance. (Teeter totter analogy) Carbonate pop by adding CO 2(g) pressure. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Pop goes flat when container is opened! CO 2(g) + H 2 O (l)  H 2 CO 3(aq)

31. Equilibrium Ratios xA (aq) +yB (aq)  zC (aq) Equilibrium Ratio (K) = products/reactants K eq = [C] z / [A] x [B] y Coefficients = exponents! Carbonated Water Equilibrium Ratio? Each reaction has a different equilibrium ratio value. Large ratios favor the _________, while small ratios favor the _________.