2. What is the volume of one mole of a gas at STP?

3. Identify the pH associated with acids and bases.

6. Give two ways that acids are different from bases that does not include their pH.

7. 1.pH < 7.0 2.Electrolytes 3.Taste Sour 4.React with bases to form H 2 O + Salt 5.React with metals to form H 2(g) and salt Table J

8. 1.pH > 7.0 2.Electrolytes 3.Taste Bitter 4.React with acids to form H 2 O + Salt 5.Slippery, soapy feeling

9. Arrhenius  gives off an H + and forms H 3 O + - increases the H+ when dissolved in water Bronsted  proton [H + ] donor (loses an H + ) HCl  H + + H 2 O  H + + Cl - H3O+H3O+

10. Arrhenius  gives off an OH - Bronsted  proton [H + ] acceptor (gains an H + ) NaOH  Ca(OH) 2  Na + + OH - Ca +2 + OH - 2

11. Chemicals which change colors when they are put into acids or bases. These indicators change colors in response the [H + ]. Table M

13. If you were to place H 2 SO 4 onto a piece of copper, would it react to produce hydrogen gas? Explain your answer.

14. M A V A = M B V B -Perform titrations to determine an unknown volume or concentration of an acid/base -ENDPOINT = when indicator changes color -Moles of H + = Moles of OH - - Products are always water and salt M A = molarity of acid V A = volume of acid M B = molarity of base V B = volume of base

15. M A V A = M B V B If 20.0ml of a 0.50M HCl solution is needed to neutralize 65.0ml of a NaOH solution. What was the concentration of the base? M A = molarity of acid V A = volume of acid M B = molarity of base V B = volume of base (0.5M)(20.0ml) = M B (65.0ml) M B = 0.154M

16. M A V A = M B V B 43.0ml of HCl was titrated with 32.0 ml of 0.100 M NaOH. What is the molarity of the hydrochloric acid solution? M A = molarity of acid V A = volume of acid M B = molarity of base V B = volume of base M A (43.0ml)=(0.100M)(32.0ml) M A = 0.0744 M

18. Conjugate Pairs

19. HCl + KOH  HOH + KCl acidbaseconj. acidconj. base Na 2 CO 3 + 2HCl baseacidconj. acidconj. base conj. acid acid base Strong acids have weak conjugate bases Weak acids have strong conjugate bases H 2 O + H 2 SO 4  H 2 CO 3 + 2NaCl  HSO 4 - + H 3 O +

20. Identify the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs: acidbase conjugate acidconjugate base HC 2 H 3 O 2 (aq) + H 2 O (l)  C 2 H 3 O 2 – (aq) + H 3 O + (aq) conjugate acid-base pairs acid base conjugate acidconjugate base OH – (aq) + HCO 3 – (aq)  CO 3 2– (aq) + H 2 O (l) conjugate acid-base pairs

21. Information related to an experiment is listed below: H 2 SO 4 + 2KOH  K 2 SO 4 + 2H 2 O Results Volume H 2 SO 4 used12.0 ml Concentration H 2 SO 4 ? Volume KOH used36.0 ml Concentration KOH0.16 M Based on the above results, what is the concentration of H 2 SO 4 ?

22. Setup for titrating an acid with a base

25. M A V A = M B V B Calculate the molarity of an acetic acid solution if 34.57 mL of this solution are needed to neutralize 2.519 cL of 0.1025 M sodium hydroxide M A = molarity of acid V A = volume of acid M B = molarity of base V B = volume of base (M A )(34.57ml) = (0.1025M)(25.19ml) M A = 0.07469M

26. Trial 1Trial 2Trial 3Avg Final Acid Volume Initial Acid Volume Final Base Volume Initial Base Volume Volume of Acid Used Volume of Base Used

27. What are electrolytes? Give two examples.

28. 46) 25 mL 47)3000 mL 48)20 mL 49)50.0 mL 50)6.0 M 51)0.60 M 52)400 mL 53)1.0 M 54)SKIP 55) H Cl 56) H O H H + 57) O H -

29. pH of Common Substances

30. pH = -log[H + ] If [H+] = 1 x 10 -4, then pH = -a way to measure the concentration of H + ions (H 3 O + ) in a solution -concentration of H + = [H + ] 4 If [H+] = 1 x 10 -13, then pH =13 If [H 3 O + ] = 1 x 10 -7, then pH =7

31. What is the pH of a 0.00001 molar HCl solution? If the pH of your pool is 6, what is the concentration of hydronium ions in solution? As the pH of a solution is changed from 3 to 6, how does the concentration of hydronium ions change? An aqueous solution that a [H + ] of 1.0 x 10 -8 mole per liter has a pH of?

32. Because it is a logarithmic scale, each one unit change in pH really represents a 10 fold change in [H + ] So going from a pH of 6 to 7 really represents a 10 fold decrease in the number of [H + ] What is the difference in [H + ] in a pool that has a pH of 6, but in reality you want it to have a pH of 7?

33. If [OH] = 10 -8 M, what is the pH? [H + ][OH - ] = 10 -14 pH + pOH = 14 Solution: the OH = 8, so the pH must be 14 – 8 So the pH = 6

36. Solution A has a pH of 1 and solution Z has a pH of 5. How many times greater is the hydronium ion concentration in solution A?

39. -A compound that does not allow the pH to change even if an acid or base is added to the system -They have the ability to absorb/release H+ which will keep the pH relatively constant -Good buffers are amphiprotic substances -Amphiprotic – something that can act as an acid and a base

40. -Blood pH -Adirondack lakes Brooktrout Lake "Treat the earth well: it was not given to you by your parents, it was loaned to you by your children. We do not inherit the Earth from our Ancestors, we borrow it from our Children."

41. Effects of Acid Rain on Marble (marble is calcium carbonate) George Washington: BEFORE acid rain George Washington: AFTER acid rain

43. The pH of a lake is 8.0. Over a 10 year period, the pH of the water becomes 1000x more acidic. 1.Name an ion that has increased in the water over the 10 years? 2.What is the pH now? 3.If you were to use bromothymol blue to test the pH, what color would it be? [Use R.T.]

45. 1. H 2 O + H 2 O  H 3 O + + OH - 2. H 2 SO 4 + OH -  HSO 4 - + H 2 O 3. HSO 4 - + H 2 O  SO 4 -2 + H 3 O + 4. OH - + H 3 O +  H 2 O + H 2 O 5. NH 3 + H 2 O  NH 4 + + OH -

46. ACIDBASEEQUATION 1 H 2 SO 4 HSO 4 - 2 H 3 PO 4 3 F-F- 4 NO 3 - 5 H 2 PO 4 - 6 H2OH2O 7 SO 4 -2 8 HPO 4 -2 9 NH 4 + 10 H2OH2O H 2 PO 4 - HF HNO 3 HPO 4 -2 OH - HSO 4 - PO 4 -3 NH 3 H3O+H3O+ H 3 PO 4 ↔ H + + H 2 PO 4 - HF ↔ H + + F - HNO 3 ↔ H + + NO 3 - H 2 PO 4 - ↔ H + + HPO 4 -2 H 2 O ↔ H + + OH - HSO 4 - ↔ H + + SO 4 -2 HPO 4 -2 ↔ H + + PO 4 -3 NH 4 +4 ↔ H + + NH 3 H 3 O + ↔ H + + H 2 O

47. PART C 26.A, C, D 27.D 28.Presence of H + ions 29.C 30.C 31.(10.01mL)(0.100M)= MB(5.01ml) 0.200 M 32. 7 33. Colorless to pink. 34. 0.21 M 35. 0.97 M 36. Reduces error, increases reliability 37. Ca(OH) 2 + H 2 SO 4  CaSO 4 + 2H 2 O 38. pH= 6.0 39. 0.33 M 40. HCl – 9.50 ml NaOH – 3.80 ml 41. 0.25 mL 42. Methyl orange, brom blue, thymol blue 43. Between 4.4 and 5.5 44. Yellow

48. PART A 1.1 2.3 3.2 4.4 5.2 6.3 7.1 8.2 9.1 10.4 11.2 PART B 12.4 13.3 14.4 15.3 16.1 17.1 18.1 19.4 20.2 21.1 22.3 23.1 24.2 25.4

49. In a lab there were three flasks, one filled with methanol, another had NaOH, and the third HCl. ID these liquids. Test Test Results Bottle ABottle BBottle C Methyl orange Yellow Bromthymol Blue BlueGreenYellow Conductivity ConductorNonconductorconductor Reaction with Mg No Rxn Rxn 1.A student concluded that bottle C contained HCl. Identify one way that supports this finding. 2.Explain in terms of pH, why methyl orange was the same for all three liquids.

50. What is the volume of 1.00 mole of any gas at STP? Hint: Lab