3. 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 Final 100 ???

4. 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 Properties of Acids or bases General Chemistry Proton Donors And Acceptors pH Titrations

5. What color would a solution of oxalic acid turn blue litmus paper?

6. Red

7. You are given a solution that is conductive is this solution acidic or basic?

8. The solution is both acidic and basic because they both are electrolytic

9. Identify and correct the one false statement listed below. A.) Acids turn blue litmus paper red B.) Bases are electrolytes C.) Acids feel slippery when they are diluted D.) Acids and bases are corrosive

10. C.) Acids feel slippery when they are diluted Correction: Bases feel slippery when they are diluted

11. Acids and bases have different tastes to them. What are these tastes respectively?

12. Sour and bitter

13. Some properties of acids and bases 1.Turns litmus paper red 2. Turns litmus paper blue 3.pH less than 7 4. pH greater than 7 5. bitter taste 6. sour taste 7. electrolyte 8. neutralized by bases 9. Feels Slippery The properties from the list above that could be applied to describe a base are…

14. 2,4,5,7,9

15. In a solution the substance whose bonds are broken by a solvent are called what?

16. Solute

17. What is NH 3

18. Ammonia

19. DAILY DOUBLE

20. A student tested a solution with the indicators bromothymol blue, phenol red and phenolphthalein. Bromothymol blue turned blue, phenol red turned red and phenolphthalein turned colorless. What is the pH range of this unknown solution?

21. 8.0-8.2

22. Match the column on the left with its corresponding partner on the right. Neutral, Ionic CompoundHCl(aq) Neutral, Molecular CompoundNaOH (aq) Strong AcidKCl(s) Strong BaseH2CO3 (aq) Weak AcidC6H12O6

23. Ionic CompoundKCl (s) Molecular Compound C6H12O6 Strong AcidHCl (aq) Strong BaseNaOH (aq) Weak AcidH2CO3(aq)

24. What are two major differences between ionic and molecular compounds?

25. Ionic compounds are a metal and non-metal, while molecular compounds are just non-metals. Ionic compounds are bonded through the transfer of electrons, while molecular compounds form covalent bonds by sharing electrons. Ionic compounds form when positive and negative ions are attracted to each other whereas molecular compounds do not have ions. Ionic compounds will conduct electricity where as molecular compounds do not Water will dissolve most ionic crystals because of the positive and negative charges whereas molecular compounds do not always dissolve

26. A proton donor and a proton acceptor are terms that redefine ________ and ________ based on the way the act in solution rather then empirical evidence.

27. Acids and bases

28. A proton acceptor connects to its what?

29. It connects to its conjugate acid because a proton acceptor is a base.

30. If dissolved oxalic acid reacts with water draw out the reaction and label the proton donors, proton acceptors, conjugate acid and conjugate base.

31. HOOCCOOH(aq) +H20(l)  HOOCCO-(aq) + H30+(aq) Proton donors (acid): HOOCCOOH and H30+ Proton acceptors (base): H20(l) and HOOCCO- Conjugate base: HOOCCO- (aq) Conjugate acid: H3O+(aq)

32. HNO2(g)+ H2O(l)  H3O+(aq)+NO2 (aq) In the chemical reaction above the proton donors are?

33. HNO2(g) and H30+(aq)

34. Write the chemical equation for the reaction between the following substances. Label the proton donors, proton acceptors, conjugate acid and conjugate base. Phosphoric acid and ammonia

35. H3PO4(aq) + NH3(aq)  H2PO4- (aq)+ NH4+ (aq) Proton Donor: H3PO4(aq) and NH4+ Proton Acceptor: H2PO4- (aq) and NH3(aq)

36. What does pH represent?

37. Power of Hydrogen pH is the concentration of hydronium ions

38. If you are given a solution that has a pH of 3 and a solution that has a pH pf 9 how many times more basic is the solution with the pH of 9.

39. 1 000 000

40. Calculate the pH of river water that has a hydronium ion concentration of 2.73x10-7 mol/L. Answer must have correct significant digits.

41. 5.564

42. Calculate the hydronium ion concentration of a bottle of hand lotion that has a pH of 4.673

43. 2.12 x 10-5

44. The pH of an unknown solution is 9.90 meaning it is ______. During a Science 30 experiment the solution is changed. At the end of the experiment it has a pH of 3.90 meaning it is ______. The hydronium concentration has ______by a factor of _____.

45. Basic, Acidic, increased, 1 000 000

46. A question is asking you to solve for the volume of a solution. What does the rearranged version of the concentration formula look like to solve for volume?

47. v= n/c

48. Calculate the concentration of a solution that contains 195mL of solution and is made up of 2.69 mol of methanoic acid.

49. 13.79 mol/L

50. Draw and label a proper titration. (There should be 8 things labelled on your drawing.)

51. Burette, ring stand, clamp, stopcock, erlenmeyer flask, acid of unknown concentration, base of known concentration, indicator

52. What is happening at the molecular level at the start of a titration, at neutralization and after neutralization.

53. At the start of a titration there is all hydronium in the erlenmeyer flask. As more base is added to the acid the two bond together and neutralize. At the neutralization point is where the titration will change color. After neutralization if you continue to add base the solution will become basic.

54. You are given the following data for a titration performed in a lab. Find the unknown concentration Base: 2.79 mol/L Volume of acid used in each titration: 15.0 mL Average amount of base added: 6.14 mL TrialFinalInitialAddedColor 17.890.007.89Dark Pink 214.007.896.11Light Pink 320.1014.006.10Light Pink 426.3020.106.20Light Pink

55. 1.142 mol/L

57. You are given the titration data below. Find the unknown concentration. Concentration of base = 1.56 mol/L Amount of Acid = 25 mL Final Volume of NaOHInitial Volume NaOH 13.980.00 26.1713.98 38.5726.17 51.238.57

59. The concentration of the acid is 0.774 mol/L