Nature of Acids and BasesCatherine Lozier04/09/2013Chem 1310 Section C02TA Ryan BucherLab Partners:Chelsey Arnold Sunya MorinTran GHonor Pledge: I did not copy this work from any others student(s), current students in lab or old lab reports ________________________________________________SignatureDATA AND OBSERVATIONSProduct/CompoundpH pOH [H3O+] [OH-] Acidic/BasicIngredientsLemon juice 1 13 10-1 M 10-13 M AcidicToilet Bowl Cleaner 1 13 10-110-13AcidicSoda 3 11 10-310-11AcidicBeer 4 10 10-410-10AcidicShampoo 5 9 10-510-9AcidicMouthwash 5 9 10-510-9AcidicTobacco 8 6 10-810-6BasicBleach 8 6 10-810-6BasicWindex 9 5 10-910-5Basic1% baking soda 9 5 10-910-5BasicClear Ammonia 11 3 10-1110-3BasicCompounds 0.1 M 0.01 M 0.001 MAcids pH [H3O+] pH [H3O+] pH [H3O+] HCl 1.12 10-1.121.98 10-1.983.42 10-3.42Acetic Acid 2.88 10-2.883.49 10-3.494.25 10-4.25Bases pOH [OH-] pOH [OH-] pOH [OH-]NaOH 1.5 10-1.51.93 10-1.933.35 10-3.35NH4OH 3.0 10-33.88 10-3.884.92 10-4.92Percent DissociationCompounds 0.1 M 0.01 M 0.001 MAcetic Acid 1.32% 3.24% 5.62%NH4OH 1.00% 1.32% 1.20%Weak Acid Indicator Color Change pH of Color ChangePhenolphthalein Clear  pink 1.69  9.07Bromocresol Blue  lime green 6.83  10.02SAMPLE CALCULATIONS1. % dissociation = 100*[H3O+]/[acetic acid]=100*10-2.88/0.1=1.32%DISCUSSIONThe purpose of the experiment was to use various methods to determine the pH of various acids and bases. For Part A, the most acidic substances were lemon juice and toilet bowl cleaner, both with pH 1. The most basic substance was ammonia, with a pH of 11. Any error in the pH measurements of part A are likely due to the fact that the readings were taken using pH paper, the color of which must beinterpreted by the observer. Similar colors or in-between readings could have been misidentified. The pH of all acidic compounds in Part B increased as they became more diluted, and the pOH of all basic compounds increased with dilution. Percentage of dissociation increased with dilution for acetic acid and between the 0.1 M and 0.01 M concentrations of ammonium hydroxide, but decreased 0.12 percentage points between the 0.01 M and 0.001 M concentrations of ammonium hydroxide. This is likely due to human error in measurement for the dilution process. Both reactions in Part C showed distinct changes in color and pH. The phenolphthalein reaction changed from clear to pink, and had a pH change of 7.38. Thebromocresol reaction changed color from blue to bright green, and increased pH by 3.19. Part C was also probably influenced by human error in measurement, although the degree of change in color and pH weregreat enough that small measurement errors were likely insignificant.DISCUSSION QUESTIONS1. The acetic acid was a weak acid, because more and more of the ions dissociated as it was diluted. Hydrochloric acid was a strong acid, because nearly all of the ions were dissociated, regardless ofthe concentrations. Likewise, the NaOH was the weak base, as more OH ions dissociated as it became more dilute, and NH4OH was the strong base because all of the ions remained dissociated. The pH of weak acids and bases decreased with dilution, although more ions dissociated with higher dilution.REFERENCES Lab ManualChemistry for Engineering Students, Second Edition. Lawrence S. Brown, Thomas A.