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PKA & PKB of Weak Acids & Bases This laboratory is concerned with th

This laboratory is concerned with the determination of the pka and pkb of weak acids and bases. Most of the acid or base of weak acids or bases exists in the molecular form in solution, with little ionization. There are standard formulas for calculating the ka and kb of acids and bases, given the pH.

1. A small amount of each of three liquids, vinegar, seltzer water and ammonia, was placed into three separate, labeled cups. 2. The pH of the three liquids was determined using a calibrated pH meter.

3. The hydrogen ion concentration [H+] for the two weak acids was calculated using the formula pH = -log[H+] or [H+} = antilog)-pH). The results were recorded in the data table.

3. The hydroxide ion of the weak base was calculated using the formula pH = 14-pH, the [OH-] = antilog (-pOH) or [OH-] = 10-pOH. The results were recorded in the data table.

4. {A-} or [BH+] was recorded in the data table.

5. The molar concentrations of vinegar and ammonia were calculated and recorded in the data table.

6. The ka or kb were calculated and recorded in the data table.

7. The pka or pkb were calculated and recorded in the data table.

Data Table - Acid-Base Trilogy - Part I

1. acetic acid pka from Appendix D table 1 = 1.8x10-5 pka = 4.76

carbonic acid pka " " " = 4.3x10-7 pka = 6.45

ammonium hydroxide pkb " " = 1.8x10-5 pkb = 4.75

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PKA & PKB of Weak Acids & Bases This laboratory is concerned with th. (1969, December 31). In LotsofEssays.com. Retrieved 20:26, August 12, 2020, from https://www.lotsofessays.com/viewpaper/1705519.html