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The Properties of Buffers

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Submitted By amandaaax3
Words 431
Pages 2
General Chemistry II
Professor: Dr. Yang Yang
Turned in: April 9, 2014

Experiment #6

The Properties of Buffers

Abstract
In this experiment the pH of fours solutions was recorded and identified as acidic, basic, or neutral. A buffer system of 0.10 M ammonium ion (NH4+) and 0.10 M ammonia (NH3). This buffer was made three times: once with equal parts ammonium ion and ammonia, next it was diluted to double the volume, and finally it was prepared with an addition of HCl. The pH was recorded to calculate the Ka and pKa values. The most accurate Ka value recorded was the second from B2 which was 5.13x10-10. Using this Ka value the appropriate volumes of ammonium ion and ammonia were calculated to make a buffer solution with a pH of 8.7. The final volumes were 15.9 mL of ammonium ion and 4.1 mL of ammonia.
Part A solution pH acidic, basic, neutral?
0.100 M NaHSO4 1.8 acidic
0.100 M Na2CO3 11.2 basic
0.100 M NH3 10.9 basic
0.100 M NaCI 6.8 neutral

Net Ionic Reaction

NaHSO4
Na+ + HSO4- + H2O --> Na+ (SO4)2- + H3O+
HSO4- + H2O --> (SO4)2- + H3O+

Na2CO3
Na2CO3 + H2O --> NaHCO3 + NaOH
2Na+ + CO32- + H2O --> Na+ + HCO3- + Na+ + OH-
CO32- + H2O --> HCO3- + OH-

NH3
NH3 + H2O --> NH4-+ OH-

NaCI
NaCI + H2O --> H2O + Na+ + Cl-
NaCI--> Na+ + Cl-

Part B calculations attached on next page

Ka Values

Part Ka pKa
B1 6.3x10-10 9.2
B2 5.13x10-10 9.29
B3 3.98x10-10 8.4

Discussion: All of the Ka values were relatively close to one another with a mean of 5.14 x 10-10 and a standard deviation of 1.16 x 10-10. The small variability in these values could be due to slight error in preparing the solutions. Rounding errors could have also taken place while recording the pH. The B2 value of 5.13 x 10-10 was used in step 7 because it was closest to the real Ka value of 5.6 x 10-10. This was used to calculate the volumes needed of ammonium ion and ammonia to create a buffer solution at our target pH of 8.7. The calculated colume of ammonium ion was 15.9 mL and 4.1 mL of ammonia. Once this solution was made the pH was 8.8. We did not reach the target pH of 8.7. This was most likely due to an error in accuracy; trying to get 0.1 mL was very difficult.

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