Question

Salt Measured Theoretical Theoretical Theoretical PH PH Ka PH% Error Original Buffer 4.72 4.744727495 1E-05 4.744727495 52.22% Water 5.63 7.0 1E-14 14 1957.14% Buffer with HCl 4.67 4.737489086 0.000018 4.744727495 142.46% Water with HCl 2.60 1.14 1E-14 14 3719.75% Buffer with NaOH 4.66 4.751565904 0.000018 4.744727495 191.53% Water with NaOH 10.80 14 1E-14 34 1692.31% 1. Note the large pH change that resulted when a dilution was made to the strong acid solution. Why was a large pH change not noticed when a weak acid was used? Dilution has a bigger change in strong acids then we got acids because strong acids disassociate maintaining a high initial concentration of hydrogen ions 2. Calculate the percent error in your experimentally determined $K_a$ values in Table 2 as compared to the literature $K_a$ values. Are you confident that your pH measurements are accurate? Briefly explain why or why not, if not, explain where error could have resulted in your experiment. % error in $K_a$ = (calculated $K_a$ - literature $K_a$ / literature $K_a$) \times 100% 3. When you measure the pH of salt solutions does the measured pH agree with the type of salt measured? Include any deviations from your observations

          Salt
Measured
Theoretical
Theoretical
Theoretical
PH
PH
Ka
PH% Error
Original
Buffer
4.72
4.744727495
1E-05
4.744727495
52.22%
Water
5.63
7.0
1E-14
14
1957.14%
Buffer with
HCl
4.67
4.737489086
0.000018
4.744727495
142.46%
Water with
HCl
2.60
1.14
1E-14
14
3719.75%
Buffer with
NaOH
4.66
4.751565904
0.000018
4.744727495
191.53%
Water with
NaOH
10.80
14
1E-14
34
1692.31%
1. Note the large pH change that resulted when a dilution was made to the
strong acid solution. Why was a large pH change not noticed when a weak acid
was used? Dilution has a bigger change in strong acids then we got acids
because strong acids disassociate maintaining a high initial concentration of
hydrogen ions
2. Calculate the percent error in your experimentally determined $K_a$ values in
Table 2 as compared to the literature $K_a$ values. Are you confident that your pH
measurements are accurate? Briefly explain why or why not, if not, explain
where error could have resulted in your experiment. % error in $K_a$ = (calculated
$K_a$ - literature $K_a$ / literature $K_a$) \times 100%
3. When you measure the pH of salt solutions does the measured pH
agree with the type of salt
measured? Include any deviations from your observations

Salt
Measured
Theoretical
Theoretical
Theoretical
PH
PH
Ka
PH% Error
Original
Buffer
4.72
4.744727495
1E-05
4.744727495
52.22%
Water
5.63
7.0
1E-14
14
1957.14%
Buffer with
HCl
4.67
4.737489086
0.000018
4.744727495
142.46%
Water with
HCl
2.60
1.14
1E-14
14
3719.75%
Buffer with
NaOH
4.66
4.751565904
0.000018
4.744727495
191.53%
Water with
NaOH
10.80
14
1E-14
34
1692.31%
1. Note the large pH change that resulted when a dilution was made to the
strong acid solution. Why was a large pH change not noticed when a weak acid
was used? Dilution has a bigger change in strong acids then we got acids
because strong acids disassociate maintaining a high initial concentration of
hydrogen ions
2. Calculate the percent error in your experimentally determined Ka values in
Table 2 as compared to the literature Ka values. Are you confident that your pH
measurements are accurate? Briefly explain why or why not, if not, explain
where error could have resulted in your experiment. % error in $Ka$ = (calculated
Ka - literature Ka / literature Ka) ×100%
3. When you measure the pH of salt solutions does the measured pH
agree with the type of salt
measured? Include any deviations from your observations

Added by Natalie V.

Question

Please give Ace some feedback