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Data Table 1: Volume NaOH Used and [HCl]
Trials 1
2
3
Volume HCl
Vi NaOH (mL) +/- .05
Vf NaOH (mL) +/- .05
NaOH Used (mL0 +/- .05
[HCl]
% Error
10.0
50.0
45.3
4.7
0.032 +/-12.07%
40%
15.0
50.0
42.7
7.3
0.032+/-11.69%
36%
20.0
50.0
40.0
10.0
0.033+/-11.51%
34%
25.0
50.0
37.4
12.6
0.034+/-11.41%
32%
30.0
49.8
34.8
15.0
0.033+/-11.34%
34%
10.0
50.0
44.8
5.2
0.034+/-11.97%
32%
15.0
50.0
42.7
7.3
0.032+/-11.69%
36%
20.0
50.0
39.7
10.3
0.034+/-11.50%
32%
25.0
50.0
37.0
13.0
0.034+/-11.39%
32%
30.0
50.0
34.6
15.4
0.034+/-11.33%
32%
10.0
50.0
44.8
5.2
0.034+/-11.97%
32%
15.0
50.0
42.6
7.2
0.032+/-11.70%
36%
20.0
50.0
39.8
10.2
0.033+/-11.50%
34%
25.0
50.0
37.6
12.2
0.033+/-11.42%
34%
30.0
50.0
34.8
15.2
0.034+/-11.35%
32%
Qualitative Observations: Initial mass of NaOH solid = 1.9964 g +/- .0001g H20 volume = 500 mL +/- 5 mL While poring the h2o from the 500mL graduated cylinder to the beaker to make the .1 NaOH, the water was spilled resulting in a possible loss of data The initial solution of HCl was the incorrect concentration which resulted in a restart of t he lab and the previous data being thrown away. Some titrations were much darker than normal meaning too much base was used.
Sample calculation: -4 [HCl] for 10 mL: Moles NaOH = 4.7*.1 M =4.7*10 =4.7*10 /(10+4.7)=.032, [HCl] = .032 M
DCP 3- Presenting Processed Data Calculation Table 1: Title Volume HCl 10
Average [HCl] .033
Calculation (.05 mL - .033 mL)/.05 = .34*100 = 34% (.05 mL - .032 mL)/.05 = .36*100 = 36% (.05 mL - .033 mL)/.05 = .34*100 = 34% (.05 mL - .034 mL)/.05 = .32*100 = 32% (.05 mL - .034 mL)/.05 = .32*100 = 32%
.032
15
.033
20 25
.034
30
.034
Percent Error 34% 36% 34% 32% 32%
Percent Error Vs. Volume HCl 37 36 35 34 33
Percent Error
32 31 30 10
15
20
25
30
Volume HCl (mL)
The purpose of this lab was to determine if the amount of acid that is t itrated with a standard solution affects the percent error. Our hypothesis was if a larger volume of an unknown acid titrated with a standard solution of sodium hydroxide, then the results will have a smaller percent error. Based on the data that was collected from this lab this hypothesis was shown to mostly correct. As the volume of acid increased, the aver percent error decreased or remained the same for all but 10 to 15 mL. There the percent error increased from 34.66% to 36%. This was determined by comparing the literature value of the [HCl] to the experimental [HCl]. In the lab for almost all of the variations, as the volume of acid increased, the [HCl] became e closer to the literature value which reduced the percent error. Any errors in our lab were likely due to systematic errors, seeing as the % error was greater than the % uncertainty in all variations. The percent error of our measurements is how close the experimental values are to the literature, while the percent uncertainty is the margin of error in our measurements. Seeing as the percent error is relatively low and the experimental values are close to the literature values, these results can be considered accurate. During our experiment several sources of systematic error were met. One of the largest sources of error was the fact that the initial batch of HCl created for use in this lab was of the incorrect concentration. This resulted in the lab being restarted and all previous data being thrown out. Because the concentration was incorrect for the initial sample of HCl, any contamination or contact of the old HCl with the new one would result in incorrect data. Another source of error happened while setting up the lab. While preparing the solution of .1 M NaOH, the graduated cylinder used to measure and pour the waster was spilled. This resulted in the loss of some waster which slightly altered the concentration of sodium hydroxide. This was the greatest factor contributing to the percent error of the acid
concentration. A Final source of error was the fact that for some variations the solution was over titrated, resulting in too much base being used. There are several ways in which this experiment could be improved in the future. One way that would improve this experiment would be to increase the amount of trials done. In this lab only 3 trials were done limits the ability to eliminate any outliers. By only using 3 trials there is not a very large spread of data to process and examine. If this were increased it would make the results much easier to analyze. Another change that could be made is using a more precise way to measure out the water to crate the NaOH solution. By using a 500 mL graduated cylinder the uncertainty is +/- 5 mL which can make a large difference in the concentration if the solution. By increasing the precision of the tools used to measure our results would become even more reliable. Another testable question that could be considered is "How does the uncertainty of the instruments used to prepare the base solution affect the percent error of the results?" This would show the relationship between precision and accuracy when creat ing the solution and how it affects the data collected from the overall titration.
