Explain Why The Concentration Of Hcl Acid Had A Ph Level Of B3

The full strength 1M HCl acid had a pH level of 3.12 (Table 3.1). Sample A2 to A4 remained in the pH 3 level, while sample A5 and A6 had a pH range of 4 (Table 3.1). The pH level for 1M HCl dilutions slightly increased between each sample (Table 3.1). The diluted solutions of 1 M NaOH showed a few unexpected results. The original solution of 1 M NaOH was at a pH level of 11.50 (Table 3.1). However, the pH of sample B2 increased to 12.81 (Table 3.1). The remaining samples had a decreasing pH pattern for each dilution step (Table 3.1). Although the pH of B4 was less than the pH levels of B2 and B3, it was greater than the pH of full strength 1 M NaOH (Table 3.1). The unknown solutions B and F were in a lower pH range of 3.28 and 3.65, while unknown solution A had a slightly higher pH level of 4.78 (Table 3.1). Unknown solutions D, E, and C had an increasing pattern of higher pH levels 10.78, 11.41and 12.71 (Table 3.1)
In this experiment, the 10x dilution with distilled solution in A2-A6 produce solutions containing greater pH levels compared to the original 1 M HCl solution.
B5 and B6 diluted solutions of 1 M NaOH are the only tubes that have lower pH levels than the original solution. The B1 10x dilution series yielded abnormal, unexpected results without a consistent pattern as apparent in the pH levels of B2, B3, and B4 diluted solutions. This could be affected by chemicals other than H+ or simple, inconspicuous human errors throughout the procedure. The pH of the diluted solutions did not increase or decrease in integers or a whole pH level, which was different from what my previous
expectations. The results obtained for the unknown solutions in this experiment have some similarities and differences with the results acquired in Part A. In Part A and C, unknown solution C had the same pH level of 12. Unknown solutions A, B, and F maintained an acidic pH in both Part A and C, while unknown E retained a high pH level. The results for unknown D vastly contrast between Part A and Part C. During Part A, unknown D was labeled as an acidic solution with a pH level of 5. In part C, unknown D revealed a drastically different property with a measured basic pH level of 10.78.
Determining the pH of diluted samples and unknown samples with a pH meter was much more precise and easier to read compared to the colorimetric method. The care necessary to clean and dry the electrode could prolong the length of the experiment. Setting up the device and operating the meter can be another complication. Although the pH meter can provide accurate measurements, this experiment has shown us the continual possibility of creating error in results. Overall, the pH meter is a reliable and convenient method for precision. For future work, I recommend experimenting a variety of diluting methods to create a specific range of pH for a given solution.