Identifying Pb+2: 1) Took 2mL of my unknown solution and added 2 drops of HCl and got white ppt which correlates with the positive control. 2) Centrifuged the ppt and soln‚ then discarded soln and washed ppt and centrifuged again. 3) I added 2mL of H2O‚ put the test tube in the hot water bath and stirred for 3 minute with a stirring rod. 4) I then decanted the solution into another test tube. 5) I added one drop of 6M acetic acid and 3 drops of 1M K2CrO4‚ which formed a positive confirmation where
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Name ___________________________________________Date experiment performed ________________________CRN of lab section: _______________________________ | Grade: ______________Days late: ____________Instructor Initials: _____ | General Grading Items | 25 Points | Attendance at Pre-lab Meeting | /10 | Copies of lab pages attached; labeled with name and date‚ complete information‚ readable‚ data recorded matches results given in report | /5 | Waste was properly disposed of and lab area was
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Purpose This experiment shows how different concentrations of acids and bases in a solution affect its pH level. When acids and bases are combined in a solution‚ they neutralize each other. This means that depending on the concentration of both acids and bases in a solution‚ the pH will vary. A neutral pH level is 7; anything below that level is known as an acidic solution‚ while anything above is known as a basic solution. To find out the pH‚ the solutions will be diluted and tested with different
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LAB REPORT 5 – ACID/BASE CHEMISTRY No credit will be given for this lab report if the Data section is not completely filled out and if the required photographs are not received. At least one photograph must show the student’s face. NOTE: This experiment is rather lengthy. Plan accordingly. OBJECTIVES 1. Define strong electrolyte‚ weak electrolyte‚ nonelectrolyte‚ acid‚ base‚ salt‚ strong acid‚ weak acid‚ strong base‚ weak base‚ and neutralization reaction. 2. Compare and contrast the chemical
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A buffer solution can maintains a narrow range of pH even when strong acid are added. In our experiment‚ we can see water is not a buffer‚ water can undergo very big changes when small amounts of strong acid or strong bases are added. When the strong acid‚ 100µl HCl was added into the dd water‚ the pH value changed from 7.38 to 5.83 which mean the dd water has turn into acid. The same phenomenon occurs while strong base‚ 100µl NaOH was added into the dd water. The pH value changed from 7.07 to 9
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Buffer Preparation (Gozani Lab) 1. 1 M Tris-HCl Buffers pH Volume (L) TrisBase (g) HCl (ml) pH 7.0 2 242.2 150-155 pH 7.5 2 242.2 120-125 pH 8.0 2 242.2 80-85 Autoclavable. 2. EDTA 0.5 M (pH8.0) 0.5M‚ 1L: 148 g EDTA + ~30-40 g NaOH to adjust pH (or 186 g EDTA-Na.2H2O + ~20 g NaOH) Note: pH adjusted by NaOH is essential for solubility. Autoclavable. 3. TAE DNA Electrophoresis Buffer (50 X) (2 M Tris‚ 50 mM EDTA) 2L 484 g Tris 114.2 ml glacial acetic acid 200 ml 0.5 M EDTA 8.0 To make
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BUFFER SOLUTION (ACID) An acidic buffer solution is simply one which has a pH less than 7. Acidic buffer solutions are commonly made from a weak acid and one of its salts - often a sodium salt. Objectives: 1. Measure the pH of the unknown solution first with indicators and then with pH paper. 2. compare the buffer solution with both a strong acid and a weak acid materials: 2 30 mL beakers 2 100mL volumetric flask 1 10mL pipet 2 aspirator 1 50mL graduated cylinder 1 10mL graduated
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General Chemistry LABORATORY REPORT Practical 1 Title: Investigation of the suitability of indicators and instrumental detection of equivalence points in acid-base titrations Objectives 1. To understand the importance of choosing suitable indicators for detecting the end points of acid-base titrations. 2. To obtain titration curves for some acid-base titrations. Introduction Indicator is usually a weak organic acid or base that has distinctly different colours in its protonated
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Results: For the solutions acid and bases lab the results my group received are as followed. Procedure 5.1 were we had to measure the ph of the following substances Vinegar 4 Apple Juice 4 Black coffee 5 Baking Soda + Sprite 8 0.01mM HCl 4 0.1mM HCl 3 Distilled water 4.5 Tap Water 5 Procedure 5.2 -Test the ability of buffers Before Buffer After Buffer Water 4 Water 4 0.1M phosphate buffer 6.5 0.1M Phosphate buffer 6.9 0.1M NaCl 4 0.1M NaCl 4.8 Procedure 5
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As for the results of our tests‚ we came up with interesting findings. For the first test we conducted‚ pH‚ we came up with statistically significant results. Our p-value was .002‚ well below the .05 threshold. The control group’s mean pH was 6.65‚ whereas the experimental group’s was 6.46. This resulted in a change in pH of .19‚ making the water more acidic. As for the Q-values‚ the control group’s had a Q-value of 81 and the experimental had a Q-value of 75‚ that’s a decrease of 6‚ a significant
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