This can be justified by noting that for the reaction, \(K_{c} = \frac{1}{K_{b}}\) where \(K_{b}\) relates to the reaction of the conjugate base \(\ce{A^{-}}\) with water. 0.1 M sodium chloride, \(\ce{NaCl}\) (aq), 0.1 M sodium carbonate, \(\ce{Na2CO3}\) (aq), 0.1 M sodium acetate, \(\ce{NaCH3COO}\) (aq), 0.1 M sodium hydrogen sulfate, \(\ce{NaHSO4}\) (aq). When \([\ce{In^{}}]\) becomes significant compared to \([\ce{HIn}]\) the color of the solution will begin to change. where the solution is mixing smoothly but gently. and obtain your instructors initials confirming your success. After testing a solution, the student compares the strip color to the scale provided on the container and gives the solution a rating from . To perform a pH titration (OPTIONAL, if time permits). As a university or college science student, writing a lab report might not be new to you but it is a challenging process. In near future, I aspire to be an environmentalist and social worker. mark. Example of a Lab Report Conclusion. this value in the table on your data sheet. Acid-base indicators are themselves weak acids where the color of the aqueous acid is different than the color of the corresponding conjugate base. You will then Add 2 drops of phenolphthalein indicator to the remaining 50-mL of unknown acid or OPTIONAL procedure. Label Save the remaining solutions in the beakers labeled, HA and A and the beaker Consider your results for the 0-M NaCl solution. solution to completely dissolve the solid acid. The five indicators you will use in this experiment, their color transitions, and their respective values of \(\text{p}K_{ai}\) are given in Table 1. Introduction / Purpose (5 points) Why did we do this lab? Next you will equalize the volumes of the two solutions by adding water to the HA solution. After we test each substance, we recorded the data in a data table. Write the net ionic equation below that shows why this ion is acidic or basic: Consider your results for the 0-M NaHSO 4 solution. Select one of the 150-mL beakers and label it NaOH. the water. Get 5 beakers and label them A through E. Fill the beakers with 20 to 25 milliliters of the appropriate solutions and then cut a piece of pH paper at least one inch in length. noting that for the reaction, K c = 1/ K b where Kb relates to the reaction of the conjugate base A values of p K ai are given in Table 1. use this curve to find the midpoint of the titration. Rinse the 50-mL buret and funnel once with about 5 mL of 0.2 M \(\ce{NaOH}\) solution. Students looking for free, top-notch essay and term paper samples on various topics. Show the calculations you used and detail the steps you followed to prepare this buffer solution including the volumes of all solutions used: Compare the pH change of the buffer prepared above to that of deionized water upon the addition of a strong base by recording the following values: Briefly explain why the buffer is more resistant to a change of pH upon addition of the base than the water. Your instructor will demonstrate the proper use of the pH meters. Obtain a 50-mL buret from the stockroom. Explain. magnetic stirrer and stir-bar If you miss this mark, add some The lab manual may dictate where it should appear. Add a small amount of each substance into each container. Extract of sample "PH Determination of Solutions". One being acidic acidosis) and fourteen being basic (alkaline). The pH scale runs from 0 to 14, with 0 representing the highest concentration of hydrogen ions. Do not weak acids where the color of the aqueous acid is different than the color of the corresponding Summary. Performing this experiment is also, motived by the numerical correlation that the pH of a solution has on certain factors such as ion, concentration. with water. The procedure for operating every pH meter is slightly different. Record Finally, you will compare the buffering capacity of the buffer you prepare with that of deionized Dispense approximately 0.5-mL of the 0.2 M NaOH solution from your buret into your beaker. Record the results on your data sheet. 2- Theory. PH meter. Indicator p K ai 0 1 2 3 4 5 6 7, methyl violet 0 yellow blue-violet. begins to persist in solution longer before vanishing. specific pH as the pH (acidity) of the solution is varied. acid is a weak monoprotic acid. Conclusion: According to the results in Table 1, the pH of the different types of water starts to decrease after a 30 second exposure to CO 2. Eventually as [H 3 O+] decreases still further we will have, [H 3 O+] << K ai, and the color of the Your instructor will We'll not send Retrieved from https://paperap.com/paper-on-ph-lab-report-2/. axes with an appropriate scale. Record the color of the indicator in each solution on your data sheet. Conclusion By using the pH paper, dye indicators and the pH meter as tools of measurement, it has helped to determine which is more precise for this study. You will use these values to calculate \(K_{a}\). the pH meter and electrodes are calibrated against a buffer solution of known pH and potential differences are read directly in units of pH. Get 2 sets of test tubes and the label them A through E. Fill the tubes with equal amounts of solution and then in only the first set of tubes, place 2 drops of Promptly Blue dye into each and make sure it mixes in well with the solutions. Next you will equalize the volumes of the two solutions by adding water to the \(\ce{HA}\) solution. solution (available in the reagent fume hood). . Label solution longer before vanishing. bromcresol green indicator as expected? Initial pH is the result of the reading from pH meter for both solutions and the final pH is the result from adding hydrochloric acid until pH drops 1. the pH difference between subsequent 0-mL additions will start to grow larger. zinc sulfate that the color is violet. If it does not, the Data Analysis section is a good place to put it. Similarly, when \([\ce{H3O^{+}}] << K_{ai}, [\ce{HIn}] << [\ce{In^{}}]\) (the equilibrium will be shifted to the right) and the color of the solution will be essentially the same as color II. PH meter report 1. Rinse the 50-mL buret and funnel once with about 5 mL of 0-M NaOH solution. Use the pH meter to measure the pH of the solution following this addition. Around System Strategy and Policy Lab is deeply committed to delivering reforms and results.for the government and non-governmental organizations & institutions | 13 comments on LinkedIn View Measuring pH Lab Report.pdf from SCI 101 at Pocono Homeschoolers. spam or irrelevant messages, We use cookies to give you the best experience possible. { "01:_Chemical_Kinetics_-_The_Method_of_Initial_Rates_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Determination_of_Kc_for_a_Complex_Ion_Formation_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Le_Chatelier\'s_Principle_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Determining_the_Equivalent_Mass_of_an_Unknown_Acid_by_Titration_(Experiment)" : "property get [Map 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\newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 4: Determining the Equivalent Mass of an Unknown Acid by Titration (Experiment), 6: Qualitative Analysis of Group I Ions (Experiment), Part C: Using pH to Determine the Value of \(K_{a}\) for Acetic acid, \(\ce{CH3COOH}\)(aq), Part D: Determining the Value of \(K_{a}\) for an Unknown Acid by Titration, Part A: Determination of pH using Acid-Base Indicators, Part C: Using pH to Determine the Value of \(K_{a}\) for Acetic Acid, \(\ce{CH3COOH}\) (aq), Part D: Determining the Value of \(K_{a}\) for an Unknown Acid by Titration (Normal procedure), Part D: Determining the Value of \(K_{a}\) for an Unknown Acid by Titration (OPTIONAL procedure), Lab Report: pH Measurement and its Applications, Part A Determination of pH using Acid-Base Indicators, Part C Using pH to Determine the Value of \(K_{a}\) for Acetic Acid, \(\ce{CH3COOH}\) (aq), Part D Using a pH Titration to Determine the Value of Ka for an Unknown Acid, Pre-Laboratory Assignment: pH Measurement and Its Applications, status page at https://status.libretexts.org. 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