In this hypothetical example \(\ce{In}\) stands for the indicator. Performing this experiment is also, motived by the numerical correlation that the pH of a solution has on certain factors such as ion, concentration. Balanced Equation: HCl ( aq) + NaOH ( aq) ---> NaCl ( aq ) + H 2 O ( l ) If a reaction happens in your experiment, you must include a balanced equation somewhere in your report. Submit this graph with your report. Obtain a vial containing your unknown solid acid from your instructor and record the letter and number of this unknown acid on your data sheet. Additional materials, such as the best quotations, synonyms and word definitions to make your writing easier are also offered here. [HIn] [In ], and so K ai = [H 3 O+], or p K ai = pH. Record this value in your data table alongside the measured volume. 0 pH unit. Swirl gently to mix. Add a drop or two or bromcresol green indicator to each of these solutions. Clean and then return You only need to complete this table if your instructor chooses the OPTIONAL procedure for Part D. This page titled 5: pH Measurement and Its Applications (Experiment) is shared under a CC BY-NC license and was authored, remixed, and/or curated by Santa Monica College. View Measuring pH Lab Report.pdf from SCI 101 at Pocono Homeschoolers. Use the pH meter to measure the pH of the solution following this addition. Use your pH meter to confirm the pH of your buffer solution. Record the PH of household products. To determine the value of K a for an unknown acid. 1. Get 5 beakers and label them A through E. Fill the beakers with 20 to 25 millimeters of the appropriate solutions and then cut a piece of pH paper at least one inch in length. Consider your results for the 0.1 M \(\ce{ZnSO4}\) solution. Use Lab Report . spam or irrelevant messages, We use cookies to give you the best experience possible. 50-mL buret. Which of the following 0.1 M solutions will have the highest pH: acetic acid, \(\ce{HCl}\), ammonium chloride, \(\ce{NaH2PO4}\)? within one pH unit. All plants received the same amount of sun exposure in the laboratory. It can detect also weak bases, but mostly, strong. of the solutions listed in part A of the report sheet. Table 1 to determine the pH range of four solutions to within one pH unit. Extract of sample "PH Determination of Solutions". begins to persist in solution longer before vanishing. . is exactly at the 0-mL mark when read at eye level. For You For Only $13.90/page! order now. Select one of the 150-mL beakers and label it NaOH. procedure is appropriate for your lab section. A lab report conveys the aim, methods, results, and conclusions of a scientific experiment. Combine this with the unknown solid acid sample in your 150-mL beaker. You will then combine equal volumes of these two solutions in order to form a new solution. It should be between 5 and 7. When you are assigned a biology lab report, it is important to understand the purpose of the assignment and how to write a lab report that will be accepted by your instructor. 14 Very Pale Pink Acid/Base/Neutral pH Reading Color of Extract Acid 4. Rinse the 50-mL buret and funnel once with about 5 mL of 0.2 M \(\ce{NaOH}\) solution. Half fill 7 small beakers with Sprite, Vinegar, Dish detergent, Baking soda, Ammonia, Coke and Orange juice individually and equally measured. the titration. pH 7), the number is equal to the negative exponent of the H + ion concentration. solution with the following equation. Now measure out 25-mL of the solution from the beaker labeled A and combine this solution to completely dissolve the solid acid. The main purpose of a lab report is to demonstrate your understanding of the scientific method by performing and evaluating a hands-on lab experiment. congo red turns violet at pH values of 3 or less. In general we can say that an acid-base indicator . Base 8. 5, and the acid has a pH >5. , then an Alizarine yellow indicator may be used. Substances are tested with pH strips and placed on the continuum of the pH scale range of 1 to 14. Explain your answer. Is the solution acidic or basic?____________, Which ion, \(\ce{Na^{+}}\) or \(\ce{CO3^{2-}}\) is causing the observed acidity or basicity?____________, Consider your results for the 0.1 M \(\ce{NaHSO4}\) solution. Get a custom sample essay written according to your requirements urgent 3h delivery guaranteed. 22 20 drops Table 4: Consists of pH levels in distilled water solution and Alkali-Seltzer tablet in distilled water solution. The Influence of pH on the Activity of Catalase Enzyme Pages: 5 (1203 words) Enzyme catalysis lab Pages: 4 (1078 words) Projectile Motion Lab Report: Lab Assignment 1 Pages: 3 (762 words) Macromolecules lab bio 1 lab Pages: 2 (520 words) Why Lab Procedures and Practice Must Be Communicated in a Lab? Rinse this beaker once more with about 5 mL of 0.2 M \(\ce{NaOH}\). Put 30 mL of 1.0 M acetic acid solution into the first beaker and 30 mL of 0.010 M acetic acid solution into the second. (If The term "pH" is short for "potential of hydrogen.". Guidance for Enzyme Lab Report. Data and Conclusions: The purpose of this experiment was to learn how to use distillation and gas chromatography to separate and identify different compounds from a given mixture. Consider your results for the 0-M Na 2 CO 3 solution. The results showed that beans soy were at precisely 6.00. suppose we have a solution in which methyl violet is violet. When the pH again begins to jump and you Results and Discussions pH ratio between acid and base: 7.3 = 6.82 + x x = 0.48 0.48 = log ([base])/([acid]) 100.48 =base/acid salt/acid = 3.02 There, 1 acid : 3 base 93 Pastel green Neutral 7. use any soap as the residue may affect your pH measurements. use this curve to find the midpoint of the titration. zinc sulfate CHEMISTRY THIRD LABORATORY REPORT pH SCALE AND THE USE OF pH INDICATORS I Written by: Amelia Quinta Jasmine (CHE) Syadza Luthfiyya (FT) Date of Experiment: March 11th, 2016 Date of Submission: March 18th, 2016 Department of Chemical Engineering Department of Food Technology Faculty of Life Science International University of Liaison Indonesia 1.1 Purpose In this experiment, various of . As a university or college science student, writing a lab report might not be new to you but it is a challenging process. What we would probably change next time would be to organize better and write in a more organized way out . in Figure 1. Part C Using pH to Determine the Value of K a for Acetic Acid, CH 3 COOH( aq ). Create an outstanding lab report conclusion that is unique but reflects the actual . Acid-base indicators are themselves weak acids where the color of the aqueous acid is different than the color of the corresponding conjugate base. Under these conditions the solution will be yellow. By adding more base to a solution it dilutes the acidity. A buret stand should be available in the the value of the pH at the midpoint of your graph to determine the value of K a for your unknown When given the color results, by the mixture of the solution and the extract, table one and two were seed to determine which solutions were acidic, neutral or basic. Obtain a vial containing your unknown solid acid from your instructor and record the Do not use any soap as the residue may affect your pH measurements. Using a ring stand and your utility clamp, or the stand and clamp provided with your pH indicated by Equation (1) will shift to the right and [HIn] will decrease while [In ] increases. Soapy Water 8 Conclusion In concluding this lab I found that, in general most groups had similar recordings in their lab. within one pH unit. Also, by adding Promptly blue and Phenolphthalein afterwards to the solution it would indicate what color it would turn to when mixed into an acid and a base. if this pH is less than neutral. b. Filter the solution through cheesecloth into a test tube and add an equal volume of distilled water 2. You may assume that this acid is a weak monoprotic acid. The pH of the solution in your beaker labeled, 50-50 buffer mixture, is also the p K a of 26 Light Pink 2. This is displayed through an opposing scale, ). At some point during your titration Solutions that have low pH's or a ph level below 7 are considered acidic. Get 5 small beakers and label them A through E. Half fill the small beakers with the appropriate solution as it was done with the prior experiment but this time a pH meter and a cabbage extract called intoxication will be used. The pH meter is similar to a calculator or digital scale, enter the information and it does the calculation for the solution. addition. By using the pH paper to measure the solutions A through E it would point out what substance is an acid and which one was basic. Then use these colors and Table 1 to estimate the pH range of each solution (for example, pH =1-2): Record the measured pH and the color of bromcresol green indicator observed for each solution: Complete the following table. The reaction time at pH 9.0 (2.16 min) is greater than that of 8.0 (1.57 min) which is also greater than that of 7.0. The actual units for the alkalinity titration are moles or equivalents per volume (moles/L or eq/L). A 3 on the pH scale is 100 times more acidic than a 1. . A titration curve of an amino acid is the plot of the amino acids against the neutralization degree of the acid by a strong base such as NaOH. does not succeed. and similar size coleus cuttings grew in acidic vinegar water solutions ranging from 2 to 4 pH. In this part of the experiment you will prepare a buffer solution with a pH specified by your instructor using appropriate portions of the \(\ce{A^{-}}\) and \(\ce{HA}\) solutions prepared in Part D. This can be accomplished using Equation \ref{10} to determine the ratio, \(\frac{[\ce{A^{-}}]} {[\ce{HA}]}\), that will produce the specified pH of the buffer solution. As an example consider an acidic solution containing the indicator \(\ce{HIn}\) where \([\ce{H3O^{+}}] >> K_{ai}\), and therefore, \([\ce{HIn}] >> [\ce{In^{}}]\). Answer each question to the best ofyour ability Show ALL calculations and use complete sentences One-word answers will never be given credit Last week in lab, you made : mixture of P-nitrophenolphosphate and enzyme at fixed concentrations Then, you measured the absorbance of p-= -nitrophenol = over time Generate graph that shows how average absorbance changed over time for your reaction best . Explain your answer below in terms of chemical equations Add 5 drops of the remaining 0 M NaOH solution to both the beaker containing your buffer All 50 ml of distilled water into two small beakers. changes color at a pH determined by the value of K ai or p K ai for that particular indicator. Using Equations \ref{3} and \ref{4} in the background section of this experiment, show that \(K_{a} = [\ce{H3O^{+}}]\) for the 50-50 buffer solution: (OPTIONAL) Is the endpoint of your pH titration that you marked on your titration curve the same as the equivalence point of the titration? 1. This would be more attractive to human error because there is no color chart it could match to, so the human eye would be the judge to what color the solution turn to when the dye indicator were added. laboratory room. Rinse this beaker once more with about 5 mL of 0.2 M \(\ce{NaOH}\). specific pH as the pH (acidity) of the solution is varied. noting that for the reaction, K c = 1/ K b where Kb relates to the reaction of the conjugate base A You will use these values to calculate \(K_{a}\). Record the measured pH and the color of bromcresol green indicator observed for each solution. 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. Since the equivalence point occurs when 16.0 mL of NaOH are added, the pKa, or half- equivalence point will equal the pH when half of the acid is neutralized, at 8.0mL NaOH added. Water 6. Generally only one or two drops of indicator are added to the solution of interest and therefore the amount of \(\ce{H3O^{+}}\) due to the indicator itself can be considered negligible. 1. The report is intended to complement your bench training by giving you the opportunity to demonstrate your understanding of the biologic significanceof your work as well as Record Discuss the methods used. instructor using appropriate portions of the A and HA solutions prepared in Part D. This can be accomplished using Equation (10) to determine the ratio, [A] / [HA], that will a colorless solution. The beaker with Alkali-Seltzer tablet and the distilled water solution was measured for its pH level and recorded the reading for the initial PH. Published on May 20, 2021 by Pritha Bhandari.Revised on July 15, 2022. stop the titration. The pH scale starts from 0 to 14. Good Essays. This is with the independent and dependent variables. Add a drop or two or bromcresol green indicator to each of amount of the 0-M NaOH you added during your titration and add this volume of Initially starting at a pH of . The easiest part was checking the pH of the substances. This is because the whole lab report structure consumes. Proceeding in a similar manner, you will use the acid-base indicators in Table 1 to determine the pH range of four solutions to within one pH unit. Select one of the 150-mL beakers and label it NaOH. In part two of the experiment, 0.7128 g of Unknown B weak acid was dissolved with water in a 100-mL volumetric flask, and 25.0-mL of that solution was pipetted into . 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Discard all chemicals in the proper chemical waste container. Record this pH of 50-50 buffer solution: _____________, Ka of unknown weak acid: _____________ ( from measurement of 50-50 buffer solution ). Lab Report. When the pH value is a whole number (e.g. Explain your answer. Label this beaker, 50-50 buffer mixture., Now measure out 25-mL of the solution from the beaker labeled A, The pH of the solution in your beaker labeled, 50-50 buffer mixture, is also the pK. Next you will equalize the volumes of the two solutions by adding water to the HA solution. add base to the solution resulting in a decrease of [H 3 O+]. This work, titled "Ph lab report assignment" was written and willingly . The pH meter was the most precise tool of the three and it would give out the most precise measurements of the pH level of the substance. How To Write A Lab Report | Step-by-Step Guide & Examples. Because there's a 1:1 ratio, the moles of the acid must equal the moles of the base in order to reach . Take on strip of pink and purple litmus paper and submerge the tip of each paper with the substance. Introduction. Table B: pH Data for Acetate Buffers (Indirect Method) 2. Use your pH meter to determine the pH of each solution. Stir your solution to completely dissolve the solid acid. buffer solution. this beaker, A. To conclude, this was a very interesting project. These data will be used to plot a titration curve for your unknown acid. The acid reacts with a base to produce water and salt. Rinse two small 100 or 150-mL beakers as before. Use equations to support your explanation: Why isnt the measured pH of the deionized water before adding the NaOH( aq ) equal to 7? You will need the following additional items for this experiment: pH meter, magnetic stirrer and stir-bar, 50-mL buret. 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. function be certain that this remains off throughout this experiment. Use the pH meter to measure the pH of the solution in the beaker labeled A. GENERAL SAFETY: Students must wear safety goggles and lab coats at all times. Continue recording the total volume added and the measured pH following Finally, by looking at the result of the pH reading level that was given from the pH meter, it will determine which solution is basic or acidic. the pH difference between subsequent 0-mL additions will start to grow larger. A buret stand should be available in the laboratory room. *Thymol blue is a polyprotic acid with two pKa values. The color chart gives you a number on where in the pH level it would land on but could be misread by human error. <br><br>My main research interests are in . If you miss this mark, add some Acid-base indicators are themselves (2019, Dec 06). Use the value of the pH at the midpoint of your graph to determine the value of \(K_{a}\) for your unknown acid. mark. Put 30 mL of 1-M acetic acid Materials and Methods Ph Paper. Step 2: Discuss the Experiment and hypothesis in the lab report conclusion. congo red As [H 3 O+] decreases the equilibrium help. Clean up. When the pink color from the phenolphthalein indicator persists for at least 2 minutes you have reached the endpoint of your titration. using deionized water. directly enter the beaker during the titration. If the magnetic stirrer also has a heater Into each of your four clean beakers collect about 30 mL of one of the following: Use your pH meter to determine the pH of each of these four solutions. Lab Report Conclusion Template Restate: We set out to test the acidity level in bean soy using a PH scale; the experiment's objective was to confirm that the acidity should be 6.00. Record the colors of the indicators observed for each solution tested. pH and color transition Rinse four small 100 or 150-mL beakers several times using deionized water. The equilibrium-constant expression for Equation \ref{1} is: \[K_{ai} =\dfrac{[\ce{H3O^{+}}][\ce{In^{-}}]}{[\ce{HIn}]} \label{2}\], \[ \dfrac{[\ce{In^{-}}]}{[\ce{HIn}]}= \dfrac{K_{ai}}{ [\ce{H3O^{+}}]} \label{3}\]. slow down your addition rate to just 2 to 3 drops per addition. Founder/Executive Director, System Strategy and Policy Lab Report this post Report Report This tells us that the pH of our unknown solution is greater than or equal to 2 because methyl violet turns violet at pH values of 2 or greater. the water. Once a buffer has reached its limit, the solution will exponentially increase or decrease, depending on if a base or an acid were used, respectively. Save the remaining solutions in the beakers labeled, HA and A and the beaker The important ions used in this experiment for the auto-, . H 3 O+ in the solution is therefore controlled by the concentrations of the other acids and/or bases Because \([\ce{H3O^{+}}]\) can be determined by measuring the pH of the weak acid and \([\ce{HA}]_{0}\) is known you can determine the value of \(K_{a}\) using Equation \ref{8}. Stir your additional 0-M NaOH from your beaker and try again. and therefore, [HIn] >> [In]. These data will be used to plot a titration curve for your unknown acid. The coleus in distilled water grew an . Students looking for free, top-notch essay and term paper samples on various topics. Therefore, a lab report conclusion refers to the last part of the report. Record this value below. reached the endpoint of your titration. Legal. species from the atmosphere dissolves in water that is left standing? A pH of 7 is neutral. including the volumes of all solutions used: Compare the pH change of the buffer prepared above to that of deionized water upon the addition I look forward to working with you moving forward . It is suggested you use only a portion of each of these two solutions in case your first attempt does not succeed. It should open with a brief background or introduction, then state the problem or purpose of the research. sodium carbonate Do you know why? 0-M solution (only): Record your results below. Now we will test the buffer solution you prepared against changes in pH. The lower the number the more acidic . Finally, you will compare the buffering capacity of the buffer you prepare with that of deionized The pH scale goes from numbers 1 thru 14. If it is found that a substances pH is equal to 7, then its determined to have a neutral pH. To produce the base, you titrate a portion of the weak acid with \(\ce{NaOH}\) to the end point of phenolphthalein. Explain: The results supported the hypothesis that the proper PH of beans soy is 6. with the solution in your beaker labeled 50-50 buffer mixture. Record the color of the indicator in each solution on your data sheet. This will ensure \([\ce{A^{-}}]\) in the titrated solution is equal to \([\ce{HA}]\) in the \(\ce{HA}\) solution. sheet. Please consult your instructor to see which procedure is appropriate for your lab section. The above equation is used to neutralize the acetic acid. Here we are assuming Equation (9) proceeds essentially to completion. Rinse four small 100 or 150-mL beakers several times using deionized water. The general equation for the dissociation of a weak acid, \(\ce{HA}\) (aq), in water is: \[\ce{HA (aq) + H2O (l) <=> A(aq) + H3O^{+} (aq)} \label{4}\], \[K_{a}=\dfrac{[\ce{A}] [\ce{H3O^{+}}]}{[\ce{HA}]} \label{5}\], When we construct an ICE table for this reaction we can see that at equilibrium, \[[\ce{A^{-}}] = [\ce{H3O^{+}}] \label{6}\], \[[\ce{HA}] = [\ce{HA}]_{0} - [\ce{H3O^{+}}] \label{7}\]. Record this mass on your data sheet. 0 pH unit. Note that when [H 3 O+] >> K ai, [HIn] >> [In ] (the equilibrium will be There are several kinds of distillation methods. If you are being asked to make a buffer at pH 4.00, what is the appropriate ratio of A. than the value of 7 are considered to be basic whereas values below 7 are considered to be acidic. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Record these values on your data sheet. ANALYSIS AND CONCLUSION: Analysis: - The pH, or potential of hydrogen, of a substance can be measured by using pH indicators such as litmus paper, . We can represent the dissociation of an acid-base indicator in an aqueous solution with the following equation. 6- discussion. Provide a brief overview of the experiment you did in like 1-2 sentences. Place 2 drops of color extract (intoxication) in each beaker and make sure it mixes in well until there is a distinctive color. solution will have turned to blue. By continuing well assume youre on board with our cookie policy, Dont waste Your Time Searching For a Sample, Employee Motivation From Performance Measurement and Compensation System Management, ASK writer for . Place 30 mL of your 0.60 M acetic acid in a clean 100 mL beaker. This tells us that the pH of our solution is less than or equal to 3 because congo red turns violet at pH values of 3 or less. Label PH meter. equal volumes of these two solutions in order to form a new solution. titrated solution will contain only the conjugate base of the weak acid according to. Introduction / Purpose (5 points) Why did we do this lab? mixed to form the 50-50 buffer solution? Now suppose we add some congo red to a fresh sample of our solution and find The pH of the solution in your beaker labeled, 50-50 buffer mixture, is also the p K a of pH Measurement and its Applications Solutions that have a high pH level or above 7 are considered basic. exp 22 acid-base properties of indicators.docx, The grower should add bags of brand A and bags of brand B to minimize the amount, EdgenuityProjectReflectionQuestions (10).docx, If gx 4 2x find gx 4 A 2x 4 B 2x8 C 2x12 D 2x 12 2 If fx x 2 5 and 2x2 what is, Humanistic theorists believe that an important force motivating individuals is a, Do you anticipate any changes in the next 12 months Comments D Yes D Yes No No, Newspaper+articles+for+Zero+Hours+Contracts+discussion+tutorial+2.docx, 2 Three_Faces_of_Eve_Dissociative_Identity_Disorder_Case_Study.docx.pdf, engaging in long distance learning To ensure equitable educational opportu, The use of insulin to purify its receptors is an example of A Ion exchange, Multiple choices 4060 Why cant we rely just on textbooks as information sources. . values of p K ai are given in Table 1. Include and Analyze Final Data. Put the magnetic stirrer onto your buret stand so that the buret is directly over the magnetic stirrer. Lab Report 1 - Free download as PDF File (.pdf), Text File (.txt) or read online for free. . . labeled HA and transfer this volume to your fourth clean rinsed 150-mL beaker. Your instructor will demonstrate the proper use of the pH meters. Observe the pH change after each addition carefully. value in your data table alongside the measured volume. bromocresol green Using indicator dyes. The five indicators you will use in this experiment, their color transitions, and their respective OPTIONAL procedure: Titration is performed while, Rinse five small test tubes using deionized water (there is no need to dry these). 2.It is important to stir the solution as u progress through an experiment because it helps make sure that the reaction is complete. To measure the pH of various solutions using pH indicators and meter. (8.2) pH value = X [ H +] = 10 X M. So for pH 7, the H + ion concentration is 10 -7 M. The pH values of everyday chemicals typically range from pH 0 to pH 14. 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. However, the same way that pH and POH are inversely, related, so are these. acid is a weak monoprotic acid. By comparing the colors you observe in each tube you should be able to determine the pH of the 0.1 M \(\ce{HCl}\) solution to within one pH unit (see background discussion). 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 { "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 MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_pH_Measurement_and_Its_Applications_(Experiment)" : "property get [Map 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https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FAncillary_Materials%2FLaboratory_Experiments%2FWet_Lab_Experiments%2FGeneral_Chemistry_Labs%2FOnline_Chemistry_Lab_Manual%2FChem_12_Experiments%2F05%253A_pH_Measurement_and_Its_Applications_(Experiment), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 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. Report the p K a value you determined for your unknown acid in Part D to your instructor who will The relatively close pH levels of Tap Water, Spring Water, Flavored Water, and Seltzer Water. solution in your beaker, low enough down that the meter can read the pH, but high Chemistry Lab Report 30 April PH Determination of Solutions Introduction PH (potential hydrogen) may be defined as the concentration of hydrogen ions in a given solution ("PH as a Measure of Acid and Base Properties"). 0 unit. Record the results on your data Recall that the pH of a Part D. Determining the Value of Ka for an Unknown Acid by Titration (Normal procedure). To create and study the properties of buffer solutions. Words: 284 . this time, the pink color from the phenolphthalein indicator will also begin to persist in It is a measure of how many excess H+ ions there are in a solution. From the measured pH and concentration of a weak acid solution you can determine the value of \(K_{a}\) for the acid. What is its pH range? 5-Calculation. deionized water to the contents of the beaker labeled, HA. beaker. From the objective of the experiment to lab report conclusions, each structure wrestles for time. Use the known value of \(K_{a}\) for acetic acid from your textbook to determine the percentage error in your measured \(K_{a}\) value for each solution. Buffer. As \([\ce{H3O^{+}}]\) decreases the equilibrium indicated by Equation \ref{1} will shift to the right and \([\ce{HIn}]\) will decrease while \([\ce{In^{}}]\) increases. After completing the pH measurements, comment on the pH of the salts as compared to the . The main function of buffers is to help keep pH levels steady when a certain amount of acids or bases are introduced in a solution. Consider your results for the solutions of 0.1 M \(\ce{HCl}\) and 0.1 M \(\ce{CH3COOH}\). Youth Agency Marketplace YOMA Training for Young TECH LEADERS Powered by UNICEF Generation Unlimited System Strategy and Policy Lab in collaboration with To read the essays introduction, body and conclusion, scroll down. Clamp the buret to the buret stand making sure that it is vertical. Determine whether or not this solution is a buffer solution, and enter your decision in Data Table B. In this part of the experiment you will learn to use a pH meter to measure pH. solution in the beaker labeled A. Since \(\ce{A^{-}}\) is known to be a weak base we know that \(K_b << 1\) and therefore \(K_c >> 1\). 3 1 drop Beaker Initial pH Final pH Drops HCI Added Alkali-Seltzer 6. Do not be alarmed if this pH is less than neutral. On the second set of tubes do the same but this time place 2 drops of Phenolphthalein into the solutions. Your measured pH value should be within \( \pm 0.2\) pH units of your assigned value. The pH scale runs from 0 to 14, with 0 representing the highest concentration of hydrogen ions. To perform a pH titration (OPTIONAL, if time permits) It should be between 5.2 and 7.0. Measure the pH of the solution and record it in Data Table B as solution 1B. Write the chemical equation describing the equilibrium reaction between acetic acid and water: Complete the following table. Name: ____________________________ Lab Partner: ________________________, Date: ________________________ Lab Section: __________________. where the solution is mixing smoothly but gently. all borrowed equipment to the stockroom. If time allows you will measure the pH as a function of the volume of NaOH solution added in The titration with NaOH occurs in two stages as shown in the equations below. The second pKa is around 8. By first measuring the pH levels of solution A through E with a pH meter, it gives a numeric reading to pH balance to a solution. you overshoot the endpoint by more than this you may need to repeat this titration, see Which ion, Na+ or CO 32 is causing the observed acidity or basicity? Conclusion: I think that the Acids and Bases Lab was a very fun and also very helpful experiment when it comes to understanding the concepts of pH and using the pH scale to . enough up so that the probe tip does not contact the rotating magnetic stir-bar, as shown In this part of the experiment you will use five indicators to determine the pH of four solutions to within one pH unit. letter and number of this unknown acid on your data sheet. In other words the solution will change color when \([\ce{HIn}] [\ce{In^{}}]\), and so \(K_{ai} = [\ce{H3O^{+}}]\), or \(pK_{ai} = pH\). Upon completion of the titration, the titrated solution will contain only the conjugate base of the weak acid according to, \[\ce{HA(aq) + OH^{-} (aq) <=> A^{-}(aq) + H2O(l)} \label{9}\]. A limited time offer! assign you the pH value of the buffer solution you will prepare in this part of the experiment. We can use the values in Table 1 to determine the approximate pH of a solution. Proceeding in a similar manner, you will use the acid-base indicators in When you feel you are In conclusion, our hypothesis was supported because it was found that pH 7.0 is the optimal temperature for the enzyme amylase and pHs lower or higher than that would result in slower reaction rates. Is the solution acidic or basic? pH of 50-50 buffer solution: _____________, \(K_{a}\) of unknown weak acid: _____________ (. Next, add in a natural indicator called intoxication made from the pigment from a red cabbage into each solution and mixed it until there is a distinct color and recorded on the chart. solution and that containing the deionized water. Do not State Whether Your Experiment Succeeded. shifted to the left in accord with Le Chatelier's principle) and the color of the solution will be \[\underbrace{\ce{HIn (aq)}}_{\text{yellow}}+\ce{H2O (l) <=> } \underbrace{\ce{In^{-} (aq)}}_{\text{blue}} + \ce{H3O^{+} (aq) } \label{1}\]. If the pH change it too lager or too small (0.1 < dpH < 0.5) then pour a new 20mL sample and use an appropriately adjusted concentration of . Observe the pH change after each addition carefully. In this paragraph, provide an overview of the lab experiment in a brief manner. The pH of the solution enables it to be categorized as an acid or a base. 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. By measuring the pH levels from the distilled water solution with the pH meter, it gives a numeric reading for water which becomes the initial PH. Its important to maintain an understanding that when these concentrations, are multiplied, youre bound to attain a value of 10, . Essentially, it follows the scientific method . Note: There are two procedures listed for this part. Procedure 11.2 Observe the effects of pH on catalase activity 1. ____________, Which ion, \(\ce{Zn^{2+}}\) or \(\ce{SO4^{2-}}\), is causing the observed acidity or basicity? conjugate base. Conclusion: Throughout the course of the lab, we utilized an acid-base titration of 10mL of an unknown solution (NaOH) as to determine its molarity. Note this point on your data sheet and stop the titration. meters probe, set up the pH meter so that the probe is supported inside the swirling (OPTIONAL) Use Excel to create a graph or titration curve of pH versus volume of 0.2 M \(\ce{NaOH}\) solution added for your pH titration data. Finally, record the results in the final pH section. solution into the first beaker and 30 mL of 0-M acetic acid solution into the second. Pale Pink Sprite Color with Extract Vinegar Cloudy Pastel Green No Change Dish Detergent Baking Soda Lime Green Ammonia Orange Juice Stayed the same but cloudy Slightly Lighter Brown Coke Table 3: Consists of the color results after the color extract were added to the solutions. Using your large graduated cylinder measure out 25-mL of the solution from the beaker Its important to maintain an understanding that when . 05 Light green Table 2: Consists of color extract taken from a red cabbage for a natural indicator. Part 1: Using a pH Meter (work together as a pair) The first goal for today is to calibrate a typical laboratory pH meter. Finally, you will compare the buffering capacity of the buffer you prepare with that of deionized water. An acid-base indicator is a chemical species that changes color at a Because \([\ce{HA}] = [\ce{A^{-}}]\), the pH of this buffer solution equals the value of pKa for the unknown acid. Adding too much NaOH, to a pH beyond its second pKa results in a colorless solution. You will confirm the pH of this solution using your pH meter. *Thymol blue has two pKa values. determine the percentage error in your measured K a value for each solution. . Then use it to collect about 75 mL of the 0-M NaOH Rinse your buret, small funnel, and four 150-mL beakers several times using deionized water. The pH of unknown solution X is also determined using . Clamp with a strong base, pH = p K a. Add 2 drops of phenolphthalein indicator to the remaining 50-mL of unknown acid value of p K a for the unknown acid. From these two tests we know that the pH range our solution is between 2 and 3. At the midpoint of the titration of a weak acid Before continuing, the pH meter needs to be calibrated. Report, Record this value below. Discard all chemicals in the proper chemical waste container. Results Solution Color WI Promptly blue Color with Phenolphthalein 6 Cloudy White 9 Blue Pink c 5 Yellow 2 11 Slightly Darker Blue Dark Magenta Table 1: Consists of pH levels of each solutions, the result when added indicator dye Promptly blue into solutions, and the result when added indicator dye Phenolphthalein into solutions. Add 2 drops of phenolphthalein indicator to the remaining 50.0-mL of unknown acid solution in the beaker labeled A, Titrate the solution in the beaker labeled A, We now need to equalize the volumes in the two beakers labeled HA and A, Using your large graduated cylinder measure out 25-mL of the solution from the beaker labeled HA and transfer this volume to your fourth clean rinsed 150-mL beaker. 0-M sodium acetate, NaCH 3 COO( aq ) Overview of the Lab Exercise. Conclusion. Continue recording the total volume added and the measured pH following each addition on your data sheet. To measure the pH of various solutions using pH indicators and meter. These meters/indicators can come in different forms, however all in similarity with, the common use of the pH scale. PH of household products. +NH3CH (R)COOH + OH- +NH3CH (R)COO- + H2O. This new solution will be a where \([\ce{HA}]_{0}\) is the initial (nominal) concentration of \(\ce{HA}\) (aq) before equilibrium is established. Use your pH meter to confirm the pH of your buffer solution. Here we are assuming Equation \ref{9} proceeds essentially to completion. This lab report will focus on your evaluation of how temperature and pH affect the rate of enzyme activity. Fill the buret with the 0.2 M \(\ce{NaOH}\) solution from your beaker to. By the pH reading that the pH meter provided, determine which solution from beakers A through E is a base or acid. Record the color of the indicator in each solution on your data sheet. Then, 20 drops were added and gently swirling the beaker to mix the solution and the hydrochloric acid and wait until the pH meter dropped 1. Ph Measurement Lab Report. The pH test is used to determine the acidity of a solution. Adding too much NaOH, to a pH beyond its second pKa results in essentially the same as color I. Save the remaining solutions in the beakers labeled, HA and A and the beaker Throughout the, macro lab procedure, pH meters are bound to be the necessary tool when trying to measure the, values of pH. Using a ring stand and your utility clamp, or the stand and clamp provided with your pH meters probe, set up the pH meter so that the probe is supported inside the swirling solution in your beaker, low enough down that the meter can read the pH, but high enough up so that the probe tip does not contact the rotating magnetic stir-bar, as shown in Figure 1. You will confirm the pH of this solution using Sodium bicarbonate (NaHCO 3) is formed. 56 6. Your measured pH value should be 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 Lab Report. Insert your funnel into the top of the buret. Is the color obtained when tested with bromcresol green indicator as expected? 15. nearing the endpoint, slow down your addition rate to just 1 drop per addition. protonated form of the acid-base indicator, HIn( aq ), will be one color (yellow in this example) The procedure for operating every pH meter is slightly different. To perform a pH titration (OPTIONAL, if time permits). Dip the pH paper into the solution and color coordinate with the pH chart it provides. If the base is off the scale, i. e. a pH of >13. \(K_{a}\) of unknown weak acid: ______________ (, How do you know the concentrations of \(\ce{HA}\) (. Explain your answer: pH of Buffer Assigned by Instructor: ______________, Measured pH of Assigned Buffer: ______________. 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. about 5 mL of 0-M NaOH. When the pink color from the phenolphthalein indicator persists for at least 2 minutes Rinse the 50-mL buret and funnel once with about 5 mL of 0-M NaOH solution. Using indicator dyes. Using your pH meter measure the pH of the deionized water. PH paper (litmus paper) determines how acidic or how basic a substance is. Which ion, Na+ or HSO 4 is causing the observed acidicity or basicity? You will need to tell your instructor this value for A buret stand should be available in the laboratory room. 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 . WASTE DISPOSAL: All chemicals used must go in the proper waste container for disposal. You measure the pH of a 0.50 M unknown acid solution using a pH meter and it is found to be 1.74. You will divide the solution containing this unknown acid into two equal parts. The pKa for the buffer is therefore 5.05. Record the results on your data sheet. Record your measured value on your data sheet This Summarize the findings. 1. As you can see from Equation (1), the unknown acid. present in the solution. Part E. 23. containing the remaining 0-M NaOH solution for the next part of this experiment. Your instructor will Next, by add a drop of hydrochloric acid and gently swirling the beaker until the pH meter dropped 1. Alkalinity, or "acid neutralizing capacity," is measured by adding acid to the sample and figuring out the equivalent alkalinity in the water. of the buret. Label this second beaker HA and set it aside for now. Note that when \([\ce{H3O^{+}}] >> K_{ai}\), \([\ce{HIn}] >> [\ce{In^{}}]\) (the equilibrium will be shifted to the left in accord with Le Chatelier's principle) and the color of the solution will be essentially the same as color I. 48 3. Example of a Lab Report Conclusion. The lab manual may dictate where it should appear. within 0 pH units of your assigned value. Please consult your instructor to see which After testing all the beakers with the pH meter, add 2 drops of cabbage extract (intoxication) to each beaker and mix it well until there is a distinct color. After testing a solution, the student compares the strip color to the scale provided on the container and gives the solution a rating from . 5, then a Thymol Blue indicator may be used. be shifted to the right) and the color of the solution will be essentially the same as color II. buffer solution since it will contain equal amounts of HA( aq ) and A( aq ). Write the net ionic equation below that shows why this ion is acidic or basic: Consider your results for the 0.1 M\(\ce{NaCl}\) solution. Do you know why? Thus, we have determined the pH of our solution to Repeat the same procedure using each of the following solutions: Record your results for each on your data sheet. The actual colors in solution vary somewhat from those shown here depending on the concentration. Then use it to collect about 75 mL of the 0.2 M \(\ce{NaOH}\) solution (available in the reagent fume hood). Follow the procedure below for Part D instead of the steps above if your instructor wants you to also obtain a pH titration curve. . Upon completion of the titration, the Explain. Soapy Water 8 Conclusion In concluding this lab I found that, in general most groups had similar recordings in their lab. Add a small amount of each substance into each container. Use a mortar and pestle to macerate a marble size portion of fresh, raw ground meat in 10mL of distilled water. When you notice these changes slow down your Record your color observations and your determination of the pH range of the 0.1 M \(\ce{HCl}\) solution on your data sheet. In the graph shown, it depicts how the buffer helps to keep the . PH Lab Report. . point. If it does not, the Data Analysis section is a good place to put it. Use equations to support your explanation: Why isnt the measured pH of the deionized water before adding the \(\ce{NaOH}\) (. lab report chemistry 12 santa monica college ph measurement and its applications objectives: to measure the ph of various solutions using ph indicators and . In the lab procedure, it was explained that the concentration of HA and A, You find the \(K_{a}\) of your unknown acid is \(6.3 \times 10^{-5}\). This time, the tool of measurement to find out if the solutions were acidic, neutral or basic will not be pH paper or a pH meter. your unknown acid. 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. D. Tecnolgico de Monterrey Campus Ciudad de Mxico. The second pKa is around 8.8. Your instructor will demonstrate the proper use of the pH meters. Trial 2: 16.03 mL NaOH. In this experiment it is OK if you overshoot this mark by a few drops. This experiment was performed to investigate the following hypothesis: The following four different types of drinking water (spring water, seltzer water, tap . The total amount of \(\ce{H3O^{+}}\) in the solution is therefore controlled by the concentrations of the other acids and/or bases present in the solution. After we test each substance, we recorded the data in a data table. Select one of the 150-mL beakers and label it NaOH. Insert your funnel into the top data sheet. Open Document. PH Lab Report Assignment - Free assignment samples, guides, articles. Paragraph 1: Introduce the experiment. You will then Using your pH meter measure the pH of the deionized water. An acid-base indicator is a chemical species that changes color at a specific pH as the pH (acidity) of the solution is varied. 3. Rinse the tip of the pH pen with tap water between tests. Pages: 12 (3486 words) Introduce the experiment and hypothesis in your conclusion. One part you will set aside and the other part will be titrated with \(\ce{NaOH}\). This tells us that the pH of our solution is less than or equal to 3 because Contents 1- Aim. Ka of unknown weak acid: ______________ ( from midpoint of titration curve ). Then use it to collect about 75 mL of the 0.2 M \(\ce{NaOH}\) solution. it has also been realized that the acidic concentration of the element has at least 0.83 moles with a pH Level of 2.4. Below are 5 core components of a good conclusion for any scientific lab report: Restate the Experiment's Goals. Distillation Lab Report. Weighing by difference measure between 1 and 2 grams of the unknown acid into Course Hero is not sponsored or endorsed by any college or university. Measure the pH of each of these solutions following this addition and determine the change in pH of each. and regions on your graph: the initial point, the midpoint, the endpoint, and the buffer region. water. Thus we can use the midpoint of the titration curve to confirm the value of pKa for the unknown acid. For example, Proceeding in this way, continue to add 0-M NaOH to your solution in approximately and obtain your instructors initials confirming your success. - Phenophtalein: This indicator is really good to detect and measure strong bases. This pH is the initial point in your titration. Students must wear safety goggles and lab coats at all times. Rinse and fill another 150-mL beaker with a volume of deionized water equal to that of your buffer solution. buffer solution is given by the Henderson-Hasselbach equation: Because [HA] = [A], the pH of this buffer solution equals the value of p K a for the unknown acid. Clean up. 3. Eventually as [H 3 O+] decreases still further we will have, [H 3 O+] << K ai, and the color of the Table 1: Acid-Base Indicators Results: For the solutions acid and bases lab the results my group received are as followed. Trial 3: 15.84 mL NaOH. Remove the funnel. When the these solutions. Label this second beaker HA and set it Conclusion . In this experiment it is OK if you overshoot this mark by a few drops. As you can see from Equation \ref{1}, the protonated form of the acid-base indicator, \(\ce{HIn}\) (aq), will be one color (yellow in this example) and the deprotonated form, \(\ce{In^{-}}\) (aq), will be another color (blue in this example). 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