Since A is known to be a weak base we know that Kb << 1 and therefore Kc >> 1. 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. Carefully, added 1 drop of hydrochloric acid into the solution of distilled water until the pH dropped 1. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic. When you notice these changes . Finally, you will compare the buffering capacity of the buffer you prepare with that of deionized water. 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"). Clean and then return all borrowed equipment to the stockroom. 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 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. H 3 O+ in the solution is therefore controlled by the concentrations of the other acids and/or bases Explain. However, the same way that pH and POH are inversely, related, so are these. The term "pH" is short for "potential of hydrogen.". Please consult your instructor to see which procedure is appropriate for your lab section. It also covers impact of these drivers and restraints on production for 4D Printing manufacturing marke Example of a Lab Report Conclusion. One part you will set aside and the other part will be titrated with \(\ce{NaOH}\). Program. Now using the remaining solutions in the beakers labeled HA and A, prepare a buffer 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. 22 20 drops Table 4: Consists of pH levels in distilled water solution and Alkali-Seltzer tablet in distilled water solution. of the buret. First you will learn aboutthe general operating techniques used with a pH meter and calibrate the meter at pH 10. Before continuing, the pH meter needs to be calibrated. 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. After testing a solution, the student compares the strip color to the scale provided on the container and gives the solution a rating from . 26 Light Pink 2. You will need to tell your instructor this value for all borrowed equipment to the stockroom. Comparing the colors with other tables, the end result of the solutions being acidic, basic or neutral. pH of 50-50 buffer solution: _____________, Ka of unknown weak acid: _____________ ( from measurement of 50-50 buffer solution ). Dispense approximately 0.5-mL of the 0.2 M NaOH solution from your buret into your beaker. You will then combine Which of the following 0.1 M solutions will have the highest pH: acetic acid, \(\ce{HCl}\), ammonium chloride, \(\ce{NaH2PO4}\)? and therefore, [HIn] >> [In]. 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. 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. Record this value below. 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? Proceeding in a similar manner, you will use the acid-base indicators in By comparing the colors to table 1 and 2 determine if the solutions are acidic, basic or neutral. Include and Analyze Final Data. In other words the solution will change color when \([\ce{HIn}] [\ce{In^{}}]\), and so \(K_{ai} = [\ce{H3O^{+}}]\), or \(pK_{ai} = pH\). The second pKa is around 8. By the pH reading that the pH meter provided, determine which solution from beakers A through E is a base or acid. Solutions that have a high pH level or above 7 are considered basic. Summary. 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. An acid-base indicator is a chemical species that changes color at a Is the solution acidic or basic?____________, Which ion, \(\ce{Na^{+}}\) or \(\ce{HSO4^{-}}\) is causing the observed acidicity or basicity?____________. 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. Thus we can use the measured pH of this buffer solution to determine the value of pK a for our unknown acid. procedure is appropriate for your lab section. Record these values on your 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. PH Lab Report Assignment - Free assignment samples, guides, articles. the titration. and obtain your instructors initials confirming your success. Using your large graduated cylinder, measure out 50 mL of your unknown acid solution I'm a waste water treatment professional as I gained experience in waste water treatment industry working as a Lab Assistant under R & D department at BPC/NEPL Site, Ahmedabad. Rinse the 50-mL buret and funnel once with about 5 mL of 0.2 M \(\ce{NaOH}\) solution. These data will be used to plot a titration curve for your unknown acid. . Create an outstanding lab report conclusion that is unique but reflects the actual . solution will have turned to blue. Since \(\ce{A^{-}}\) is known to be a weak base we know that \(K_b << 1\) and therefore \(K_c >> 1\). The titration with NaOH occurs in two stages as shown in the equations below. 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. Please consult your instructor to see which Continue recording the total volume added and the measured pH following each addition on your data sheet. Record the results on your data sheet. In this part of the experiment you will use your pH meter to measure the pH of two acetic acid solutions of known concentration. The ones we have in lab are fairly self-explanatory so we would like you to independently figure out how to calibrate the lab pH meters. 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. Explain. assign you the pH value of the buffer solution you will prepare in this part of the experiment. Write the chemical equation describing the equilibrium reaction between acetic acid and water: Show your calculations (using an equilibrium or ICE table) for obtaining the value of \(K_{a}\) for the 0.010 M solution (only): Record your results below. This new solution will be a In other words the solution will change color when Record this value below. amount of the 0-M NaOH you added during your titration and add this volume of It can detect also weak bases, but mostly, strong. Pages: 12 (3486 words) Then use it to collect about 75 mL of the 0-M NaOH Trial 2: 16.03 mL NaOH. Using Initially starting at a pH of . A buret stand should be available in the laboratory room. with a strong base, pH = p K a. 3 1 drop Beaker Initial pH Final pH Drops HCI Added Alkali-Seltzer 6. At the midpoint of the titration of a weak acid 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. will ensure [A] in the titrated solution is equal to [HA] in the HA solution. Continue to record the volume added and the pH after each addition. Record Use your pH meter to determine the pH of each solution. If it is found that a substances pH is equal to 7, then its determined to have a neutral pH. The study includes drivers and restraints of the global 4D Printing Market. directly enter the beaker during the titration. Its important to maintain an understanding that when . Use your pH meter to determine the pH of each solution. You will then use this curve to find the midpoint of the titration. Soapy Water 8 Conclusion In concluding this lab I found that, in general most groups had similar recordings in their lab. Finally, summarize the results and implications of the study. laboratory room. Converting alkalinity from eq/L to "mg/L as CaCO3" takes into account that one mole of . POH is set to be the inverse relationship to pH and its known to, concentrate on the OH ions contained in a substance. the buret tip dropwise until the bottom of the meniscus of the NaOH solution in the buret Record these values on your data sheet. Procedure 11.2 Observe the effects of pH on catalase activity 1. 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. each addition on your data sheet. acid. using deionized water. Using unknown acid. Rinse your buret, small funnel, and four 150-mL beakers several times using deionized water. shifted to the left in accord with Le Chatelier's principle) and the color of the solution will be Pages: 1 . Label Insert your funnel into the top of the buret. . Using your large graduated cylinder, measure out exactly 100.0 mL of deionized water. Students looking for free, top-notch essay and term paper samples on various topics. Extract of sample "PH Determination of Solutions". changes color at a pH determined by the value of K ai or p K ai for that particular indicator. 1. if this pH is less than neutral. - Genaro. Put 30 mL of 1-M acetic acid Obtain a magnetic stirrer, magnetic stir-bar, and 50-mL buret from the stockroom. use this curve to find the midpoint of the titration. titrated solution will contain only the conjugate base of the weak acid according to. 0.1 M sodium hydrogen phosphate, \(\ce{NaH2PO4}\) (aq). Place the magnetic stir-bar into the solution in the beaker labeled A. Record your color observations and your determination of the pH range of the 0.1 M \(\ce{HCl}\) solution on your data sheet. A good lab report abstract is concise usually no more than 200 words. Your graph should have an appropriate title and labeled axes with an appropriate scale. Part E. nearing the endpoint, slow down your addition rate to just 1 drop per addition. Stir your solution to completely dissolve the solid acid. this time, the pink color from the phenolphthalein indicator will also begin to persist in Base 8. Essentially, it follows the scientific method . You will confirm the pH of this solution using This new solution will be a buffer solution since it will contain equal amounts of \(\ce{HA}\) (aq) and \(\ce{A^{-}}\) (aq). 14 Very Pale Pink Acid/Base/Neutral pH Reading Color of Extract Acid 4. within one pH unit. Fill the buret with the 0-M NaOH solution from your beaker to just above the 0-mL The concentration of specific ions are to be used to understand, the characteristics between acids and bases and this is performed before any values are put, through a logarithmic function. You will then combine equal volumes of these two solutions in order to form a new solution. Take all safety precautions necessary and prepare your materials. Combine this with the unknown solid acid sample in your 150-mL beaker. 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. Thus, we have determined the pH of our solution to within one pH unit. This work, titled "Ph lab report assignment" was written and willingly . For either procedure you will perform a titration on an unknown acid. 5, then a Thymol Blue indicator may be used. To create and study the properties of buffer solutions. In part 4 of this experiment, you are asked to prepare a solution in which the concentration of a weak acid is equal to the concentration of its conjugate base. As an example consider an acidic solution containing the indicator \(\ce{HIn}\) where \([\ce{H3O^{+}}] >> K_{ai}\), and therefore, \([\ce{HIn}] >> [\ce{In^{}}]\). 0-M solution (only): Record your results below. 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. the value of the pH at the midpoint of your graph to determine the value of K a for your unknown Additional materials, such as the best quotations, synonyms and word definitions to make your writing easier are also offered here. If time allows you will measure the pH as a function of the volume of \(\ce{NaOH}\) solution added in the titration. Students investigate the pH level of household substances by testing a variety of common compounds. In general we can say that an acid-base indicator changes color at a pH determined by the value of \(K_{ai}\) or pKai for that particular indicator. You may assume that this acid is a weak monoprotic acid. 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}. What 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 pH of unknown solution X is also determined using . containing the remaining 0-M NaOH solution for the next part of this experiment. Around this time, the pink color from the phenolphthalein indicator will also begin to persist in solution longer before vanishing. Now we will test the buffer solution you prepared against changes in pH. 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. value in your data table alongside the measured volume. By taking 7 small beakers and half filling it individually with the appropriate solutions, color extract was added to make out what color it will turn the solutions. The easiest part was checking the pH of the substances. You will divide the solution containing this unknown acid into two equal parts. Lab Report 1 - Free download as PDF File (.pdf), Text File (.txt) or read online for free. 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 the buret to the buret stand making sure that it is vertical. 0-M NaCl 0 M-Na 2 CO 3 0 M-CH 3 COONa 0 M NaHSO 4 0 pH unit. All plants received the same amount of sun exposure in the laboratory. You will need the following additional items for this experiment: pH meter, magnetic stirrer and stir-bar, 50-mL buret. 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