# To determine the equivalence points of two titrations from plots of ph versus ml of titrant added.

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1 Titration Curves PURPOSE To determine the equivalence points of two titrations from plots of ph versus ml of titrant added. GOALS 1 To gain experience performing acid-base titrations with a ph meter. 2 To plot titration curves of ph vs ml of titrant added. 3 To determine the equivalence point of a titration from a titration curve. 4 To determine the pk a of an analyte from a titration curve. INTRODUCTION A titration 1 is an analytical procedure in which a reaction is run under carefully controlled conditions. The stoichiometric volume of one reactant of known concentration, the titrant, that is required to react with another reactant of unknown concentration, the analyte 2, is measured. The concentration of the analyte is determined from the concentration and volume of titrant and the stoichiometry of the reaction between them. The experimental setup is shown in Figure 1. A buret, which contains the titrant, is calibrated so the volume of solution that it delivers can be determined with high accuracy and precision. Titrant is added to the analyte until the stoichiometric volume of titrant has been added. This is called the equivalence point 3, at which the volume of titrant delivered by the buret is read. Usually, the volume readings are estimated to the nearest 0.01 ml. The delivery of the titrant is adjusted with the stopcock on the buret. With practice, one can dispense fractions of a drop of titrant and control the procedure well enough that replicated titrations agree within 0.10 ml point c Advanced Instructional Systems, Inc. and North Carolina State University 1

2 Figure 1: Titration Setup Often, the equivalence point is determined visually as a color change of an indicator. The indicator, a substance that changes color near the equivalence point, is added to the analyte solution. Since the color change is near but not exactly at the equivalence point, the point at which the color change occurs is called the end point. 4 Indicators are chosen so the endpoint is very close to the equivalence point. It is important to keep a titration well mixed, so the titrant and analyte can contact each other and react rapidly. Either manual swirling of the flask or mechanical stirring can be used. You will use mechanical stirring in this experiment to ensure complete mixing of the solutions. In this experiment, you will compare the predicted equivalence point to the experimentally determined equivalence point of two titrations. The first will be a monoprotic acid, potassium hydrogen phthalate (KHP), titrated with sodium hydroxide (NaOH) and the second will be a disodium salt, sodium carbonate (Na 2 CO 3 ), titrated with hydrochloric acid (HCl). In the first, you will observe only one equivalence point according to the following reaction where P refers to the phthalate ion (C 8 H 4 O 2-4 ). HP (aq) + OH (aq) P 2 (aq) + H 2 O(l) (1) In the second, two distinct equivalence points will be observed as two protons are added stepwise to the carbonate anion (CO 3 2- ) according to the following reactions. 4 %28chemistry%29 c Advanced Instructional Systems, Inc. and North Carolina State University 2

3 CO 2 3 (aq) + H 3O + (aq) HCO 3 (aq) + H 2O (2) HCO 3 (aq) + H 3O + (aq) H 2 CO 3 (aq) + H 2 O(l) (3) The ph will be recorded for the analyte solution as increasing amounts of titrant are added. The plot of ph (y-axis) vs volume of titrant added (x-axis) is called a titration curve. 5 Figure 2: Predicted titration curve of 0.1 M NaC 2 H 3 O 2 titrated with 0.20 M HCl Although indicators will be used in each of the titrations, they are simply for visual assistance. The ph will begin to change rapidly as the equivalence points are approached. Thus, the equivalence points can be detected simply by monitoring the ph of the analyte solution. Also, the equivalence point of the titration can be determined from the titration curve. It is the volume of titrant where the slope of the titration curve is the greatest. You will be asked to compare the endpoints predicted by the indicators to the equivalence points determined from the titration curves. You will also compare the predicted ph for various amounts of titrant added in each titration to the experimentally determined ph s. One of these points is the midpoint. This is where one half of the equivalence volume has been added. It is special because at this volume of titrant added, exactly half of the analyte has been converted into its conjugate pair. At this solution composition, the Henderson-Hasselbalch equation predicts that the ph will be equal to the pk a of the acid species of the conjugate pair. Thus, you will also be able to determine the pk a s of the analytes from the titration curves. These will be equal to the ph of the analyte solution at one half the equivalence volume of titrant added. You will compare the pk a values for both phthalic acid and carbonic acid found in reference tables to those determined from your titration curves. Another point where the calculated ph will be compared to the measured ph is the first 5 curve c Advanced Instructional Systems, Inc. and North Carolina State University 3

4 equivalence point of the diprotic titration curve. At this point, the amphoteric 6 intermediate species is the only species present. In the case of the carbonate (CO 3 2- ) titration, the intermediate species is hydrogen carbonate or bicarbonate (HCO 3 - ). Because this species can act as both an acid and a base, both equilibria must be considered. HCO 3 (aq) + H 2O(l) CO 2 3 (aq) + H 3O(aq) (4) HCO 3 (aq) + H 2O(l) H 2 CO 3 (aq) + OH (aq) (5) To mathematically solve this system rigorously, it would involve solving five equations and five unknowns simultaneously! However with a few assumptions, the result is quite simple. At the first equivalence point of a diprotic titration curve, the ph is the average of the pk a s for that diprotic acid. ph = 1/2(pK a1 + pk a2 ) (6) Use this equation for any solution containing only the intermediate form of a diprotic acid. For example, a solution of KHP, which you begin with in Part B. Phthalic acid is H 2 P and HP - is the intermediate form. Remember this when you are doing your prelab calculations! As a reminder on concentration units: molarity is defined as the number of moles of solute in a liter of solution. This is numerically equal to the number of millimoles of solute in a milliliter of solution. It is often convenient to use this second definition of molarity in titrations and other work where small quantities are involved. Note that the volume measurements in titrations are usually reported to four significant figures, so the concentrations are usually reported to four significant figures as well. Watch this in your work. EQUIPMENT 1 MicroLab Interface 1 MicroLab ph Measurement Instruction Sheet 6 c Advanced Instructional Systems, Inc. and North Carolina State University 4

5 1 ph electrode in ph 7.00 buffer 2 30 ml beakers 2 50 ml beakers ml beaker ml graduated cylinder ml volumetric pipet 1 pipet bulb 1 magnetic stir plate 1 magnetic stir bar 1 25 ml buret 1 ring stand 1 clamp 1 buret clamp ml beaker for electrode rinsings 1 deionized water squirt bottle 1 box of Kimwipes REAGENTS 25 ml 30 ml 0.20 M potassium hydrogen phthalate (KHP) 0.20 M sodium hydroxide (NaOH) 3 drops phenolphthalein solution 25 ml 0.10 M sodium carbonate (Na 2 CO 3 ) 30 ml 0.20 M hydrochloric acid (HCl) 3 drops methyl orange solution 15 ml 15 ml 15 ml 200 ml ph 4.00 buffer ph 7.00 buffer ph buffer deionized water c Advanced Instructional Systems, Inc. and North Carolina State University 5

7 Immediately prior to use, the electrodes are rinsed with deionized water and gently blotted with a tissue, then placed in the test solution. The electrodes are rinsed and blotted again after the measurement and returned to the ph 7 buffer solution. Part A: Calibrating the MicroLab ph Electrode 1 Open the MicroLab program. 2 Make sure the ph electrode is plugged into the interface. 3 Calibrate the ph electrode using the MicroLab instructions provided in the lab. The calibration standards for the ph electrode will be a ph = 4.00 (red) buffer solution, a ph = 7.00 (yellow) buffer solution, and a ph = (blue) buffer solution. Use about 15 ml of each in 30 ml beakers. 4 After the calibration is complete, continue with the MicroLab instructions provided. The program will be configured to accept a volume of titrant, read from the buret, for each ph measurement. 5 For each ph reading, you will be prompted for a keyboard entry; enter the total volume of titrant as read from the buret. Make sure the electrode is immersed in the solution and allow for a few seconds equilibration. Part B: Titration of KHP with NaOH 1 Using a clean, dry 50 ml beaker, obtain about 25 ml of 0.20 M potassium hydrogen phthalate (KHP) solution. Record the exact concentration of the KHP in Data Table A. 2 Condition a ml volumetric pipet with KHP solution as shown in the Pipeting Techniques video under Instructional Videos and as described in the Volumetric Glassware section of the Introductory Material in this lab manual. 3 Pipet ml of the potassium hydrogen phthalate (KHP) solution into a 250 ml beaker, and add 100 ml of deionized water (graduated cylinder) and 3 drops of phenolphthalein indicator. 4 Obtain about 30 ml of 0.20 M NaOH solution in a clean, dry 50 ml beaker. Record the exact concentration of NaOH in Data Table A. 5 Condition the 25.0 ml buret with NaOH solution as shown in the Conditioning a Buret video and as described in the Volumetric Glassware section of the Introductory Material in this lab manual. 6 Fill the buret with NaOH and carefully clamp it with the buret clamp to the ring stand. 7 Carefully slide the stir bar into the 250 ml beaker while tilted to avoid splashing or damage to the beaker. Position the stir plate under the 250 ml beaker and begin stirring slowly. c Advanced Instructional Systems, Inc. and North Carolina State University 7

12 Question 8: How did the endpoint indicated by the methyl orange compare to the equivalence points determined by the titration curve? What conclusion can you make about the need for an indicator in a ph titration? 23 Before leaving, enter your results in the in-lab assignment. If all results are scored as correct, log out. If not all results are correct, try to find the error or consult with your lab instructor. When all results are correct, note them and log out of WebAssign. The In-Lab assignment must be completed by the end of the lab period. If additional time is required, please consult with your lab instructor. c Advanced Instructional Systems, Inc. and North Carolina State University 12

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### Lab #11: Determination of a Chemical Equilibrium Constant

Lab #11: Determination of a Chemical Equilibrium Constant Objectives: 1. Determine the equilibrium constant of the formation of the thiocyanatoiron (III) ions. 2. Understand the application of using a

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CHM 130LL: ph, Buffers, and Indicators Many substances can be classified as acidic or basic. Acidic substances contain hydrogen ions, H +, while basic substances contain hydroxide ions, OH. The relative