1. A pH change of 0.2 units requires the addition of 0.05 mL of NaOH. You are probably at what point in the titration?a. very close to equivalence pointb. after equivalence pointc. either before or after the equivalence pointd. before equivalence point2. A pH change of 0.2 units requires the addition of 1.50 mL of NaOH. You are probably at what point in the titration?a. after equivalence pointb. either beforeor after the equivalence pointc. very close to equivalence pointd. before the equivalence point3. Looking at the graph provided, which of the following indicators could be used to find the equivalence point for this titration the conventional way? Select all that apply.a. methyl orange (turns red to yellow from a pH of 3.1 to 4.4)b. methyl red (turns red to yellow from a pH of 4.2 to 6.3)c. cresol red (turns yellow to red from a pH of 7.2 to 8.8)d. thymol blue (turns yellow to red form a pH of 8.0 to 9.6)e. phenolphthalein (turns colorless to dark pink from a pH of 8.3 to 10.0)f. alizarin yellow R (turns yellow to orange -red from a pH of 10.1 to 12.0)4. In a potentiometric titration is the titration stopped as soon as the equivalence point is reached? Why or why not?a. No. The 2-4 mL portions of base should be added until a buret is empty. Otherwise the experiment is not completed.b. Yes. There is no need to continue the titration after the equivalence point is reached because only the equivalence point is the essential information in this experiment.c. No. Five or six more portions of 2-4 mL portions of base should be added otherwise the equivalence point cannot be determined accurately from the graph.5. Does it matter how much water is used to dissolve the unknown monoprotic acid? Explain your answer.a.Yes. Adding a higher (or lower) amount of water would change the number of moles of the unknown monoprotic acid in the solution, so the equivalence point will be reached at different pH.b. No. Adding water does not change the number of moles of the unknown monoprotic acid, so the amount of water is insignificant.c. Yes. Adding a higher (or lower) amount of water would change the initial concentration of unknown monoprotic acid, so the equivalence point will be reached at different pH. point.12. After the equivalence point is passed (about 1 mL of base is again required to change the pHby 0.2 units), continue the titration for 5 or 6 more readings.13. After you are finished with the titration, rinse the buret by filling it with deionized water andallowing it to drain.14. Plot your titration curve. (This has been done for you. See data and graph)15. From the graph find the pH and volume at theequivalence point.Data16. From the graph find the pH at the half-equivalence point.Volume of NaOH (mL)pH3.117. Complete all the calculations and questions.2.23.555.43.944.164.344.544.747.910.112.414.616.34.9417.85.1618.719.85.375.7720.15.9620.256.146.366.66.7820.420.620.720.87.067.237.467.848.439.369.7810.0320.8520.920.952121.0321.0621.121.1510.2221.210.4521.310.6521.4521.6221.922.310.8711.111.3111.5511.7322.823.825.75283211.9812.212.3912.5812.7837.448.612.97 2. Obtain a pH meter, a magnetic stirrer, a buret, and about 100 mL of the standard NaOH.Note the molarity of the base and record. (given)3. Standardize the pH meter using buffers 4, 7, and 10.4. Using an analytical balance obtain about 0.2500 g of an unknown monoprotic acid in a 400 -mL beaker. Record the exact mass to 4 decimal places. (given)Dissolve the acid inwater.5. To clean the buret rinse with deionized water. With the stopcock closed, add some deionizedwater to the buret. Tip and roll the buret, allowing the water to have contact with all of theinside surfaces. Open the stopcock and allow the water to drain. If the water drains withoutleaving any droplets on the side, repeat the rinse one more time. If droplets remain on theinside surface, wash the buret with detergent solution, rinse several times with tap water, thenrinse twice with deionized water.6. After rinsing the buret with deionized water, close the stopcock and add about 5 mL of theNAOH solution. Again, roll and tip the buret so the solution has contact with all the insidesurfaces. Open the stopcock and allow the solution to drain. Discard the rinse. Repeat thisstep.7. Fill a clean buret with the standard NaOH to above the 0.00 mL mark. To remove air bubblesfrom the tip of the buret, quickly drain out the NaOH until the bottom of the meniscus is atthe 0.00 mL mark.8. Set up the apparatus as shown below. Make surethat the stirring bar in the beaker does not strikethe electrodes when the magnetic stirrer is turnedon. (When inserting or removing electrodes,always make sure to turn the pH meter toSTANDBY and always shut off the magneticstirrer.)-Buret containingNaOH(aq) of knownconcentration9. Record the initial pH of the solution.10. Run about 4 mL of base into the beaker. Recordthe buret reading and the pH. Repeat this step twomore times.pH meter11. Now add the base until the pH changes by 0.2units. At first this may require about 1 mL of basebut eventually you will only need one drop (0.05mL) of base to change the pH by 0.2 units aremore. You are now approaching the equivalenceBeaker containingsolution of unknownacid

Since you have asked multiple questions, we will solve the first question for you. If you want any…

1. A pH change of 0.2 units requires the addition of 0.05 mL of NaOH. You are probably at what point in the titration? a. very close to equivalence point b. after equivalence point c. either before or after the equivalence point d. before equivalence point 2. A pH change of 0.2 units requires the addition of 1.50 mL of NaOH. You are probably at what point in the titration? a. after equivalence point b. either beforeor after the equivalence point c. very close to equivalence point d. before the equivalence point 3. Looking at the graph provided, which of the following indicators could be used to find the equivalence point for this titration the conventional way? Select all that apply. a. methyl orange (turns red to yellow from a pH of 3.1 to 4.4) b. methyl red (turns red to yellow from a pH of 4.2 to 6.3) c. cresol red (turns yellow to red from a pH of 7.2 to 8.8) d. thymol blue (turns yellow to red form a pH of 8.0 to 9.6) e. phenolphthalein (turns colorless to dark pink from a pH of 8.3 to 10.0) f. alizarin yellow R (turns yellow to orange -red from a pH of 10.1 to 12.0) 4. In a potentiometric titration is the titration stopped as soon as the equivalence point is reached? Why or why not? a. No. The 2-4 mL portions of base should be added until a buret is empty. Otherwise the experiment is not completed. b. Yes. There is no need to continue the titration after the equivalence point is reached because only the equivalence point is the essential information in this experiment. c. No. Five or six more portions of 2-4 mL portions of base should be added otherwise the equivalence point cannot be determined accurately from the graph. 5. Does it matter how much water is used to dissolve the unknown monoprotic acid? Explain your answer. a.Yes. Adding a higher (or lower) amount of water would change the number of moles of the unknown monoprotic acid in the solution, so the equivalence point will be reached at different pH. b. No. Adding water does not change the number of moles of the unknown monoprotic acid, so the amount of water is insignificant. c. Yes. Adding a higher (or lower) amount of water would change the initial concentration of unknown monoprotic acid, so the equivalence point will be reached at different pH.