The second reaction that occurred during the acid-base neutralization of the experiment is: NaHSO: (ag) + NaOH (ag) → H20 (1) + Na2SO3 (ag) d. Write the net ionic equation for this reaction. e. What buffering system is present during this reaction? List the formula for the acid component and the base component in the buffer.
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- a.For a weak acid (HA) titration, what are the net ionic reactions for the following processes? i.The hydrolysis (reaction with water) of a pure weak acid (HA) in distilled water. ii.The neutralization reaction between HA and sodium hydroxide. iii.The hydrolysis equilibrium of the conjugate base, A-, with water. b.Besides water, what is the dominant (most concentrated) chemical species for the situations in ai, aii, and aiii? c.Please include a figure showing the generic titration curve and label the regions that correspond to the situations in ai, aii, and aiii.Out of the potential unknowns in this experiment, which one would be the best choice to create a buffer with a pH of 7.0? Note: Copying and/or posting this question without the express written permission from Dr. Burke and the Department of Chemistry & Biochemistry at the University of Delaware is a violation of intellectual property copyright law. Out of the potential unknowns in this experiment, which one would be the best choice to create a buffer with a pH of 7.0? Formic acid Sodium bisulfate Phenol Hypobromous acid Boric acid Sodium bicarbonate Potassium hydrogen phthalate Sodium bisulfite Disodium hydrogen citrate Ascorbic acidWhy does the dilution of the initial sample (say 75 mL versus 100 mL) not affect in the final results of the titration? Select one:a. Because the indicator still works in the diluted sample.b. Because the total moles of hydronium ions in the sample are not changed after dilution.c. All options are incorrect.d. Because the pH for the sample is unchanged after dilution.
- 1. What process is responsible for the increase in the total negative charge as soil pH increases? a.Protonation b. Dehydration reaction c. H+ bond formation d. Deprotonation 2. What ionic form of nutrient would most likely be easily leached/washed out from the soil? a. Cation b. Conjugate ion c. Anion d. Spectator ion 3. When a soil with cation-Ca complexed is poured with distilled water, what would you expect if the leachate will be reacted with ammonium oxalate? a.The leachate will be negative for calcium b. The leachate will manifest a false negative c. The leachate will be positive for Calcium d. The leachate will manifest a false positiveFollowing the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. Consider that the burette was completely filled to the 0 mL mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 21.2 mL C. 21.3 mL D. 22.7 mL 2. What is the unknown weight (grams) in the problem? Your Answer:. Answer the following questions regarding a 50.0 mL solution of 0.100 M solution of a weak acid, HY, Ka = 1.80 x 10-8 . The solution is titrated with o.100 M NaOH. a. Calculate the volume of base needed to reach the equivalence point. b. Calculate the pKa for the weak acid. c. Determine the pH of the original acid solution. d. Sketch a titration curve for this experiment, (You can insert a graph or write on a graph paper paper)
- 11. Which is a highly purified compound that serves as a reference material in titration? A. secondary standard B. indicator solution C. primary standard D. reference solution17. This type of analysis implies that the constituent determined was present in very, very low concentration. a. Macro analysis b. Semi-macro analysis c. Micro analysis 18. Which of the following does not happen during digestion? The crystals dissolve and re-precipitate under equilibrium conditions. b. Weakly bound water are lost from the precipitates. c. Filterability improves d. None of the choicesWhat is the result when these samples are mixed with 5 mL strong alkali NaOH then 1ml ethanol a. vegetable oil b. margarine c. mineral oil
- The Henderson-Hasselbalch equation: a. relates the pH of a solution to the pKa and the concentration of acid and salt. b. allows the graphical determination of the molecular weight of a weak acid from its pH alone. c. is equally useful with solutions of acetic acid and of hydrochloric acid. d. employs the same value for pKa for all weak acids.5. x10-5. A student is preparing a pH buffer solution with 1.663 M NH3 solution and (NH4)₂SO4 solid. Please answer the following questions. A. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815 B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1" if the answer is pH = 4.741 + 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 ± 1, please put down "4" if the answer is pH = 9.26±10. Please provider your answer below. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.67 buffer solution? The volume of the buffer solution is 250.0 mL. grams Please provider your answer below. 0² 0₂ $In this experiment, you titrated H3PO4 with NaOH. When the titration was done, all that remained was Na3PO4. What would the titration curve of 0.10 M Na3PO4 titrated with 0.10 M HCl look like? (Hint: It is related to the Part 2 curve) Draw it on the graph in your lab manual. Take a photo of your work, include your name and date in the photo and insert the photo below.