= 6 10 Hi = 3 In hydrogen. Paschen b. Based on the Bohr model of the atom, calculate the ionization energy for a single IS TO Eicrgy Per mule lUI photunsS TUI the trdlisitiun i 6o N = 3 In hydrogen. if the electron begins in the n = 2 level. %3D
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- A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
- 1. A student titrates 25.0 mL of an unknown base with 0.10 M HCI. During the titration the pH is monitored and the collected data is recorded. These data are shown in the table at the right. a. Use the information provided to draw a titration curve showing the pH as a function of the volume of added HCI. Be certain to label your axes. b. Identify the equivalence point on your graph and justify your selection of this particular point. c. Use the data to determine the Kö value for the weak base. Be certain to show the mathematical steps you take to arrive at the answer. Report your final answer to the correct number of significant digits. d. The student has three indicators that she could use for this experiment. The indicators (with their endpoints) are: Bromophenol Blue (3.0 - 4.6), Methyl Red (4.2 – 6.3), and phenolphthalein (8.3 – 10.0). Which indicator would be appropriate for this titration? Justify your selection. e. Determine the (i) molarity and the (ii) % ionization of the…For the following data:*attached a. What volume of HCl was added in order to reach the equivalencepoint?EXAM 1 CHEMISTRY 1308 FALL 2020b. What is the original concentration of the 50.0 mL of NaOH solution?c. What was the original concentration of the HCl used in the titration?250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A. B. A pH buffer solution contains 1.747 mole CH3COOH and 1.630 mole CH3COONa. The volume of the pH buffer solution is C. What is the pH of the solution? pH = Please provider your answer below. 0² 0₂ $ If you add 5.000 mL, 1.998 M of HC1 to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Please provider your answer below. → П $ П If you add 5.000 mL, 1.998 M of Ba(OH)₂ to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Please provider your answer below. $
- 8. The following titration data was collected in a lab. Based on the results, determine the concentration of the aqueous sulfuric acid acid. Concentration of NaOH used: 0.50 M Volume of NaOH used: 50.0 mL Indicator: phenolphthalein Endpoint color change: olorless to pale pink Table 1 Volume of sulfuric acid Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 31.28 39.17 46.70 Initial reading 1.18 9.08 16.62 Volume H2SO4 used (mL)Titration of Acids and Bases fa Vola!! Part B. Determination of the molar concentration of an unknown acid. Volume of unknown acid used (mL) Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) an unknown and Molarity of unknown acid Trial 1 10mL 9.6 mL 0.5mL 9,1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10mL 18,9 Trial 3 Average molarity of unknown acid solution: 10mL 28.3mL 9.6 ml 18,9ml 9,3m² 9.4mL mol NaOH used? M N₂OH = M acid= .1 Gril n.1 To multiple decimalsA 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH. A) Calculate the pH at 0 mL of added base. Express your answer using two decimal places. B)Calculate the pH at 5 mL of added base. Express your answer using two decimal places. C) Calculate the pH at 10 mL of added base. Express your answer using two decimal places. D) Calculate the pH at the equivalence point. Express your answer using two decimal places. E)Calculate the pH at one-half of the equivalence point. Express your answer using two decimal places. F) Calculate the pH at 20 mL of added base. Express your answer using two decimal places. G) Calculate the pH at 25 mL of added base. Express your answer using two decimal places.
- Titration of Acids and Bases Part B. Determination of the molar concentration of an unknown acid. Molarity of N₂OH = .09M ☆ Volume of unknown acid used (mL) Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mb Moles 9.6 mL 0.5mL 9.1mL (OH) Sample calculations for molarity of unknown acid solution: Trial 2 10mL 18,9 Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 9.6 ml 18.9ml 9,3mL 9.4mL mol NaOH used? M N₂OH = M acid = .1 Gril To multiple decimals1. Dilution of NaOH Solution: Molarity of NaOH stock solution 1000M Volume of the NaOH stock solution used for dilution. 10,00mL Total volume after dilution. 250,0mL Molarity of diluted (standard) NAOH solution (SHOW YOUR CALCULATION) 2. Titration: Determination of Molarity of Sulfuic Acid (H,SO4) Volume of the sulfuric acid used in titration: ..10,00ML... ...10,00mL ...10,00mL ..... ww ww Volume of NaOH used in titration: ...15,30mL.... ...14,50mL.... ...14,30mL.... ww Average volume of NaOH used in 3 titrations: ..14,70mL.... Molarity of the sulfuric acid (WRITE CHEMICAL EQUATION AND SHOW YOUR CALCULATION):Exactly 24.57 mL of 0.045 M strong acid is added to a 25.00 mL sample of a 0.044 M weak base solution. What is the pH at this point in the titration? Ky for the base is 4.62x10-4. REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS. Type your answer...