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- One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used? please explain than solveChoose the equation that correctly describes the relationship between the volume during the end point (Vend) and the volume during equivalence point (Veq) of titrimetric analysis of CH₃COOH (acetic acid) using a phenolphthalein indicator? Vend ≤ Veq The information is insufficient Vend = Veq Vend ≥ Veq5. One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?
- Match the type of titration involve Choices: A. Iodimetry B. Acidimetry C. Argentometry D. Iodomtetry E. Complexometry F. Alkalimetry E. Permanganimetry Questions: 1. Determination of percent acetic acid in vinegar 2. Determination of percent carbonate in pearl ash 3. The amount of ascorbic acid in Vitamin C 4. Determination of biochemical oxygen demand by Winkler method 5. Determination of oxalate in oxalic acid by permanganate 6. Determination of chloride content in water 7. Total hardness of waterIn the potentiometric titration of phosphoric acid, pH readings at the first and second half-equivalence points were pH1 = 2.12 and pH2 = 7.21 respectively. Determine the Ka1 and Ka2 for phosphoric acid, rounded to 3 sig figs. At the half-equivalence points, pH = pKa. Also, pH = –log [H+] and pKa = –log Ka. Type your answers one below the other. Use formatting tools where applicable.Data Analysis Base on your titration curve, read the volume of NaOH and pH at the equivalence point (the midpoint of the vertical section of the curve) mLof NaOH at equivalence point: _______________________________ pH: ____________________________ Calculate the volume of at the half equivalence point (1/2 of the mL at equivalence point): _____________________________ Read the pH at the half equivalence point: ____________________________ For a weak acid, the value of pH at the half equivalence point equals pKa of the weak acid. pKa of the weak acid is: __________________________ Identify the unknown acid with pKa and molar mass using the following table. Acid pKa Chemical formula Crotonic 4.69 C4H6O2 Methylmalonic 3.07 C4H6O4 Diphenylacetic 3.94 C14H12O2 Picric ~0.4 C6H3N3O7 Alloxanic 6.64 C4H4N2O5 methyl-m-aminobenzoic 5.10 C8H9NO2 The unknown acid is : ____________________________
- (Answer highlighted question please) Calculate the pH for each of the cases in the titration of 25.0 mL25.0 mL of 0.180 M0.180 M pyridine, C5H5N(aq)C5H5N(aq) with 0.180 M0.180 M HBr(aq)HBr(aq). The ?bKb of pyridine is 1.7×10−9. after addition of 18.0 mL18.0 mL of HBrpHA sample may contain NaOH, sodium carbonate and sodium bicarbonate, alone or in compatible combination. Titration of a 50.00 mL aliquot of the sample to a phenolphthalein end point required 8.50 mL of 0.0905 M HCl. A second 50.00 mL aliquot required 22.40 mL of the HCl when titrated to a methyl red end point. Calculate the molar concentration of the base component/sA 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055MNaOHsolution using phenolphthalein as theindicator. (a) If 19.60mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? At the end-point, the volume of NaOH consumed was found to be 32.00 mL. The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)
- Table 12.5 (data) Indicator Color in 0.05 M HCl Color in 0.05 M NaOH Methyl red Bromcresol Phenolphthalein Methyl orange Methyl violet Table 12.6 (report) Indicator showing very distinct color difference in acid and base Indicator showing only slight color difference in acid and baseAn automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?13,How many milliliters of 0.0854 M NaOH are required to titrate 25.00 mL of 0.1250M HI to the equivalence point? Group of answer choices A, 17.08 B, 17.1 C, 36.6 D, no correct answer E, 36.593