Use the following information to answer the next question Kai's Titration of 25.0 mL of NaHCO3 (a) with 0.352 mol/L HCl(aq) Trial 1 2 3 4 Final volume (mL) 16.5 31.8 47.0 16.4 Initial volume (mL) 0.6 16.5 31.8 1.2 Volume of HCl) used (mL) Color at endpoint Yellow Green Green Green (bromothymol blue) 21. Based on the given data above, what is the concentration of NaHCO3 in this titration? 0.578 mol/L- 0.571 mol/L 0.214 mol/L 0.217.mol/L

Use the following information to answer the next question Kai's Titration of 25.0 mL of NaHCO3 (a) with 0.352 mol/L HCl(aq) Trial 1 2 3 4 Final volume (mL) 16.5 31.8 47.0 16.4 Initial volume (mL) 0.6 16.5 31.8 1.2 Volume of HCl) used (mL) Color at endpoint Yellow Green Green Green (bromothymol blue) 21. Based on the given data above, what is the concentration of NaHCO3 in this titration? 0.578 mol/L- 0.571 mol/L 0.214 mol/L 0.217.mol/L

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 3ASA: A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to...

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A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Which of the following is TRUE about titration employing spectrophotometric method? O Spectrophotometric method is less precise than visual endpoint titration. O Spectrophotometric method allows the use of colored solutions only. O Spectrophotometric method is not applicable to reactions that have unfavorable equilibrium constants. O None of the above
Aqueous Equilibria Strong Acid/ Strong Base Titrations H 14 13 12 11 Phenolphthalein color- change interval 10 9 8 pH 7 Equivalence point 2 Steps for Strong Acid/Strong Base Titrations: 1. 2. Methyl red color- change interval 3. 0 10 20 30 40 50 60 70 80 mLNaOH Na+ Initial acid Remaining acid Example: Calculate the pH when the following quantities of 0.200 M NaOH solution have been added to 50.0 mL of a 0.100 M HCI solution. a. O mL NaOH b. 10 mL NaOH c. 25 mL NaOH d. 40 mL NaOH
Last 3 parts please D ,E ,F
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29 In GC, the sample injected in liquid state vaporizes inside the column. * True False 30 In GC, the sample is carried through the column by inert gas. True False
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
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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
Calculate the pH during the titration of 50.00 mL of0.0500 M NaOH with 0.100 M HCl at 25oC after theaddition of the following volumes of reagent:a. 0.00 mLb. 10.00 mLc. 15.00 mLd. 20.00 mLe. 24.5 mLf. 25.00 mLg. 25.5 mLh. 27 mL
In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 2: Methyl red: pH transition = 4.8-6.0 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 4: Thymolthalein: pH transition = 8.5-10.5 O Indicator 5: Indigo Carmine: pH transition= 11.6- 14.0 O Indicator 3: Cresol red: pH transition = 7.2-8.8
M of NaOH: 0.100 Volume of HCI 25mL = 0.025L Moles of HCI = 2.5 mol What is the Volume of NaOH equivalence point: What is Moles of NaOH equaivalence point: What is pH at equivalence point? What is calculated pH and experimental pH of NaOH at 0.00 mL , 12.50 mL, 25mL, and 30 mL. Also what is the Error percentage for each one?