pls compute pH using Henderson equation. Ka = 1.8 x 10^-5 for 2a-2c, Kb = 1.8 x 10^-5 for 4a-4c Observed Color &ClassificationVolume ofSolutionMeasured pH Visual Indicator usi Color observed (subject Estimated pH range(acidic/basic & buffer/solution)solutionmoles of NaOH/HCI addedKa/KbCalculated pH10 mlOrange 3.1 < pH < 4.5Yellow Orange 3.1 < pH < 4.5Yellow pH > 4.5three drops of 1.0 M HCI solutionthree drops of 1.0 M NAOHnone2a4.73mixture of 15.0 mL 0.20 M10 ml2b4.82CH3COOH and 15.0 mL 0.20 M NACH3C0010 ml2c4.76 methyl orangelyellowbasic solution10 ml Classification(acidic/basic & buffer/solution)Observed Color &Volume ofSolutionMeasured pH Visual Indicator us Color observed (subject Estimated pH rangesolutionmoles of NaOH/HCI addedKalKbCalculated pH1a1b1c2a2b2cЗа3bVery light pink 8.3 < pH < 10.0Light Pink 8.3 < pH < 10.0Light Pink 8.3 < pH < 10.010 ml10 ml10 mlthree drops of 1.0 M HCI solutionthree drops of 1.0 M NaOH4a9.139.389.30 phenolphthaleinmixture of 15.0 mL of 0.20 M4bNH3 and 15.0 mL of 0.20 M NH4CI4clight pinkbasic buffernone

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Classification (acidic/basic & bufferisolution) Observed Color & Volume of Solution Calculated pH solution 10 ml Measured pH Visual Indicator usi Color observed (subject Estimated pH range Imoles of NaoH/HCI added Ka/Kb 4.73 4.82 4 76lmethid oranne Orange 3.1 < pH < 4.5 Yellow Orange 3.1 < pH < 4.5 Vellow pH 45 10 ml 10 ml 10 ml three drops of 1.0 M HCI solution three drops of 1.0 M NAOH 2a mixture of 15.0 mL 0.20 M 2b снзсоон аnd 15.0 mL 0.20 MNaCHзсоо vellow haric solutinn Inone

Classification (acidic/basic & bufferisolution) Observed Color & Volume of Solution Calculated pH solution 10 ml Measured pH Visual Indicator usi Color observed (subject Estimated pH range Imoles of NaoH/HCI added Ka/Kb 4.73 4.82 4 76lmethid oranne Orange 3.1 < pH < 4.5 Yellow Orange 3.1 < pH < 4.5 Vellow pH 45 10 ml 10 ml 10 ml three drops of 1.0 M HCI solution three drops of 1.0 M NAOH 2a mixture of 15.0 mL 0.20 M 2b снзсоон аnd 15.0 mL 0.20 MNaCHзсоо vellow haric solutinn Inone

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.33QAP

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Which indicator using in .complexometeric and what the pH Eriochromo red T and pH range is 8-10. O Eriochromo black T and pH range is 8- 10.
How mdes of Aee to add to a 100.0mt solwtion of ammonium bromide NHaBr Wayle you need mony 0.200m NHz to obtain a OH of 6:30. ote the Kis of N Hz=18x105. 'Assume uolwne of NH uBr does not affect uolwme of Soution. Solution with a described in D Determine the pA of the buffer a after '6mL of 0.300m HBr is a dded to the solwhion Determine the p4 of the buffer descrbed o part, after4,00mL of 0 300 m NaoH, is added to the solwton:
Paragraph BIEE Table 1: pH readings after addition of NaOH to a buffer solution and water Tabel 1: pH metings na byvoeging van NaOH tot die buffer oplossing en water Volume NaOH added Total Volume NaOH added to Volume NaOH bygevoeg Totale Volume NaOH bygevoeg tot pH measurement/ lesing (mL) (mL) Water Buffer Buffer Water 0. 0. 4.6 6.2 5. 5. 4.8 11.4 10 10 4.9 11.7 15 15 4.9 11.9 10 25 25 5.1 12.0 10 35 35 5.4 12.1 20 55 55 6.2 12.2 Path: p » span » strong O555 WIN
*which of the following are correct of the Procedural Steps: toit □ The PH meter be calibrated before use. 109, 9/ Used solutions, □ A 25.0 ml Sample of vinegar is diluted to 250ml □ Solutions of Known PH; called buffer are to calibrate the pH meter. □PH and volume measurements are collected approximately every 0.2 change in PH. of (spropst pak Ord noi tulo? Not od to smolou thy09 344 7) NO 1917, no 11 SHE 20 ENOT STEF bit OUSIN p 401 gonsloviope pr 5 10 triot Song Lovrops holo) 69 sub of bonp⁹7 2999912 70 70/4 TO
Wed Mar 8 ilibrium arro... Question 3 of 16 > 1 Assignment Score: tan Learning pH = AA 2.3 Assessment - G... Incorrect 31.3% achieve.macmillanlearning.com Chempendix - S... QHow to distingui... Resources Ex Give Up? J If the K₂ of a monoprotic weak acid is 5.9 x 10-6, what is the pH of a 0.21 M solution of this acid? S If the K_a of Feedback
What is the pH of abupfer which has been prepured y miaing 250 my M, cl anel 200 ml, oM Nty soiutiun ? what is the pH of this afHer 10 mmut Hd has been added ? Kb = 1.8 #c0-5 Aas.: ( ५.88, १.०१)
a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to K+CH3CH2COO-. Ka=1.3*10-5; pKa=4.89 b) Calculate the pH of the same solution after adding 0.015M KOH c) Calculate the pH of the same solutions as in part (a) but after addition of 0.015M HBr
ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…
atistics (22111--AB---C.. [References) Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.10 mol NaOH is added, and calculate the pH after 0.22 mol HCl is added to the original solution. Ka = 7.2x10-4 pH = when NaOH is added pH = when HCl is added
Just as pH is the negative logarithm of H3O+], pKa is the negative logarithm of Ka, pKa = – log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH = pK, +log base] [acid] %3D Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid].
I Review I Constants I P III LI IS LILI alivin, ti e connceIILI aliun UI Dase iS KNOWN aliu Can Ue useu LU Caiculale e uiKN Learning Goal: concentration: To calculate the concentration of a solution using moles of base moles of acid concentration of base concentr acid-base titration data. In an acid-base titration an acid (or base) of known concentration is aaded to a base (or acid) of unknown concentration until the number of moles of H and OH are equal, a condition called the equivalence point. Since you know the number of moles of HT (or OH) that you added, you can Part A How many moles of Ba(OH)2 are present in 205 mL of 0.600 M Ba(OH),? Express your answer with the appropriate units. determine the number of moles of OH (or H) in View Available Hint(s) the unknown solution. For example, a solution containing 1 mol of H2 SO4 contains 2 mol of ionizable hydrogen atoms, and would therefore require 2 mol of NaOH for neutralization. A ? M 0.123 Previous Answers Request Answer Submit…
Part B Calculate the percerit lonization of 0.130 M lactic acid in a solution containing 0.0080 M sodium lactate. Express the percent lonization to two significant figures. View Available Hint(s) ΜΕ ΑΣΦΑ Submit ? %