I have contacted Bartleby customer support and they said this question is valid to be asked! They have said if someone denys again, i can contact them back and they will know who has declined and have a talk with them! Dont cause any issues!Use acid-base titration to determine theconcentration of:– A weak acid: CH3COOH0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOHPhenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10 Data• Determine the equivalence point of each acid by using:- pH meter:• HCI – pH=7.00• CH,COOH- Indicator: the point at which the indicator turns "pink"Calculation of the acid concentration:- [acid]=(VNAOH at equivalence mL · 0.100 M)/10 mLCompare to the accepted concentration of the acids:- HCI: 0.100 M- сн,сOон: 0.100 МUse acid-base titration to determine theconcentration of:- A strong acid: HCI0.100 M NAOH (standardized)•0.100 M HCI0.100 M CнзсоонPhenolphthalein is used for endpoint determination- Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10Procedure - Titration of Acid• Ensure that the initial reading of the burette is recorded and that the pH meter is fullysubmerged into the acid solution before continuing.• Add NaOH from the burette to the acid solution in portions (total volume added: 2, 4,6, 7, 7.5, 8, 8.5, 9, 9.2, 9.4, 9.6, 9.8, 10.0, 10.2, 10.4, 10.6, 10.8, 11, 12, 14, 16, 18,20 mL) making sure to write the exact volume added each time and thecorresponding pH when it has stabilized.• Record the initial and final burette volume, the pH, and indicator colour in a table(see below for an example).InitialFinalVolumepHColour ofvolume (* volume(+ 0.05mL)addedindicator0.05 mL)(+ ? mL)2.104.202.10 Apparatus - Burette241025Reading9.63 mlReading24.16 mlTitration ITitration 2Final Reading (ml)9.63 + 0.05 24.16 ± 0.05www.indigo.comInitial Reading (ml)0.00 + 0.050.00 + 0.05Total Volume (ml)9.63 + 0.10 24.16 ± 0.10Acid-Base TitrationStrong Acid-Strong BasePHInitial Burette ReadingFinal Burette ReadingTotal Volume added(mL)(mL)0.00(mL)0.001.890.001.970.002.022.022.092.254.024.022.024.026.026.022.496.028.018.012.978.019.819.813.079.8110.0210.023.203.6510.0210.2110.2110.2110.4610.464.3910.4610.7610.766.0510.7610.9610.9610.7211.6111.8912.0110.9611.9613.8611.9611.9613.8613.8615.9615.9615.9617.8617.8620.0217.8612.1220.02-- ---

Since the given data is of strong acid only, thus concentration of strong acid has been determined.…

Use acid-base titration to determine the concentration of: – A weak acid: CH3COOH 0.100 M NaOH (standardized) •0.100 M HCl 0.100 M CH3COOH Phenolphthalein is used for endpoint determination – Changes from colourless to pink as a solution becomes more basic • Only need 2-3 drops per titration • pH range: 8.3-10

Use acid-base titration to determine the concentration of: – A weak acid: CH3COOH 0.100 M NaOH (standardized) •0.100 M HCl 0.100 M CH3COOH Phenolphthalein is used for endpoint determination – Changes from colourless to pink as a solution becomes more basic • Only need 2-3 drops per titration • pH range: 8.3-10

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.18QAP

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A water sample was analyzed for Fe content using the iron- phenanthroline method. The following data were obtained from the analysis: Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution Concentration of Standard Solution (ppm) Absorbance (au) (mL) 0.50 10.00 0.012 1.00 10.00 0.132 2.00 10.00 0.267 3.00 10.00 0.349 4.00 10.00 0.428 5.00 10.00 0.560 Volume of Unknown Solution Total Volume of Unknown Solution Trial Absorbance (au) (mL) (mL) 1 5.00 10.00 0.289 2 5.00 10.00 0.296 3 5.00 10.00 0.281 Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r²) A m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 B m = 0.1128; b = -4.0 x 10-5; r² = 0.9762 C) m = 0.1128; b = -3.0 x 10-³; r² = 0.9880 D m = 0.1128; b = -3.0 x 10-³; r² = 0.9762
part A:> to Calculate Concentzahion, use M,V, = M2V2 AB1 - 0.025 M X 2.5 ml = ax 5 ml %3D 0.0125 M 0.01 M x 2. S ml= 5°-]x Ŝ ml [s2] = 0.008 M 0. 002 M 11 2 a - X = 0. 01 M Sohtion a 9- X timels) 9-X ABI 0-0125 0-0025 0.01 0. 223 84.8 0.016구 0.0016구 0.015 0.10 구 니1.2 AB 2 0.0 S16 19.5 O.02 0. 00 1 0. 이19 AB 3 0. 0164 0.0816 28.5 0.이구8 0. 0014 AB 니 0. 0022 0.011 구 0.172 60 AB § 0.이139 0.270 95.2 O. ol14 0.0027 0.008구 A8 6 0. 389 14 5.5 0.0096 0.0031 0.0065 AB구
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3. sample of pure CaCO3 (MW 100.09) weighing 0.4148 g is dissolved in 1: 1 hydrochloric acid and the solution is diluted to 500 mL in a volumetric flask. A 50.0 –mL aliquot is withdrawn with a pipet and placed in an Erlenmeyer flask. The solution is titrated with 40.34 mL of an EDTA solution using Erichrome Black T indicator. Calculate the molarity of the EDTA solution.
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2+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 mL portion of the resulting solution was transferred by pipet to a 50 ml volumetric flask and diluted to volume. An analysis showed that the concentration of 2+ Cu* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?
A water sample was analyzed for Fe content using the iron-phenanthroline method. The following data were obtained from the analysis:(photo) Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r2) m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 m = 0.1128; b = - 3.0 x 10-3; r2 = 0.9762 m = 0.1128; b = - 3.0 x 10-3; r2 = 0.9880 m = 0.1128; b = -4.0 x 10-5; r2 = 0.9762