Consider the H2O-NaCl-n-propanol ternary diagram. Given a 70-30 mixture of NaCl-n-propanol titrated with 60-40 H2O-n-propanol, answer the following: a) What are the phases present in the starting analyte? [ Select] [ Select ] water-rich liquid phase, alcohol rich liquid phase, and solid water-rich liquid phase and solid water-rich liquid phase and alcohol rich liquid phase alcohol-rich liquid phase and solid alcohol-rich liquid phase water-rich liguid phase b) What happens at the first endpoint? [Select] c) What happens at the second endpoint? [Select]

Consider the H2O-NaCl-n-propanol ternary diagram. Given a 70-30 mixture of NaCl-n-propanol titrated with 60-40 H2O-n-propanol, answer the following: a) What are the phases present in the starting analyte? [ Select] [ Select ] water-rich liquid phase, alcohol rich liquid phase, and solid water-rich liquid phase and solid water-rich liquid phase and alcohol rich liquid phase alcohol-rich liquid phase and solid alcohol-rich liquid phase water-rich liguid phase b) What happens at the first endpoint? [Select] c) What happens at the second endpoint? [Select]

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 11P

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Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 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
Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH…
The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?
How do i determine the ml of KOH? (Picture posted) A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink
A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink Table 1: Volume of Potassium Hydroxide Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 29.28 36.62 43.98 Initial reading 1.78 9.28 16.62 Volume of KOH used (mL) Average of 2 closest values to within 0.10 mL: Questions Complete Inclosed table Write the molecular equation for the reaction that occurs between potassium hydroxide and hydrobromic acid. Calculate the molar concentration, in mol/L, of the aqueous potassium hydroxide.
please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 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
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