please show the method and answers Consider the titration of 40.0 mL of 0.250 Methanoic acid, CH3COOH, with 0.100 M calciumhydroxide. The Ka of ethanoic acid is 1.8 x 10-5. Complete the following table with theappropriate volumes and pH readings. Report volumes to one decimal place and pH values totwo decimal places. You may ignore the autoprotonation of water. Please clearly show allwork. You may attach additional paper to this sheet as needed.pHVol. Ca(OH)2 (mL)initialmidpointequivalence point0.0 mL60.0 mL

To solve this problem, we need to understand that methanoic acid (also known as formic acid) is a…

Answered: Consider the titration of 40.0 mL of…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

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Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. Group of answer choices 3.22 3.32 4.70 4.80 9.60 9.39
A sample of 50.00 mL of 0.1000 M aqueous solution of chloroacetic acid, CH2ClCOOH (K1= 1.4 × 10-3), is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following stages in the titration, and plot thetitration curve: 0, 5.00, 25.00, 49.00, 49.90, 50.00, 50.10, and 55.00 mL NaOH.
Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA) in the titration, with the following data: HA + NaOH à NaA + H2O. -A pH reading of 3.65 is obtained when 13.0 mL of 0.413 M NaOH is added to the 25.0 mL analyte. -The endpoint of the titration is achieved when 31.25 mL of NaOH have been added. Show all your calculations.
50 mL of benzoic acid (HC7H5O2) 0.1 mol L-1 are titrated with NaOH 0.1 mol L-1. Calculate the pH after addition of 0, 20, 50 and 100 mL of NaOH (Ka = 6.31 x 10-5). Generate the titration curve and choose the best indicator for this procedure.Note: possible answers are 2.60; 3.60; 4.20 and 8.45. Although there are the answers, show the calculations and generate the titration curve.
In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?
Chemistry Questions 17-20 pertain to the titration of 50.00 mL of a solution that is 0.400 M in hydrazoic acid with a solution that is 0.800 M in the strong base lithium hydroxide. The Ka of hydrazoic acid is 2.5 x 10-5. What is the initial solution pH?
Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
Titration is performed on 30 mL of 0.04 M Hydrazine (NH2NH2) (Kb: 2.10-6 ) with 0.02 M HCl in the following volumes . Find the pH values.)(ka:1,4x10-5) (volumes:30 mL ; 45 mL ; 90 mL ; 120 mL; DN)
50.00 mL of benzoic acid (HC7H5O2) 0.1000 mol L-1 are titrated with NaOH 0.1000 mol L-1. Calculate the pH after addition of 0, 20, 50 and 100 mL of NaOH (Ka = 6.31 x 10-5). Generate the titration curve and choose the best indicator for this procedure.Note: possible answers are 2.60; 3.60; 4.20 and 8.45.Although there are the answers, show the calculations and generate the titration curve.
At 25°C, 50.00 mL of a 0.1000 M solution of maleic acid, a diprotic acid whose ionization constants are Ka1 5 1.42 × 10-2 and Ka2 5 8.57 × 10-7 , is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following volumesof added base: 0, 5.00, 25.00, 50.00, 75.00, 99.90, 100.00, and 105.00 mL.
Ka for benzoic acid, c6h5cooh, 6.5x10^-5. Calculate the pH of solution after addition of the followinga. 10.0ml of 0.10 M NaOH to 40.0 mL of 0.10 M Benzoic acidb. 20.0ml of 0.10 M NaOH to 40.0 mL of 0.10 M Benzoic acid
You mix 50.0 mL of 0.250 M CH3COOH with 1.00 mL of 0.500 M NaOH. Calculate the pH of the mixture. The total volume is 51.0 mL. Use two stages method to solve this problem (I. stoichiometric reaction between acid and base, II. Acid-Base Equilibrium, ICE). Ka of CH3COOH = 1.8 x 10-5.

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