Use the following experimental titration data to calculate the concentration of the acid being analysed.Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade. Observations:The initial solution of acetic acid (HC,H,0,) is clear and colourless. A few drops ofphenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide(concentration 2.50 x 104 mol/L) is used as the titrant. As the mixture reaches the endpoint,flashes of pink colour are seen and the titrant is added drop by drop. The endpoint isreached when one drop of titrant turns the mixture a pale pink colour that does not fade.TrialVolume of acetic acidInitial burette readingFinal burette reading (mL)(HC,H,O,) (mL)(mL)110.000.0024.27210.0024.2748.55310.0048.5572.81

The neutralisation reaction taking place can be written as, => HC2H3O2 + NaOH ------->…

Use the following experimental titration data to calculate the concentration of the acid being analysed. Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.

Use the following experimental titration data to calculate the concentration of the acid being analysed. Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 8P

See similar textbooks

Similar questions

why is it necessary to test the ph? PROCEDURE To a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide.
A 50.0 mL of 3.1% (w/v, g/mL) NaOH solution is mixed with 40.00 mL of 1.2% (w/v, g/mL) Na2CO3 solution. What volume of 0.087 M HCl will be required to titrate the resultant solution to bromocresol green indicator end point (Bcg pH transition range 3.8-5.4, Fwt of NaOH=40 g/mol, Na2CO3= 105.99 g/mol).
Transfer 3-4 drops or a pinch of the test compound (Aniline) to 3 ml of the solvents, 5% NaOH and 5% HCL Shake the mixture thoroughly. The time required for the solute to dissolve in the solvent should not be more than 2 minutes. Indicate with (+) or (-) if the test compound is soluble or insoluble in the solvent. Is Aniline solube or insolube in 5% NaOH? _______ Is Aniline soluble or insolube in 5% HCL? _______
Transfer 3-4 drops or a pinch of the test compound (Acetanilide) to 3 ml of the solvents, 5% NaOH and 5% HCL Shake the mixture thoroughly. The time required for the solute to dissolve in the solvent should not be more than 2 minutes. Indicate with (+) or (-) if the test compound is soluble or insoluble in the solvent. Is Acetanilide solube or insolube in 5% NaOH? _______ Is Acetanilde soluble or insolube in 5% HCL? _______
25.0 cm3 of sodium hydroxide solution is tritrated against 0.200 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.Which of the following pieces of apparatus should be used to transfer 25.0 cm3 of the sodium hydroxide solution?a. Burette b. Pipette c. Measuring cyclinder d. Volumetric flask
Transfer 3-4 drops or a pinch of the test compound (Acetanilide) to 3 ml of the solvents, 5% NaOH and 5% NaHCO3 Shake the mixture thoroughly. The time required for the solute to dissolve in the solvent should not be more than 2 minutes. Indicate with (+) or (-) if the test compound is soluble or insoluble in the solvent. What is the theoretical solubility of Acetanilide in 5% NaOH? _______ What is the theoretical solubility of Acetanilide in 5% NaHCO3? _______
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…
An experiment to observe the effect of ionic strength on the solubility of Ca(OH)2 was conducted. Ca(OH)2 was added to 250 mL 0.01 M KCl, stirred until equilibrium. This was then filtered, and 50 mL of the filtrate was measured out. The 50 mL filtrate was then titrated with standardized 0.13 M HCl solution until phenolphtalein endpoint (11 mL). How do I solve for the solubility s of Ca(OH)2? Please provide an explanation of the process (do I multiply ionic strength μ to the solubility [where s = [Ca(OH)2) = [Ca2+] = 1/2[OH-]?) I would like to know how the diverse ion effect would affect the solubility of Ca(OH)2. How does the ionic strength μ of KCl affect this?
Mr. Clean recently bought a laboratory-grade sodium carbonate from a chemical company known as Brand X. He was supposed to use it in the production of detergents. Unfortunately, he was scammed by the company. He suspected that he purchased a crude sodium carbonate so he tasked the Quality Assurance Department to determine the components of the purchased chemical. The chemist assigned to analyze the sample used double indicator method. For the standardization of HCl titrant, 0.1025 g Na2CO3 of 99.5% purity (FW: 106.00) required 8.20 mL of the titrant to reach the phenolphthalein endpoint. FW: NaOH (40.00), NaHCO3 (84.01), Na2CO3 (106.00) a. What is the molarity of the titrant? The chemist obtained a 3.150 g sample and dissolved it in distilled water to produce a 50.0 mL solution. An aliquot of 10.00 mL was obtained and diluted in a 100.0 mL volumetric flask. A 50.00-mL aliquot of the diluted sample was taken and it required 25.70 mL of titrant for the methyl orange endpoint, while…
A 500ml solution of NaOH was made using 2g of NaOH(s) Three trials of titration were made with using KHP(s) as the acid dissolved with about 25ml of deionized water and 4 drops of phenolphthalein indicator. Slowly adding the NaOH solution until the clear solution had turned pink which would give us our end point and allow us to find the NaOH molarity by equivalence point. Trial 1: - 0.484g of KHP were used - initial volume of buret containing NaOH solution was 0.0 ml - final volume of buret was 23.60ml Trial 2: - 0.485g of KHP were used - initial volume was 0.0ml - final volume was 24.00ml Trial 3: - 0.486g of KHP - initial volume was 0.0ml - final volume was 23.80ml The molarity of NaOH was found by using the moles of KHP(as at equivalence, both solutions are balanced in moles) divided by the total volume of NaOH used to neutralize the solution. Giving us 0.100M for trial 1, 0.099M for trial 2, and 0.100M for trial 3. Make a rough sketch of a titration curve that…
1. Will a 5% preparation of caffeine citrate compounded in citrate buffer, pH 4.8 with no additional co-solvents be a solution – Yes or No? Explain. The MW of caffeine is 194.19 Da and that of caffeine citrate is 386.3 Da. The intrinsic solubility of caffeine is 2.17g/100 mL. please explain the answer.
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5.…