To find 2 (a) and (b): Are you supposed to use the volume of the dilute vinegar to find the conc. of the dilute vinegar? Is the moles of CH3COOH and NaOH, 1:1? 11Sélect ObjectsDraw with TouchAttach your acetic acid titration curves*include a normal and an expanded scale plot*1.Volume of dilute vinegar used:(from procedure)Concentration of standard NaOH: .100OM(from procedure)NaOH equivalence point volume:(clearly marked on your expanded (i.e., zoomed in) graph)2 (a).Calculation of acetic acid concentration in dilute vinegar solution2 (b). Calculation of acetic acid concentration in original vinegar solution Determination of the [CH3COOH] in vinegar by titration adilute vinegar solution against a 0.1000 M NaOH solutionFrom the balanced equation:CH,COOH + NaOH → H20 + Na*CH,CO-& at the Equivalence Point:moles CH,COOH = moles NAOH%3DCalculate the [CH;COOH]

Concentration of vinegar is calculated using law of equivalence.

Attach your acetic acid titration curves *include a normal and an expanded scale plot* 1. Volume of dilute vinegar used: (from procedure) Concentration of standard NaOH: .1t00M (from procedure) NaOH equivalence point volume: 2 (clearly marked on your expanded (i.e., zoomed in) graph) 2 (a). Calculation of acetic acid concentration in dilute vinegar solution 2 (b). Calculation of acetic acid concentration in original vinegar solution

Attach your acetic acid titration curves include a normal and an expanded scale plot 1. Volume of dilute vinegar used: (from procedure) Concentration of standard NaOH: .1t00M (from procedure) NaOH equivalence point volume: 2 (clearly marked on your expanded (i.e., zoomed in) graph) 2 (a). Calculation of acetic acid concentration in dilute vinegar solution 2 (b). Calculation of acetic acid concentration in original vinegar solution

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

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Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration)1. No blank correction Ex _______ET2. Bubbles trapped in the tip of burette: EX ______ ET3. Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX _____ ET
A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ET
4. Are ‘equivalence point’ and ‘end point’ the same? If yes, why? Otherwise, differentiate the two. 5. Aside from repeating the experiment, what can be done to remedy a sample that is ‘over-titrated’.
While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…
Calculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid (HOAc, HC2H3O2) to a phenolphthalein end-point. Report the answer with a precision of two decimal places.
A 4.0520g sample of HCl, specific Gravity 11.18, required 44.15ml of 0.9035M of Sodium Hydroxide in titration, compute for percent purity. Please explain thoroughly. I have an answer of more than 100% concentration and I'm not sure I just want to double check. Thank you and have a great day.
A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055MNaOHsolution using phenolphthalein as theindicator. (a) If 19.60mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? At the end-point, the volume of NaOH consumed was found to be 32.00 mL. The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)
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volumetric or graduated piptte, Which one of them is commonly used for Titration and reagent and which one is more accurate, why?
In the procedure below for a weak diprotic acid titation experiment what are the independent, dependent, and controlled variables? Prepare your Buret• Condition a 50 mL buret (2x with DI H2O followed by 2x standardized NaOH)• Fill the buret with the standardized NaOH close to but not exactly 0.00 mL Prepare Your Analyte • Your analyte will need to be placed in a 250 mL beaker and should contain thefollowing:*0.5 – 0.75 g KHP** About 100 mL DI water* Magnetic stir bar• Once all contents are in the 250 mL beaker, stir for at least 5 minutes to dissolve. Ifneeded, add a bit more water.* For unknown diprotic acids, use the mass provided by the instructorNext Run the Titration (note you will need to run the titration several times for data collection so you are able to use the average molar mass to find the unknown diaprotic acid).
-Are ‘equivalence point’ and ‘end point’ the same? If yes, why? Otherwise, differentiate the two. -Aside from repeating the experiment, what can be done to remedy a sample that is ‘over-titrated’. -If the manufacturer claims 4.5% acid content, what does it mean if you calculated 4.67%