A volume of 100 mL of 1.00 mol L- HCl solution is titrated with 1.00 mol L-NaOH solution. You added the following quantities of 1.00 mol L-' NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point. Drag the appropriate items to their respective bins. » View Available Hint(s) Reset Help 200 mL of 1.00 mol L- NAOH 50.0 mL of 1.00 mol L- NaOH 100 mL of 1.00 mol L- NaOH 150 mL of 1.00 mol L- NaOH 5.00 mL of 1.00 mol L--N2OH|10.0 mL of 1.00 mol L- NaOH Before equivalence point At equivalence point After equivalence point

A volume of 100 mL of 1.00 mol L- HCl solution is titrated with 1.00 mol L-NaOH solution. You added the following quantities of 1.00 mol L-' NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point. Drag the appropriate items to their respective bins. » View Available Hint(s) Reset Help 200 mL of 1.00 mol L- NAOH 50.0 mL of 1.00 mol L- NaOH 100 mL of 1.00 mol L- NaOH 150 mL of 1.00 mol L- NaOH 5.00 mL of 1.00 mol L--N2OH|10.0 mL of 1.00 mol L- NaOH Before equivalence point At equivalence point After equivalence point

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.29QAP

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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: Measured mass of the precipitate 1. Filter paper was dried prior to filtration. EX _____ ET TOPIC: Standardization of Titrant 2. 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) 3. No blank correction EX ______ ET
Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
Calculate the molar solubility of tin(II) hydroxide (Ksp = 5.45x10-27). Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-2).
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: Measured mass of the precipitate Question 4 Overignition which causes the conversion of BaSO4 precipitate to BaO. EX ___ ET Question 5 Precipitate was not washed thoroughly. Ex ___ ET TOPIC: Standardization of Titrant Question 6 Adding insufficient amount of titrant to reach acceptable endpoint color: EX ___ ET
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: Measured mass of the precipitate 1. Overignition which causes the conversion of BaSO4 precipitate to BaO. EX _____ ET2. Precipitate was not washed thoroughly. Ex _____ ET TOPIC: Standardization of Titrant 3.Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX _______ ET
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
ou let your partner do a trial since you're nice. He/she adds a few mL of NaOH, but you realize that nobody recorded the initial buret level! RATS! What do you do? a) Just get light pink since that's the point of titrations anyways. b) Finish the titration and record the final buret reading. Ask your instructor what the initial buret reading was since he knows all of them by heart...right? c) Just record the current level as the "initial" reading. Precision isn't THAT important. d) Restart the trial since you have no idea how much NaOH was added so far.
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.
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