B. Titration Data A 100 mL Kool-Aid solution was made: 0.3210 g of Kool-Aid powder was quantitatively transferred to 100 mL volumetric flask. The flask was filled to the meniscus to the calibration mark. 1. 2. 10.00 mL aliquots of this solution were used for each titration. The concentration of the sodium hydroxide titrant was 0.02468 M. Three drops of phenolphthalein indicator were used for each titration. 3. Four titrations were performed. The initial and final volumes of the sodium hydroxide solution for each trial are given in Table 1. Table 1. Titration Data Trial 1 Trial 2 Trial 3 Trial 4 Initial NaOH volume 0.24 (mL) Final NaOH volume (mL) NAOH volume used (mL) 17.26 0.13 17.32 17.46 34.50 17.32 34.53

B. Titration Data A 100 mL Kool-Aid solution was made: 0.3210 g of Kool-Aid powder was quantitatively transferred to 100 mL volumetric flask. The flask was filled to the meniscus to the calibration mark. 1. 2. 10.00 mL aliquots of this solution were used for each titration. The concentration of the sodium hydroxide titrant was 0.02468 M. Three drops of phenolphthalein indicator were used for each titration. 3. Four titrations were performed. The initial and final volumes of the sodium hydroxide solution for each trial are given in Table 1. Table 1. Titration Data Trial 1 Trial 2 Trial 3 Trial 4 Initial NaOH volume 0.24 (mL) Final NaOH volume (mL) NAOH volume used (mL) 17.26 0.13 17.32 17.46 34.50 17.32 34.53

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.40QAP

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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
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1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.
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You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an EDTA back titration. CaCO3 has a Ksp of 5x10-9. You add 50.00 mL of 0.3484 M CaCl2 to 500.0ml of sample and filter the solution to remove the precipitate. You then take 250.0 mL of the filtered solution and titrate with 0.1786 M EDTA. You require 23.72 mL to reach the endpoint. What is the concentration of carbonate in the original sample?
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The zinc contained in a 0.7555-g sample of foot powder was titrated with 21.27 mL 0.01645 M EDTA. Find the percent Zn (MM=65.41) in the sample. Answer: 3.029%
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