You are asked to determine the alkali present and the percentage of each in a component of a sample material containing components of NaOH, Na,CO, and NaHCO, or mixtures of this together with inert material. Each sample being tested weighs 2g and uses 0.25N hydrochloric acid for neutralization. Sample 1: Using phenolphthalein indicator, 48.64ml acid was used. A duplicate sample needed 97.28ml of acid was used with methyl orange indicator. Sample 2: No color change using phenolphthalein as an indicator but with methyl orange 76.94ml acid is required. Sample 3. To cause a color change, the sample was titrated cold with phenolphthalein, 30.58ml of acid is necessary, and an additional 33.19ml was required for complete neutralization

You are asked to determine the alkali present and the percentage of each in a component of a sample material containing components of NaOH, Na,CO, and NaHCO, or mixtures of this together with inert material. Each sample being tested weighs 2g and uses 0.25N hydrochloric acid for neutralization. Sample 1: Using phenolphthalein indicator, 48.64ml acid was used. A duplicate sample needed 97.28ml of acid was used with methyl orange indicator. Sample 2: No color change using phenolphthalein as an indicator but with methyl orange 76.94ml acid is required. Sample 3. To cause a color change, the sample was titrated cold with phenolphthalein, 30.58ml of acid is necessary, and an additional 33.19ml was required for complete neutralization

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 77QAP: Two students were asked to determine the Kb of an unknown base. They were given a bottle with a...

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ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…
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You are working in a laboratory researching detection methods for components of street drugs. You are asked to classify the molecules as ionizable acid, ionizable base or non-ionizable (neutral) to develop a liquid-liquid extraction protocol. Label each component of the following mixture: v non-ionizable (neutral) v ionizable acid v ionizable basic 1. CH3 НО ОН 2. H 3.
Wed Mar 8 ilibrium arro... Question 3 of 16 > 1 Assignment Score: tan Learning pH = AA 2.3 Assessment - G... Incorrect 31.3% achieve.macmillanlearning.com Chempendix - S... QHow to distingui... Resources Ex Give Up? J If the K₂ of a monoprotic weak acid is 5.9 x 10-6, what is the pH of a 0.21 M solution of this acid? S If the K_a of Feedback
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.