What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators HIn → In- рH range Solution X methyl orange red-yellow 3.2-4.4 yellow methyl red red-yellow 4.8-6.0 yellow bromthymol blue yellow-blue 6.0-7.6 green phenolphthalein colorless-pink 8.2-10.0 colorless O 8.2-10.0 O 6.0 – 7.6 O 4.8 - 6.0 O 3.2 -4.4

What is the approximate pH of a solution X that gives the following responses with the indicators shown? Indicators HIn → In- рH range Solution X methyl orange red-yellow 3.2-4.4 yellow methyl red red-yellow 4.8-6.0 yellow bromthymol blue yellow-blue 6.0-7.6 green phenolphthalein colorless-pink 8.2-10.0 colorless O 8.2-10.0 O 6.0 – 7.6 O 4.8 - 6.0 O 3.2 -4.4

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 2ASA: In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a...

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In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
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In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
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Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Define the term" WEAK ACID"
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