This is a Dry Lab since we cannot meet on Campus. You would have first calibrated apH meter and then measured the pH of four different Acid Aqueous Solutions andexamined the data for trends. You would have calculated the expected pH of each ofthe strong acid HCI solutions by assuming that the HCI is 100% ionizedor dissociated when dissolved in water and thus Molarity HCI equals the MolarityH+. Using pH= -log H+ Molarity, the pH of a 1 X 10 to the -4 powerM HCI solution (0.0001 M) is set up as pH= -log(0.0001) = 4. Use the log function ofyour calculator to get the answer.Create a data table like this one and put your calculated HCI pH values in the table.HCI Solution Molarity: 0.1 M0.01 M0.001 MExperimental pH (given) 1.203.08Calculated pHAnswer these questions.1. As the H+ Molarity increases, what happens to the pH ?2.15

pH can be calculated using the given concentration of acid using the formula : pH = - log[H+]

Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.001 M 1.20 3.08 0.01 M Experimental pH (given) Calculated pH Answer these questions. 1. As the H+ Molarity increases, what happens to the pH ? 2.15

Create a data table like this one and put your calculated HCI pH values in the table. HCI Solution Molarity: 0.1 M 0.001 M 1.20 3.08 0.01 M Experimental pH (given) Calculated pH Answer these questions. 1. As the H+ Molarity increases, what happens to the pH ? 2.15

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 116IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...

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In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 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 to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was 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 the pH of the sample.c) Using…
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 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 to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…
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